Answer:
16
Explanation:
The number of orbitals can be calculated when energy level is given.
For example:
n = 4
So in 4th energy level number of orbitals are,
n² = 4² = 16
There are 16 orbitals when n=4
One is 4s three are 4P five is 4d and seven are 4f.
while the number of electrons in energy level can be calculated as
2n²
n is energy level.
For n=4
number of electrons are,
2(4)² = 32
German physicist Werner Heisenberg related the uncertainty of an object's position ( Δ x ) (Δx) to the uncertainty in its velocity ( Δ v ) (Δv) Δ x ≥ h 4 π m Δ v Δx≥h4πmΔv where h h is Planck's constant and m m is the mass of the object. The mass of an electron is 9.11 × 10 − 31 kg. 9.11×10−31 kg. What is the uncertainty in the position of an electron moving at 6.00 × 10 6 m/s 6.00×106 m/s with an uncertainty of Δ v = 0.01 × 10 6 m/s ?
Answer:
[tex]5.788\times 10^{-9} m[/tex] is the uncertainty in the position of a moving electron.
Explanation:
Heisenberg's uncertainty principle is given by the equation:
[tex]\Delta x\times m\times \Delta v=\frac{h}{4\pi}[/tex]
The mass of an electron = m
Uncertainty in velocity = Δv
Uncertainty in position = Δx
h = Planck's constant
We are given:
The mass of an electron = m = [tex]9.11\times 10^{-31} kg[/tex]
Uncertainty in velocity = Δv = [tex]0.01 \times 10^6 m/s[/tex]
Uncertainty in position = Δx
[tex]\Delta x=\frac{h}{4\pi \times m\times \Delta v}[/tex]
[tex]=\frac{6.626\times 10^{-34} Js}{4\times 3.14\times 9.11\times 10^{-31} kg\times 0.01 \times 10^6 m/s}[/tex]
[tex]=5.788\times 10^{-9} m[/tex]
[tex]5.788\times 10^{-9} m[/tex] is the uncertainty in the position of a moving electron.
The uncertainty in the position of an electron is equal to [tex]5.76 \times 10^{-9}\; meters[/tex]
Given the following data:
Mass of an electron = [tex]9.11 \times 10^{-31}[/tex] kgUncertainty in velocity = [tex]0.01 \times 10^{6}[/tex] m/sTo find the uncertainty in the position of an electron, we would use Heisenberg's uncertainty principle:
Mathematically, Heisenberg's uncertainty principle of an object is given by the formula:
[tex]\Delta x \times m \times \Delta v = \frac{h}{4\pi }[/tex]
Where:
[tex]\Delta x[/tex] is the uncertainty in position.m is the mass of an object.[tex]\Delta v[/tex] is the uncertainty in velocity.h is Planck constant ([tex]6.626 \times 10^{-34}[/tex]).Making [tex]\Delta x[/tex] the subject of formula, we have:
[tex]\Delta x = \frac{h}{4\pi \times m \times \Delta v}[/tex]
Substituting the given parameters into the formula, we have;
[tex]\Delta x = \frac{6.626 \times 10^{-34}}{4\times \;3.142 \;\times \;9.11 \times 10^{-31}\; \times \;0.01 \;\times 10^{6}}\\\\\Delta x = \frac{6.626 \times 10^{-34}}{1.15 \times 10^{-25}}\\\\\Delta x = 5.76 \times 10^{-9}\; meters[/tex]
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When aluminum is placed in concentrated hydrochloric acid, hydrogen gas is produced. 2 Al ( s ) + 6 HCl ( aq ) ⟶ 2 AlCl 3 ( aq ) + 3 H 2 ( g ) What volume of H 2 ( g ) is produced when 3.60 g Al ( s ) reacts at STP?
When 3.60 g of aluminum reacts with hydrochloric acid at STP, approximately 4.48 liters of hydrogen gas is produced. This is calculated using stoichiometry and the conditions of STP, which state that one mole of any gas occupies 22.4 liters.
Explanation:To calculate the volume of hydrogen gas produced when 3.60 g of Al reacts with hydrochloric acid, stoichiometry and the concept of Standard Temperature and Pressure (STP) can be used. Firstly, we need the molar mass of Al, which is approximately 26.98 g/mol. The number of moles of Al in 3.60 g can be calculated by dividing the mass by the molar mass. This gives us approximately 0.133 mol of Al. From the balanced chemical equation, we know that every 2 moles of Al produces 3 moles of H2, so 0.133 mol of Al would produce approximately 0.200 mol of H2.
As per the conditions of STP (Standard Temperature and Pressure), one mole of any gas occupies a volume of 22.4 liters. Therefore, 0.200 mol of H2 would occupy a volume of 0.200 * 22.4 L, which approximates to 4.48 L. So, when 3.60 g of aluminum reacts with hydrochloric acid under the conditions of STP, roughly 4.48 liters of hydrogen gas would be produced.
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A 100-W lightbulb is placed in a cylinder equipped with a moveable piston. The lightbulb is turned on for 0.020 h, and the assembly expands from an initial volume of 0.90 L to a final volume of 5.88 L against an external pressure of 1.0 atm. calculate work done
Answer: The workdone W = 505J
Explanation:
Applying the pressure-volume relationship
W= - PΔV
Where negative sign indicates the power is being delivered to the surrounding
W = - 1.0atm * ( 5.88 - 0.9)L
= - 1.0atm * (4.98)
W = -4.98 atmL
Converting to Joules
1atmL = 101.325J
-4.98atmL = x joules.
Work done in J = -4.98 * 101.325
W= -505J
Therefore the workdone is -505J
If the volume of wet gas collected over water is 85.0 mL at 20°C and 760 mm Hg , what is the volume of dry gas at STP conditions? (The vapor pressure of water at 20°C is 17.5 mm Hg.) Express your answer with the appropriate units.
Answer: 77.4 mL
Explanation:
Combined gas law is the combination of Boyle's law, Charles's law and Gay-Lussac's law.
The combined gas equation is:
[tex]\frac{P_1V_1}{T_1}=\frac{P_2V_2}{T_2}[/tex]
where,
[tex]P_1[/tex] = initial pressure of dry gas = (760 - 17.5) mmHg= 742.5 mm Hg
[tex]P_2[/tex] = final pressure of dry gas at STP = 760 mm Hg
[tex]V_1[/tex] = initial volume of dry gas = 85.0 mL
[tex]V_2[/tex] = final volume of dry gas at STP = ?
[tex]T_1[/tex] = initial temperature of dry gas = [tex]20^oC=273+20=293K[/tex]
[tex]T_2[/tex] = final temperature of dry gas at STP = [tex]0^oC=273+0=273K[/tex]
Now put all the given values in the above equation, we get the final volume of wet gas at STP
[tex]\frac{742.5mmHg\times 85.0ml}{293K}=\frac{760mmHg\times V_2}{273K}[/tex]
[tex]V_2=77.4mL[/tex]
Volume of dry gas at STP is 77.4 mL.
Brass is made from a combination of copper and zinc. The relative amounts of each element are varied by metalworkers to produce the desired properties. Is brass a compound or a mixture?
Answer:
Mixture
Explanation:
Brass is an alloy. An alloy is a combination of two or more metals that gives rise to another metal to give a more desirable end product metal.
The metals combined are only physically combined. They still retain their individual properties. Although the compositions are varied, it is only varied to produce desired properties and not to alter any chemical combination as in the case of compounds.
It is important to note that there are no chemical combinations between these metals.
The beta oxidation pathway degrades activated fatty acids (acyl-CoA) to acetyl-CoA, which then enters the citric acid cycle. Additional enzymes are required to oxidize unsaturated, odd-chain, long-chain, and branched fatty acids.
Which of the following statements are true?
a.A 14-carbon monounsaturated fatty acid with cis configuration yields more ATP than a 14-carbon saturated fatty acid.
b.Enoyl-CoA isomerase, an enzyme that converts cis double bonds to trans double bonds in fatty acid metabolism, bypasses a step that reduces Q, resulting in a higher ATP yield.
c.Even-chain saturated fatty acids are oxidized to acetyl-CoA in the beta oxidation pathway.
d.Complete catabolism of the three-carbon remnant of a 15-carbon fatty acid requires some citric acid cycle enzymes.
e.Trans double bonds in unsaturated fatty acids are not recognized by beta oxidation enzymes.
f.The final round of beta oxidation for a 13-carbon saturated fatty acid yields acetyl-CoA and propionyl-CoA, a three-carbon fragment.
Final answer:
Enoyl-CoA isomerase bypasses a step that reduces Q, resulting in higher ATP yield. Even-chain saturated fatty acids are oxidized to acetyl-CoA in beta oxidation. Complete catabolism of a 15-carbon fatty acid requires some citric acid cycle enzymes.
Explanation:
Statement b is true. Enoyl-CoA isomerase, an enzyme in fatty acid metabolism, bypasses a step that reduces Q, resulting in higher ATP yield.
Statement c is true. Even-chain saturated fatty acids are oxidized to acetyl-CoA in the beta oxidation pathway.
Statement d is true. Complete catabolism of the three-carbon remnant of a 15-carbon fatty acid requires some citric acid cycle enzymes.
in the reaction a + b -> c the following information applies. at the beginning of the reaction there was 1.0 mol of chemical a and 0.5 mol of chemical c was recovered. what are the limiting reagent, the theoretical yield, and the percent yield for this reaction
By titration, it is found that 81.1 mL of 0.117 M NaOH ( aq ) is needed to neutralize 25.0 mL of HCl ( aq ) . Calculate the concentration of the HCl solution.
Explanation:
mole ratio of base to acid is 1:1 hence same moles of NaOH required to neutralize HCl
According to your textbook, how many of the following are properties of covalent compounds:
a. *Can be gas, liquid or solid at room temperature
b. *Does not conduct electricity
c. *Exist as an extended array of atoms
d. *Involves the sharing of electrons
Answer:
a, b and d are correct.
Explanation:
There are two types of attractive forces in covalent compounds:
The force that holds the atoms together in a molecule (the covalent bond).The force that operates between molecules, called an intermolecular force.Because intermolecular forces are usually quite weak compared with the forces holding atoms together within a molecule, molecules of a covalent compound are not held together tightly. Consequently, covalent compounds are usually gases, liquids, or low-melting solids.
Most covalent compounds aqueous solutions generally do not conduct electricity, because the compounds are nonelectrolytes.
help!! please!! 30 points and i will give brainliest!
Answer:
CaCl2
The charge can be +3 or +2
Explanation:
It takes two atoms of chloride and 1 atom of calcium to make this compound
Answer: chemical formula is CaCl2.
CaCl2------> Ca^2+ + Cl^-1
Explanation:
+2 for calcium ion and -1 for the chlorine ion.
For K2Cr2O7
The oxidation state of chromium=
(+1×2) + 2x + (-2×7) = 0
+2+2x-14= 0
2x= 12
x= 12/2
x=+6.
Therefore, the oxidation number of Chromium, Cr in K2CrO7 is +6
Although coal is a complex mixture of substances, its elemental composition can be approximated by the formula C135H96O9NS. Using this chemical formula, calculate the percentage, by mass, of carbon (C) in coal.
Answer:
85%
Explanation:
Firstly, we will need to calculate the molar mass of the molecule. We simply use the atomic masses of each of the elements. The atomic masses are as follows:
C = 12
H = 1
O = 16
N = 14
S = 1
All units are in a.m.u
The molecular mass is thus:
(135 × 12) + (96 × 1) + (16 × 9) + 14 + 32 = 1906g/mol
The percentage by mass of carbon = (135 × 12)/1906 × 100% = 85%
Final answer:
The percentage by mass of carbon (C) in coal, given the formula C135H96O9NS, is approximately 84.97%.
Explanation:
To calculate the percentage by mass of carbon (C) in coal using the approximate formula C135H96O9NS, we first need to determine the molar mass of the entire compound, and then compare it to the mass of just the carbon atoms within the compound. The atomic masses for C, H, O, N, and S are roughly 12.01 g/mol, 1.008 g/mol, 16.00 g/mol, 14.01 g/mol, and 32.07 g/mol, respectively.
To find the molar mass of C135H96O9NS:
C: 135 atoms × 12.01 g/mol = 1621.35 g/mol
H: 96 atoms × 1.008 g/mol = 96.768 g/mol
O: 9 atoms × 16.00 g/mol = 144.00 g/mol
N: 1 atom × 14.01 g/mol = 14.01 g/mol
S: 1 atom × 32.07 g/mol = 32.07 g/mol
The total molar mass of the coal formula is therefore 1621.35 + 96.768 + 144.00 + 14.01 + 32.07 = 1908.198 g/mol.
To calculate the percentage of carbon in the compound:
Percentage of C = (Mass of C / Molar mass of compound) × 100
Percentage of C = (1621.35 g/mol / 1908.198 g/mol) × 100 ≈ 84.97%
Therefore, the percentage by mass of carbon in coal for this given formula is approximately 84.97%.
Calcium ions, barium ions, and magnesium ions all have two positive charges. What could explain the differences in the way each reacted with a sodium hydroxide solution?
C3.
Tes
Example 8
Name each ionic compound.
CaCl2
AlF3
Co2O3
Solution
Using the names of the ions, this ionic compound is named calcium chloride. It is not calcium(II) chloride because calcium forms only one cation when it forms an ion, and it has a characteristic charge of 2+.
The name of this ionic compound is aluminum fluoride.
We know that cobalt can have more than one possible charge; we just need to determine what it is. Oxide always has a 2− charge, so with three oxide ions, we have a total negative charge of 6−. This means that the two cobalt ions have to contribute 6+, which for two cobalt ions means that each one is 3+. Therefore, the proper name for this ionic compound is cobalt(III) oxide.
Test Yourself
Name each ionic compound.
Sc2O3
AgCl
Answers
scandium oxide
silver chloride
How do you know whether a formula—and by extension, a name—is for a molecular compound or for an ionic compound? Molecular compounds form between nonmetals and nonmetals, while ionic compounds form between metals and nonmetals. The periodic table (Figure 3.2 “A Simple Periodic Table”) can be used to determine which elements are metals and nonmetals.
There also exists a group of ions that contain more than one atom. These are called polyatomic ions. Table 3.7 “Common Polyatomic Ions” lists the formulas, charges, and names of some common polyatomic ions. Only one of them, the ammonium ion, is a cation; the rest are anions. Most of them also contain oxygen atoms, so sometimes they are referred to as oxyanions. Some of them, such as nitrate and nitrite, and sulfate and sulfite, have very similar formulas and names, so care must be taken to get the formulas and names correct. Note that the -ite polyatomic ion has one less oxygen atom in its formula than the -ate ion but with the same ionic charge.
Table 3.7 Common Polyatomic Ions
Name Formula and Charge Name Formula and Charge
ammonium NH4+ hydroxide OH−
acetate C2H3O2−, or CH3COO− nitrate NO3−
bicarbonate (hydrogen carbonate) HCO3− nitrite NO2−
bisulfate (hydrogen sulfate) HSO4− peroxide O22−
carbonate CO32− perchlorate ClO4−
chlorate ClO3− phosphate PO43−
chromate CrO42− sulfate SO42−
cyanide CN− sulfite SO32−
dichromate Cr2O72− triiodide I3−
The naming of ionic compounds that contain polyatomic ions follows the same rules as the naming for other ionic compounds: simply combine the name of the cation and the name of the anion. Do not use numerical prefixes in the name if there is more than one polyatomic ion; the only exception to this is if the name of the ion itself contains a numerical prefix, such as dichromate or triiodide.
Writing the formulas of ionic compounds has one important difference. If more than one polyatomic ion is needed to balance the overall charge in the formula, enclose the formula of the polyatomic ion in parentheses and write the proper numerical subscript to the right and outside the parentheses. Thus, the formula between calcium ions, Ca2+, and nitrate ions, NO3−, is properly written Ca(NO3)2, not CaNO32 or CaN2O6. Use parentheses where required. The name of this ionic compound is simply calcium nitrate. Write the proper formula and give the proper name for each ionic compound formed between the two listed ions. cause the ammonium ion has a 1+ charge and the sulfide ion has a 2− charge, we need two ammonium ions to balance the charge on a single sulfide ion. Enclosing the formula for the ammonium ion in parentheses, we have (NH4)2S. The compound’s name is ammonium sulfide.
Because the ions have the same magnitude of charge, we need only one of each to balance the charges. The formula is AlPO4, and the name of the compound is aluminum phosphate.
Neither charge is an exact multiple of the other, so we have to go to the least common multiple of 6. To get 6+, we need three iron(II) ions, and to get 6−, we need two phosphate ions. The proper formula is Fe3(PO4)2, and the compound’s name is iron(II) phosphate.
Test Yourself
Write the proper formula and give the proper name for e
Answer: check explanation.
Explanation:
The three elements/metals, that is Calcium, Barium and Magnesium all belongs to group 2A on the periodic table. Other elements/metals of group 2A in the periodic table are; Beryllium, Strontium and Radium.
As one go down the group, the atomic radius increases from Magnesium to Barium(this is because of the increase in number of shells of electrons). And, as one go down the group the first ionization energy decreases.Because of this decease in ionization energy it makes it easier for the valence electrons to be removed and thus, REACTIVITY INCREASES DOWN THE GROUP.
Ca^2+ + 2OH^- --------> Ca(OH)2.
Mg^2+ + 2OH^- ---------> Mg(OH)2.
PS: The Na^+ is a spectator ion.
Carbon dating requires that the object being tested contain
Answer:
Organic Material
Explanation:
Carbon Dating is the process in which the age of a piece of organic matter is determined by the proportions of carbon isotopes it contains.
Carbon dating requires that the object being tested contains carbon-14 (14C) isotopes.
Carbon-14 is a radioactive isotope of carbon that is present in the Earth's atmosphere in small amounts. Living organisms, including plants and animals, take in carbon-14 through the process of photosynthesis or by consuming other organisms.
Once an organism dies, it no longer takes in carbon-14, and the concentration of carbon-14 in its remains gradually decreases over time due to radioactive decay.
By measuring the remaining amount of carbon-14 in a sample, scientists can determine the age of an object or organism.
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What is the volume of 1.56 kg of a compound whose molar mass is 81.86 g/mole and whose density is 41.2 g/ml?
Answer:
v = 37.9 ml
Explanation:
Given data:
Mass of compound = 1.56 kg
Density = 41.2 g/ml
Volume of compound = ?
Solution:
First of all we will convert the mass into g.
1.56 ×1000 = 1560 g
Formula:
D=m/v
D= density
m=mass
V=volume
v = m/d
v = 1560 g / 41.2 g/ml
v = 37.9 ml
The volume of the compound is 37.86 mL.
What is volume?Volume is the capacity of an object.
To calculate the volume of the compound, we use the formula below.
Formula:
D = m/v............. Equation 1Where:
D = Density of the compoundm = mass of the compoundv = Volume of the compoundmake v the subject of the equation
v = m/D.............. Equation 2From the question,
Given:
m = 1.56 kg = 1560 gD = 41.2 g/mlSubstitute these values into equation 2
v = 1560/41.2v = 37.86 mL.Hence, the volume of the compound is 37.86 mL.
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The fundamental force underlying all chemical reactions is
Answer:
Electromagnetic Force
Explanation:
Every aspect of chemical reaction is the output of electromagnetic force though the forces can take on many forms because of the quantum wave nature of particles.
The electromagnetic force has the ability to attract opposite charges such as protons and electrons and it repels same charges such as electrons and protons.
This force is an important force in the chemical reaction as it it is responsible for bonding between atoms. Though other forces are unique in their own way but they don't affect chemical reaction. Force of gravity is not strong enough to affect chemical reactions; when nuclear forces are involved in a reaction, such reaction is a nuclear reactor; not chemical reaction.
One of the roles of the electromagnetic force in chemical reaction is that it holds the electrons that are in the outer orbit around the nucleus; this, in the long run creates bonds with other chemical elements to create a visible matter.
The electromagnetic force is the principal force underlying all chemical reactions. It governs the interactions between charged particles in atoms and molecules, leading to the formation and breaking of chemical bonds.
Explanation:The fundamental force underlying all chemical reactions is the electromagnetic force. This force is responsible for the interactions between charged particles which make up atoms and molecules. For example, in a chemical reaction, atoms or molecules rearrange to create new substances. This rearrangement involves the breaking and forming of chemical bonds, which are effectively governed by electromagnetic forces. This is due to the fact that electrons (which are negatively charged) are attracted to the nuclei of atoms (which are positively charged) which encourages them to stay within certain regions of space (creating what we know as chemical bonds).
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Determine the bond order from the molecular electron configurations. ( σ 1 s ) 2 ( σ 1 s * ) 2 ( σ 2 s ) 2 ( σ 2 s * ) 2 ( σ 2 p ) 2 ( π 2 p ) 4 ( π 2 p * ) 2 bond order: ( σ 1 s ) 2 ( σ 1 s * ) 2 ( σ 2 s ) 2 bond order:
Explanation:
The bond order is defined as number of electron pairs present in a bond of the two atoms.
The formula of bond order is given by:
= [tex]\frac{1}{2}\times (\text{Number of bonding electrons}-\text{Number of anti-bonding electrons})[/tex]
1) [tex](\sigma 1 s )^2 ( \sigma 1 s*)^2 (\sigma 2s )^2 ( \sigma 2 s*)^2 ( \sigma 2 p )^2 ( \pi2 p )^4 (\pi 2 p *)^2 [/tex]
Number of bonding electrons = 10
Number of anti-bonding electrons = 6
The bond order : [tex]\frac{1}{2}\times (10-6)=2[/tex]
2) [tex]( \sigma 1 s )^2 ( \sigma 1 s * )^2 ( \sigma 2 s )^2[/tex]
Number of bonding electrons = 4
Number of anti-bonding electrons = 2
The bond order : [tex]\frac{1}{2}\times (4-2)=1[/tex]
The bond order can be determined from the molecular electron configurations by counting the number of bonding and antibonding electrons and calculating the bond order as (number of bonding electrons - number of antibonding electrons)/2.
Explanation:The bond order can be determined from the molecular electron configurations. In this case, the electron configuration given is ( σ 1 s ) 2 ( σ 1 s * ) 2 ( σ 2 s ) 2 ( σ 2 s * ) 2 ( σ 2 p ) 2 ( π 2 p ) 4 ( π 2 p * ) 2. We need to count the number of bonding and antibonding electrons to calculate the bond order. The number of bonding electrons is the sum of the electrons in all the bonding molecular orbitals. In contrast, the number of antibonding electrons is the sum of the electrons in all the antibonding molecular orbitals. The bond order is then calculated as (number of bonding electrons - number of antibonding electrons)/2. In this case, the bond order is (2+2+2+4-2)/2 = 4/2 = 2, indicating a double bond.
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Which tags do not depend on a silicon microchip and use plastic or conductive polymers instead of silicon-based microchips allowing them to be washed or exposed to water without damaging the chip?
Answer: Chipless RFID tags
Acetylene gas, C2H2, can be produced by the reaction of calcium carbide and water. CaC2(s) + 2H2O(l) --> C2H2(g) + Ca(OH)2(aq) How many liters of acetylene at 742 mm Hg and 26C can be produced from 2.54 g CaC2(s)?
Answer:
1.0 L
Explanation:
Given that:-
Mass of [tex]CaC_2[/tex] = [tex]2.54\ g[/tex]
Molar mass of [tex]CaC_2[/tex] = 64.099 g/mol
The formula for the calculation of moles is shown below:
[tex]moles = \frac{Mass\ taken}{Molar\ mass}[/tex]
Thus,
[tex]Moles= \frac{2.54\ g}{64.099\ g/mol}[/tex]
[tex]Moles_{CaC_2}= 0.0396\ mol[/tex]
According to the given reaction:-
[tex]CaC_2_{(s)} + 2H_2O_{(l)}\rightarrow C_2H_2_{(g)} + Ca(OH)_2_{(aq)}[/tex]
1 mole of [tex]CaC_2[/tex] on reaction forms 1 mole of [tex]C_2H_2[/tex]
0.0396 mole of [tex]CaC_2[/tex] on reaction forms 0.0396 mole of [tex]C_2H_2[/tex]
Moles of [tex]C_2H_2[/tex] = 0.0396 moles
Considering ideal gas equation as:-
[tex]PV=nRT[/tex]
where,
P = pressure of the gas = 742 mmHg
V = Volume of the gas = ?
T = Temperature of the gas = [tex]26^oC=[26+273]K=299K[/tex]
R = Gas constant = [tex]62.3637\text{ L.mmHg }mol^{-1}K^{-1}[/tex]
n = number of moles = 0.0396 moles
Putting values in above equation, we get:
[tex]742mmHg\times V=0.0396 mole\times 62.3637\text{ L.mmHg }mol^{-1}K^{-1}\times 299K\\\\V=\frac{0.0396\times 62.3637\times 299}{742}\ L=1.0\ L[/tex]
1.0 L of acetylene can be produced from 2.54 g [tex]CaC_2[/tex].
About 1 liter of acetylene gas can be produced from 2.54 g of calcium carbide under the given conditions of 742 mmHg and 26C.
Explanation:The question requires you to calculate the volume of acetylene gas produced from a known amount of calcium carbide using the given reaction under specified conditions. To answer this, we need to use the principles of stoichiometry combined with the ideal gas law. First, we need to convert the mass of CaC2 to moles because stoichiometry deals with mole ratios. The molar mass of CaC2 is around 64.1 g/mol so 2.54 g of CaC2 is around 0.04 moles. From the balanced equation, we can see that one mole of CaC2 produces one mole of C2H2. Therefore we also have 0.04 moles of acetylene gas produced.
Next, we use the ideal gas law (PV=nRT) to find the volume of acetylene gas produced. Here P is pressure, V is volume, n is the moles of gas, R is the ideal gas constant, and T is temperature. The pressure should be in atmospheres, so we convert 742 mmHg to around 0.97 atm. The temperature should be in kelvin, so we convert 26C to around 299K. The value for R is 0.0821 L·atm/mol·K.
Plugging in our values into the equation gives (0.97 atm x V) = (0.04 mol x 0.0821 L x atm/mol x K x 299K). Solving for V gives approximately 0.983 L or about 1 liter of acetylene gas under these conditions.
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Calculate the percent by mass of the solute in each of the following aqueous solutions: (a) 5.50 g of NaBr in 78.2 g of solution, (b) 31.0 g of KCl in 152 g of water, (c) 4.5 g of toluene in 29 g of benzene.
Answer:
For a: The mass percent of NaBr is 7.03 %
For b: The mass percent of KCl is 16.94 %
For c: The mass percent of toluene is 13.43 %
Explanation:
To calculate the mass percentage of solute in solution, we use the equation:
[tex]\text{Mass percent of solute}=\frac{\text{Mass of solute}}{\text{Mass of solution}}\times 100[/tex] .......(1)
For a:We are given:
Mass of NaBr (Solute) = 5.50 g
Mass of solution = 78.2 g
Putting values in equation 1, we get:
[tex]\text{Mass percent of NaBr}=\frac{5.50g}{78.2g}\times 100\\\\\text{Mass percent of NaBr}=7.03\%[/tex]
Hence, the mass percent of NaBr is 7.03 %
For b:We are given:
Mass of KCl (Solute) = 31.0 g
Mass of water (solvent) = 152 g
Mass of solution = (31.0 + 152) g = 183 g
Putting values in equation 1, we get:
[tex]\text{Mass percent of KCl}=\frac{31.0g}{183g}\times 100\\\\\text{Mass percent of KCl}=16.94\%[/tex]
Hence, the mass percent of KCl is 16.94 %
For c:We are given:
Mass of toluene (Solute) = 4.5 g
Mass of benzene (solvent) = 29 g
Mass of solution = (4.5 + 29) g = 33.5 g
Putting values in equation 1, we get:
[tex]\text{Mass percent of toluene}=\frac{4.5g}{33.5g}\times 100\\\\\text{Mass percent of toluene}=13.43\%[/tex]
Hence, the mass percent of toluene is 13.43 %
To calculate the percent by mass of the solute in each aqueous solution, divide the mass of the solute by the mass of the solution and multiply by 100%
Explanation:To calculate the percent by mass of the solute in each aqueous solution, you'll need to use the formula:
Percent by mass = (mass of solute/mass of solution) x 100%
For example, in solution (a) with 5.50 g of NaBr in 78.2 g of solution, the mass of the solute is 5.50 g and the mass of the solution is 78.2 g. Plugging these values into the formula gives:
Percent by mass = (5.50 g / 78.2 g) x 100% = 7.03%
Similarly, you can calculate the percent by mass for solutions (b) and (c) using the same formula.
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how many grams of silver chromate will precipitate when 150 ml of 0.500 M silver nitrate are added to 100 mL of 0.400 M potassium chromate
When 150 ml of 0.500 M silver nitrate are added to 100 mL of 0.400 M potassium chromate, a silver chromate precipitate forms. Considering the stoichiometry of the reaction and the quantities of reactants, 24.88 grams of silver chromate will precipitate.
Explanation:The subject of this question is based on precipitation reactions in Chemistry. Precipitation reactions occur when two solutions combine to form an insoluble solid known as a precipitate. The moles of silver nitrate present in a 150 mL of 0.500 M solution can be calculated using the formula Molarity = Moles ÷ Volume (in Litres).
Thus, Moles of AgNO3 = 0.500 M * 0.15 L = 0.075 mol AgNO3. According to the reaction equation 2AgNO3 + K2CrO4 → 2AgCrO4(precipitate) + 2KNO3, for every mole of K2CrO4, we have two moles of AgNO3. Thus, based on stoichiometry and the given quantities of the reactants, the limiting reactant will be AgNO3, and it will totally react and form the silver chromate precipitate. The moles of Ag2CrO4 formed would therefore also be 0.075 mol. To convert this into grams, we use the molar mass of Ag2CrO4, which is approximately 331.73 g/mol. Hence, grams of Ag2CrO4 = 0.075 mol Ag2CrO4 * 331.73 g/mol = 24.88 g Ag2CrO4.
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Iron reacts with copper (II) sulfate to produce copper and iron (II) sulfate. If 5.6 moles of iron react, how many molecules of iron (II) sulfate will be produced?
1 Fe + 1 CuSO4 --> 1 Cu + 1 FeSO4
Answer:
The molecules of Fe formed are 3.37 ₓ10²⁴
Explanation:
The reaction is this one:
Fe + CuSO₄ --> Cu + FeSO₄
And the ratio for the reaction is 1:1
If 5.6 moles of iron react, you will have 5.6 moles of FeSO₄. By the way, you should use NA to calculate the number of molecules.
1 mol ____ has ___ 6.02x10²³
5.6 moles _______ (5.6 x 6.02x10²³) = 3.37 ₓ10²⁴
When 1 mol CS2(l) forms from its elements at 1 atm and 25°C, 89.7 kJ of heat is absorbed, and it takes 27.7 kJ to vaporize 1 mol of the liquid. How much heat is absorbed when 1 mol CS2(g) forms from its elements at these conditions
Answer:
There is 117.4 kJ of heat absorbed
Explanation:
Step 1: Data given
Number of moles CS2 = 1 mol
Temperature = 25° = 273 +25 = 298 Kelvin
Heat absorbed = 89.7 kJ
It takes 27.7 kJ to vaporize 1 mol of the liquid
Step 2: Calculate the heat that is absorbed
C(s) + 2S(s) → CS2(l) ΔH = 89.7 kJ (positive since heat is absorbed)
CS2(l) → CS2(g) ΔH = 27.7 kJ (positive since heat is absorbed)
We should balance the equations, before summing, but since they are already balanced, we don't have to change anything.
C(s) + 2S(s)---> CS2 (g)
ΔH = 89.7 + 27.7 = 117.4 kJ
There is 117.4 kJ of heat absorbed
How is the atomic mass of an element calculated from isotope data
Answer:
[tex]aam=\frac{\Sigma m_{i} \times ab_{i} }{100}[/tex]
Explanation:
When an atom has 2 or more isotopes, the average atomic mass (aam) depends on the mass of each isotope (mi) and the percentual abundance in nature of each isotope (abi). The average atomic mass can be calculated using the following expression:
[tex]aam=\frac{\Sigma m_{i} \times ab_{i} }{100}[/tex]
In a 1-L beaker, 213 mL of 0.345 M ammonium chromate was mixed with 107 mL of 0.227 M chromium(III) nitrite to produce ammonium nitrite and chromium(III) chromate. Write the balanced chemical equation for the reaction occurring here. (Use the lowest possible coefficients. Use the pull-down boxes to specify states such as (aq) or (s). If a box is not needed, leave it blank.)
Answer:
3(NH₄)₂CrO₄ (aq) + 2Cr(NO₂)₃ (aq) → 6NH₄NO₂ (aq)+ Cr₂(CrO₄)₃ (aq)
Explanation:
Which process is a chemical reaction? Which process is a chemical reaction? Limescale is formed on the kettle walls Dew condensing on grass during the night Gasoline evaporating from a gasoline tank Lake freezes in winter
Answer:
Limescale formed on kettle walls
Explanation:
A chemical reaction is one which is associated with a chemical change. While the other two examples are mere change in physical state, the formation of limescale on kettle is a chemical change. It is called the furring of kettles.
These limescales are formed when Calcium bicarbonate decomposes into calcium carbonate. It is this calcium carbonate that causes the furring of kettles.
It is one of the consequence of using temporary hard water. Temporarily hard water contains soluble magnesium bicarbonate and calcium bicarbonate. Now the heating of this water causes the decomposition of the calcium bicarbonate into calcium carbonate which forms these scales on the body of the kettle.
Calcium bicarbonate decomposes into calcium carbonate according to the following equation;
CaH(CO3)2 (aq) ---------> CaCO3 (s) + H2O (l) + CO2 (g)
For a sample of acetylene collected over water, total gas pressure is 760 torr and the volume is 459 mL. At the temperature of the gas (23°C), the vapor pressure of water is 21.0 torr. How many grams of acetylene are collected?
Answer:
0.52g
Explanation:
To calculate the mass of acetylene collected, we can calculate the number of moles of acetylene collected and multiply this by the molar mass of acetylene.
To calculate the number of moles of acetylene collected, we can use the ideal gas equation I.e PV = nRT
Rearranging the equation, n =PV/RT
We now identify each of the terms below before substituting and calculating.
n = number of moles, which we are calculating.
R = molar gas constant = 62.64 L.Torr. K^-1. mol^-1
V = volume = 459ml : 1000ml ÷ 1L, hence , 459ml = 459/1000 = 0.459L
T = temperature = 23 degrees Celsius = 273 + 23 = 296K
P = pressure. But since the gas was collected over water, we subtract the vapour pressure of water from the total pressure = 760 - 21 = 739torr
We substitute these values into the equation to yield the following:
n = (739 × 0.459) ÷ ( 62.64 × 300)
n = apprx 0.02 moles
To calculate the mass of acetylene collected, we need the molar mass of acetylene. The molecular formula of acetylene = C2H2, atomic mass of carbon = 12 and atomic mass of hydrogen = 1, thus , the molar mass = 2(12) + 2(1) = 26g/mol
Thus the mass of acetylene collected = 0.02 mole × 26g/mol = 0.52g
The visible spectrum for a colored solution has a maximum absorbances around both 440 nm and around 600 nm and a minimum absorbance between 510 and 540 nm. What is the color of the solution?
Answer:
Green
Explanation:
In the visible spectrum, which ranges from around 400-700 nm wavelength, the lower wavelength corresponds to the violet side of rainbow spectrum and, high wavelength corresponds to red side. As our solution absorbs highly at around 440 and 600 nm, it means that violet side and red side of the spectrum should be absorbed and would not be visible. the lowest absorbance at around 520 nm corresponds to green color, and therefore, it should be the colour visible from the solution
The solution would appear yellow-green in color due to the maximum and minimum absorbances observed in the visible spectrum.
Explanation:The solution would appear yellow-green in color. The visible spectrum ranges from approximately 400 nm (violet) to 750 nm (red) with different colors corresponding to specific wavelengths. In this case, the maximum absorbances around 440 nm and 600 nm, and the minimum absorbance between 510 and 540 nm would indicate that the solution primarily absorbs light in the blue and red regions, resulting in the complementary color of yellow-green being observed.
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The flavor of anise is due to anethole, a compound with the molecular forumal C10H12O. Combustion of one mole of anethole produces 5541 kJ of thermal energy. If 0.950 g of anethole is combusted in a bomb calorimeter whose heat capacity (Ccalorimeter) is 7.854 kJ/°C, what is the change in temperature of the calorimeter?
Final answer:
The change in temperature of the calorimeter upon combusting 0.950 grams of anethole is approximately 24.90°C. This is calculated using the energy released in the combustion and the calorimeter's heat capacity.
Explanation:
The change in temperature of the calorimeter can be calculated using the relationship between the heat capacity of the calorimeter and the amount of heat released during combustion of the substance. Given the combustion of anethole releases 5541 kJ per mole, we first need to determine the amount of energy released during the combustion of 0.950 grams of anethole. Since the molecular weight of anethole (C10H12O) is approximately 148.2 g/mol, we can calculate q (the heat released) for the given mass, and then use this to determine the change in temperature (ΔT).
To calculate the energy released:
q = (0.950 g / 148.2 g/mol) * 5541 kJ/molq = 0.0353 mol * 5541 kJ/mol = 195.59 kJThen, using the calorimeter's heat capacity:
ΔT = q / CcalorimeterΔT = 195.59 kJ / 7.854 kJ/°C ≈ 24.90°CHence, the change in temperature of the calorimeter is approximately 24.90°C.
The principal source of the difference in the normal boiling points of ICI (97°C; molecular mass 162 amu) and Br2(59°C; molecular mass 160 amu) is:a. ICI has greater strength of hydrogen bonding than Br2 b. ICI has stronger dipole-dipole interactions than Br2c. ICI has stronger dispersion forces than Br2 d. The I-CI bond in ICl is stronger than the Br-Br bond in Br2 e. ICI has a greater molecular mass than Br2
Answer:
Option b
Explanation:
The difference in the boiling points of ICl and Br2 is mainly due to the dipole-dipole interactions present between iodine and chlorine in the ICl molecule because as there is difference in electronegativity between iodine and chlorine these type of forces arise
As the dipole-dipole interactions are stronger, the stronger will be the boiling point of that compound because the forces between the molecules increases and as a result the boiling point of the compound increases
In case of Br2 as both are bromine atoms there will be no difference in electronegativity and therefore these type of interactions are not present
Molecular mass can also be a explanation for difference in normal boiling points because more molecular mass means more will be the vander waals forces but as dipole interactions are stronger than vander waals forces the major factor will be due to dipole interactions
The principal source of difference in the normal boiling points of ICI and Br2 is that ICI has stronger dipole-dipole interactions. Although both have similar London dispersion forces due to similar molecular masses, ICI being a polar molecule exhibits stronger dipole-dipole attractions, requiring more energy to overcome and hence has a higher boiling point.
Explanation:The principal source of difference in the normal boiling points of ICI (97°C; molecular mass 162 amu) and Br2(59°C; molecular mass 160 amu) is that ICI has stronger dipole-dipole interactions than Br2. Both ICI and Br2 have similar masses and therefore experience similar London dispersion forces. However, compared to Br2 which is nonpolar, ICI is a polar molecule and thus also exhibits dipole-dipole attractions. These dipole-dipole attractions in ICI are stronger and require more energy to overcome, resulting in a higher boiling point for ICI.
Larger and heavier atoms and molecules like ICI exhibit stronger dispersion forces, leading to higher melting and boiling points. However, in the case of ICI and Br2, the effect of polar dipole-dipole attraction in ICI is more significant. This is apparent when we compare substances with similar molecular masses - the substance with the polar molecules has a higher boiling point, due to the stronger dipole-dipole attractions.
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Calculate the temperature change in the water upon the complete melting of the ice. Assume that all of the energy required to melt the ice comes from the water. Express your answer in terms of the initial temperature of water, T. Calculate the temperature change in the water upon the complete melting of the ice. Assume that all of the energy required to melt the ice comes from the water. Express your answer in terms of the initial temperature of water, . -0.031 T - 2.5 ∘C -2.5 T + 0.031 ∘C 0.031 T - 2.5 ∘C 2.5 T - 0.031 ∘C
Answer:
See explanation below
Explanation:
First, you are not providing any data about the mass of ice and the innitial temperature of water, so, I'm gonna use data from a similar exercise, so in order for you to get the accurate and correct answer, just replace the data in this procedure, and you should be fine.
Now, For this exercise, I will assume we have an 8 g ice cube pounded into 230 g of water. The expression to use here is the following:
q = m*Cp*ΔT (1)
Solving for ΔT:
ΔT = q / m*Cp (2)
Where:
q: heat of the water
m: mass of water
Cp: specific heat of water which is 4.18 J /g °C
Now, we don't know the heat emmited by water, we need to calculate that. To do this, we have data for ice and water, so, let's find first the heat absorbed by the melting ice, and then, the water.
Converting the grams into moles, using the molar mass of water which is 18 g/mol rounded:
moles of ice = 8 g / 18 g/mol = 0.44 moles of water
Now, we'll use the molar heat of fusion of water to convert the moles to kJ:
qi = 0.44 mol * 6.02 kJ/mol =¨2.6488 kJ
Now, as the ice is the system and water the surroundings, the melting of ice in endothermic therefore the heat of water should be the same of ice but negative, therefore:
qi = -qw = -2.6488 kJ or -2648.8 J
Finally, replace this value in equation (2) to get the temperature change:
ΔT = -2648.8 / (230 * 4.18)
ΔT = -2.75 °C
Now, use your data of ice and water and replace them here in this procedure to get the correct and accurate answer.