I need Chemistry help (Connections Unit 6 Lesson 3)
1. A sample of gold (Au) has a mass of 35.12 g.
a. Calculate the number of moles of gold (Au) in the sample and record in
Table 1. Show your work.
b. Calculate the number of atoms of gold (Au) in the sample and record
in Table 1. Show your work.
2. A sample of table sugar (sucrose, C12H22O11) has a mass of 1.202 g.
a. Calculate the number of moles of C12H22O11 contained in the sample
and record in Table 1. Show your work.
Answer:
For 1a: The number of moles of gold are 0.178 moles.
For 1b: There are [tex]1.071\times 10^{23}[/tex] atoms of gold.
For 2: The number of moles of [tex]C_{12}H_{22}O_{11}[/tex] are 0.0035 moles.
Explanation:
To calculate the number of moles, we use the following formula:
[tex]Moles=\frac{\text{Given mass}}{\text{Molar mass}}[/tex] .....(1)
For 1a:We are given:
Given mass of Au = 35.12g
Molar mass of Au = 196.97 g/mol
Putting values in equation 1, we get:
[tex]\text{Moles of Gold}=\frac{35.12g}{196.97g/mol}=0.178moles[/tex]
Hence, the number of moles of gold are 0.178 moles.
For 1b:To calculate the number of atoms in 0.178 moles of gold, we follow mole concept.
According to mole concept:
1 mole of an element contains [tex]6.022\times 10^{23}[/tex] number of atoms.
So, 0.178 moles of gold will contain [tex]0.178\times 6.022\times 10^{23}=1.071\times 10^{23}[/tex] atoms.
Hence, there are [tex]1.071\times 10^{23}[/tex] atoms of gold.
For 2:We are given:
Given mass of [tex]C_{12}H_{22}O_{11}[/tex] = 1.202g
Molar mass of [tex]C_{12}H_{22}O_{11}[/tex] = 342 g/mol
Putting values in equation 1, we get:
[tex]\text{Moles of }C_{12}H_{22}O_{11}=\frac{1.202g}{342g/mol}=0.0035moles[/tex]
Hence, the number of moles of [tex]C_{12}H_{22}O_{11}[/tex] are 0.0035 moles.
The leading cause for dementia is Alzheimer's disease.
True
False
Calculate the external pressure that must be applied to seawater, 1.14 M total ion concentration at 10 degrees C if the maximum concentration allowed in the product water is 176 mg/L. Assume that all the dissolved salts in the product water is sodium chloride.
So, I know that I need to subtract the ion concentrations before using the pi=MRT formula, but I can't figure out how to convert mg/L into molarity. Please help!
Which of the compounds, c3h8, mgcl2, zn(no3)2, ocl2, are expected to exist as molecules?
Explanation:
A molecular compound is a compound in which atoms share electrons with each other and thus, forms covalent bonds. As a result, molecular compounds are covalent compounds.
In the compound [tex]C_{3}H_{8}[/tex], since hydrogen atom has only one electron and carbon atom has 4 electrons in its valence shell. So, in order to completely fill its octet both carbon and hydrogen will share electrons with each other.
Therefore, [tex]C_{3}H_{8}[/tex] is a covalent compound. Hence, it is also a molecular compound.
In [tex]MgCl_{2}[/tex], magnesium being a metal has excess of electrons and chlorine being a non-metal has deficiency of electrons. Thus, magnesium donates its two electrons to both the chlorine atoms and forms an ionic bond.
Hence, [tex]MgCl_{2}[/tex] is an ionic compound. Thus, it is not a molecular compound.
In [tex]OCl_{2}[/tex], both oxygen and chlorine are non-metals. Hence, they have deficiency of electrons. As a result, both oxygen and chlorine will share electrons in order to complete their octet.
So, there will be formation of covalent bonds. Thus, [tex]OCl_{2}[/tex] is a molecular compound.
[tex]Zn(NO_{3})_{2}[/tex] is an inorganic compound and dissolves in water to form ions of [tex]Zn^{2+}[/tex] and [tex]NO^{-}_{3}[/tex]. Hence, [tex]Zn(NO_{3})_{2}[/tex] is an ionic compound.
Thus, we can conclude that out of the given options, [tex]C_{3}H_{8}[/tex] and [tex]OCl_{2}[/tex] exists as molecules.
The oxidation number of hydrogen in sodium hydride (NaH)
In sodium hydride (NaH), the oxidation number of hydrogen is -1, which is an exception to its usual +1 state, as it forms an ionic bond with sodium.
The oxidation number of hydrogen is typically +1, but in compounds known as metal hydrides, such as sodium hydride (NaH), the oxidation number for hydrogen is -1. This is due to hydrogen forming an ionic bond with the metal sodium, resulting in the hydride ion (H-). Since NaH is an ionic compound, we assign sodium (Na) an oxidation number of +1, which is characteristic for metals in Group IA. Consequently, to balance the charge, hydrogen must have an oxidation number of -1 in NaH, making it an exception to the typical +1 oxidation state of hydrogen when covalently bonded to nonmetals.
in the reaction mg(s)+2hcl(aq)→mgcl2(aq)+h2(g) + MgCl2 (aq) how many grams of hydrogen gas will be produced from 125.0 milliliters of a 6.0 M HCI in an excess of Mg
0.756g
Explanation:I am assuming that 6.0MHCl is a typo, and that it should be 6.0molL−1HCl , since that makes sense in the equation.
First we have to find the amount of HCl in the solution. We use the formula n=cV where n is the amount of substance in moles, c is the concentration of the solution in moles per liter, and V is the volume of the substance in liters.
n(HCl)=6.0molL−1×0.125L=0.75mol
Then we find out how many moles of hydrogen gas (H2 ) are produced. In the formula we see 2HCl , and H2 . This means there is 1 mole of H2 for every 2 moles of HCl so to find the amount of H2 we use:
n(H2)=12×0.75mol=0.375mol
Now we find the molar mass of the H2 molecules, by adding together the atomic weights of the constituent molecules. In this case: 1.008+1.008=2.016 . Then we use the formula m=nM where m is the mass of the substance in grams, and M is the molar mass of the substance in grams per mole.
m(H2)=0.375mol×2.016gmol−1=0.756g
turn the word equation into a chemical balanced equation.
Potassium chlorate breaks down into potassium chloride and oxygen gas
What is always true of a weak acid ?
Answer: D. it only partially dissociates in solution.
Explanation:
Strong acid is defined as the acid which completely dissociates when dissolved in water. They have low pH. These releases [tex]H^+[/tex] ions in their aqueous states.
[tex]HNO_3(aq.)\rightarrow H^+(aq.)+NO_3^-(aq.)[/tex]
Weak acid is defined as the acid which does not completely dissociates when dissolved in water. They have high pH. These releases [tex]H^+[/tex] ions in their aqueous states.
[tex]CH_3COOH\rightleftharpoons CH_3COO^-+H^+[/tex]
Thus the correct option is it only partially dissociates in solution.
What is the ph at the half-stoichiometric point for the titration of 0.22 m hno2(aq) with 0.1 m koh(aq)? for hno2, ka = 4.3x10-4?
Answer:- pH = 3.37
Solution:- The balanced equation for the reaction of KOH with [tex]HNO_2[/tex] is written as:
[tex]HNO_2(aq)+KOH(aq)\rightleftharpoons KNO_2(aq)+H_2O(l)[/tex]
Nitrous acid is a weak acid and KOH is a strong base. So, at half-stoichiometric point half of the acid will be neutralized to form its conjugate base and half of the acid will still be remaining.
It means at half stoichiometric point the solution will have equal moles of weak acid(nitrous acid) and its conjugate base(nitrite ion). It will act as a buffer solution and the pH of the buffer solution is calculated by using Handerson equation:
[tex]pH=pKa+log(\frac{base}{acid}) [/tex]
Since, for the half stoichiometric point, [acid] = [base]
The ratio of their concentrations becomes 1 and the log of 1 is 0.
So, pH = pKa
pKa = - log Ka
[tex]pKa=-log(4.3*10^-^4)[/tex]
pKa = 3.37
So, pH = 3.37
Hence, the pH of the solution at half equivalence point will be 3.37.
The pH at the half-stoichiometric point for the titration of 0.22 M HNO₂(aq) with 0.1 M KOH(aq) is 3.4.
Let's consider the equation for the titration of 0.22 M HNO₂(aq) with 0.1 M KOH(aq).
HNO₂(aq) + KOH(aq) ⇒ KNO₂(aq) + H₂O(l)
At the half-stoichiometric point, we have a buffer system formed by equal concentrations of the weak acid (HNO₂) and its conjugate base (NO₂⁻).
We can calculate the pH using the Henderson-Hasselbach's equation.
[tex]pH = pKa+log(\frac{[NO_2^{-} ]}{[HNO_2]} )= pKa+log1=pKa=-log(4.3\times 10^{-4} )=3.4[/tex]
The pH at the half-stoichiometric point for the titration of 0.22 M HNO₂(aq) with 0.1 M KOH(aq) is 3.4.
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A sample of a compound of mercury and bromine with a mass of 0.389 g was found to contain 0.111 g bromine. its molecular mass was found to be 561. what are its empirical and molecular formulas?
The empirical formula of the given compound is [tex]\boxed{{\text{HgBr}}}[/tex].
The molecular formula of the given compound is [tex]\boxed{{\text{H}}{{\text{g}}_2}{\text{B}}{{\text{r}}_2}}[/tex] .
Further explanation:
Empirical formula:
It is atom’s simplest positive integer ratio in compound. It may or may not be same as that of molecular formula. For example, the empirical formula of sulfur dioxide is [tex]{\text{SO}}[/tex] .
Molecular formula:
It is chemical formula that indicates total number and kinds of atoms in molecule. For example, molecular formula of sulfur dioxide is [tex]{\text{S}}{{\text{O}}_2}[/tex] .
Step 1: Mass of mercury (Hg) is to be calculated. This is done by using equation (1).
Since the given compound consists of only mercury and bromine. So the mass of mercury is calculated as follows:
[tex]{\text{Mass of mercury}}\left({{\text{Hg}}}\right)={\text{Mass of compound}} - {\text{Mass of bromine}}\left({{\text{Br}}}\right)[/tex]
…… (1)
The mass of the compound is 0.389 g.
The mass of bromine is 0.111 g.
Substitute the values in equation (1).
[tex]\begin{aligned}{\text{Mass of mercury}}&={\text{0}}{\text{.389 g}} - {\text{0}}{\text{.111 g}}\\&={\text{0}}{\text{.278 g}}\\\end{aligned}[/tex]
Step 2: The moles of mercury and bromine are to be calculated.
The formula to calculate the moles of mercury is as follows:
[tex]{\text{Moles of Hg}} = \frac{{{\text{Given mass of Hg}}}}{{{\text{Molar mass of Hg}}}}[/tex] …… (2)
The given mass of Hg is 0.278 g.
The molar mass of Hg is 200.59 g/mol.
Substitute these values in equation (2).
[tex]\begin{aligned}{\text{Moles of Hg}}&=\left( {{\text{0}}{\text{.278 g}}}\right)\left({\frac{{{\text{1 mol}}}}{{{\text{200}}{\text{.59 g}}}}}\right)\\&=0.0013859\\&\approx{\text{0}}{\text{.001386 mol}}\\\end{gathered}[/tex]
The formula to calculate the moles of bromine is as follows:
[tex]{\text{Moles of Br}} = \frac{{{\text{Given mass of Br}}}}{{{\text{Molar mass of Br}}}}[/tex] …… (3)
The given mass of Br is 0.111 g.
The molar mass of Br is 79.90 g/mol.
Substitute these values in equation (3).
[tex]\begin{aligned}{\text{Moles of Br}}&=\left({{\text{0}}{\text{.111 g}}}\right)\left({\frac{{{\text{1 mol}}}}{{{\text{79}}{\text{.90 g}}}}}\right)\\&= 0.0013892\\&\approx{\text{0}}{\text{.001389 mol}}\\\end{gathered}[/tex]
Step 4: The moles of mercury and bromine are to be written with their corresponding subscripts.
So the preliminary formula becomes,
[tex]{\text{Preliminary formula of the compound}}={\text{H}}{{\text{g}}_{0.001386}}{\text{B}}{{\text{r}}_{0.001389}}[/tex]
Step: Each of the subscripts is divided by the smallest subscript to get the empirical formula.
In this case, the smallest one is 0.001386. So the empirical formula of the compound is written as follows:
[tex]\begin{aligned}{\text{Empirical formula of the compound}}&={\text{H}}{{\text{g}}_{\frac{{0.001386}}{{0.001386}}}}{\text{B}}{{\text{r}}_{\frac{{0.001389}}{{0.001386}}}}\\&={\text{H}}{{\text{g}}_1}{\text{B}}{{\text{r}}_{1.002}}\\&\approx {\text{HgBr}}\\\end{aligned}[/tex]
Therefore the empirical formula of the compound is [tex]{\mathbf{HgBr}}[/tex] .
Step 6: The empirical formula mass of the compound is to be calculated. This is done by using equation (4).
[tex]{\text{Empirical formula mass of HgBr}}=\left( 1 \right)\left({{\text{Atomic mass of Hg}}}\right) + \left(1\right)\left({{\text{Atomic mass of Br}}}\right)[/tex]
…… (4)
Substitute 200.59 g/mol for the atomic mass of Hg and 79.90 g/mol for the atomic mass of Br in equation (4).
[tex]\begin{aligned}{\text{Empirical formula mass of HgBr}}&=\left( 1 \right)\left({{\text{200}}{\text{.59 g/mol}}}\right) + \left( 1 \right)\left( {{\text{79}}{\text{.90 g/mol}}}\right)\\ &= 280.49\;{\text{g/mol}}\\\end{gathered}[/tex]
Step 7: The molar mass of the compound is divided by its empirical formula mass to get a whole number. The formula for this is as follows:
[tex]{\text{Whole - number multiple}} = \frac{{{\text{Molar mass of compound}}}}{{{\text{Empirical formula mass}}}}[/tex] …… (5)
Substitute 560 g/mol for the molar mass of the compound and 280.49 g/mol for the empirical formula mass of the compound in equation (5).
[tex]\begin{aligned}{\text{Whole - number multiple}}& = \frac{{{\text{560 g/mol}}}}{{{\text{280}}{\text{.49 g/mol}}}}\\&= 1.99\\&\approx2\\\end{aligned}[/tex]
Step 8: The empirical formula is multiplied by the whole number multiple to get the molecular formula. So the molecular formula of the compound is [tex]{\mathbf{H}}{{\mathbf{g}}_{\mathbf{2}}}{\mathbf{B}}{{\mathbf{r}}_{\mathbf{2}}}[/tex] .
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Answer details:
Grade: Senior School
Subject: Chemistry
Chapter: Stoichiometry of formulas and equations
Keywords: empirical formula, Hg, Br, HgBr, Hg2Br2, subscript, moles of Br, moles of Hg, mass of Hg, mass of Br, molecular formula, 2, preliminary formula.
which of the following types of molecular representations can be used to show differences between isomers? Explain why each can or cannot.
a) molecular formula
b) structural formula
c) 3D drawing or model,
Molecular formula, structural formula, and 3D drawing or model can be used to show differences between isomers.
Explanation:The types of molecular representations that can be used to show differences between isomers are:
Molecular formula: The molecular formula gives only the number of each kind of atom present in a molecule. It does not provide any information about the structure of the molecule. For example, the molecular formula CH4O represents methanol, but it does not reveal the arrangement of the atoms.Structural formula: The structural formula shows how the atoms are connected in a molecule. It provides information about the arrangement of atoms and the bonds between them. For example, the structural formula of methanol (CH3OH) indicates that one carbon atom is bonded to three hydrogen atoms and one oxygen atom.3D drawing or model: A 3D drawing or model represents the three-dimensional structure of a molecule. It helps in visualizing the spatial arrangement of atoms. For example, a ball-and-stick model or a space-filling model can be used to show the differences in the arrangement of atoms between isomers.Traumatic acid contains 63.13% carbon, 8.830% hydrogen, and 28.03% oxygen. its molar mass is 228 g/mol. determine the empirical and the molecular formulas of traumatic acid.
What volume of a 2.5 M NaOH solution is required to make 1 liter of a 0.75 M NaOH?
0.3 liter
1 liter
33 liters
3.3 liters
0.3 liter of the 2.5 M NaOH solution is required to make 1 liter of a 0.75 M NaOH solution.
Explanation:To find the volume of a NaOH solution needed, we can use the formula:
(M1)(V1) = (M2)(V2)
Where:
M1 is the initial concentration of NaOH (2.5 M)V1 is the initial volume of NaOH (unknown)M2 is the final concentration of NaOH (0.75 M)V2 is the final volume of NaOH (1 L)Plugging in the given values:
(2.5 M)(V1) = (0.75 M)(1 L)
Solving for V1:
V1 = (0.75 M)(1 L) ÷ (2.5 M) = 0.3 L
Therefore, 0.3 liter of the 2.5 M NaOH solution is required to make 1 liter of a 0.75 M NaOH solution.
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"each of two or more forms of the same element that contain equal numbers of protons but different numbers of neutrons in their nuclei" and is radioactive is:
the molar mass of methane is 16.04 g/mol. Calculate the number of moles of methane burned in the ecperiment,
Consider the chemical equation in equilibrium.
CH4(g) + H2O(g) mc029-1.jpg CO(g) + 3H2(g)
What will happen to the equilibrium of this reaction if the pressure is increased?
The equilibrium will shift to the left to favor the reverse reaction.
The equilibrium will shift to the right to favor the forward reaction.
The equilibrium will not be affected by changing the pressure.
The equilibrium will not be reestablished after this kind of stress.
Answer:
The correct answer is :'The equilibrium will shift to the right to favor the forward reaction'.
Explanation:
[tex]CH_4(g) + H_2O(g) \rightleftharpoons CO(g) + 3H2(g)[/tex]
According to Le-Chatlier's principle,When the pressure is increased the equilibrium shifts in the direction where number of moles of gas molecules are greater .
The equilibrium will shift towards the product side because there are more number of moles of gas re greater on product side. So, the equilibrium will shift in the right direction favoring the forward reaction.
Please HELP ASAP HELP Think about the order of planets starting with the one closest to the sun, and moving outward. What two planets can be found on either side of Earth? A) Venus and Mars B) Mercury and Mars C) Venus and Mercury D) Mercury and Jupiter
what is the molar of mass of copper (II) sulfate CuSOu?
Name the type of compound produced by the hydrolysis of a protein.
The hydrolysis of a protein results in the production of amino acids. This procedure involves the breaking of the peptide bonds within the protein using water, resulting in the formation of individual amino acids. Additionally, amino groups are converted into waste products such as urea.
Explanation:Proteins are polymers largely composed of amino acids connected by peptide bonds. In a process known as hydrolysis, these proteins are broken down into smaller components through the introduction of water. As a result, the bonds within the protein molecule are broken, typically resulting in the formation of individual amino acids.
It's important to note that for an amino acid to participate in this breakdown procedure, its amino group must first be removed. Following this, the amino group is usually converted into ammonia. Mammalian organisms, however, convert this ammonia into a more efficient waste product known as urea.
Overall, in the hydrolysis of proteins, the primary compounds produced are amino acids, which may be further metabolized or reformed into other proteins.
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A fluid that vaporizes and condenses inside the tubing of a heat pump is called the.
C3h8 + 5 o2 --> 3 co2 + 4 h2o this is an example of a _______________.
Answer: [tex]C_{3}H_{8} + 5O_{2} \rightarrow 3CO_{2} + 4H_{2}O[/tex] this is an example of a combustion reaction.
Explanation:
A reaction in which a compound reacts with oxygen and results in the formation of carbon dioxide and water is known as combustion reaction.
For example, [tex]C_{3}H_{8} + 5O_{2} \rightarrow 3CO_{2} + 4H_{2}O[/tex] is a combustion reaction.
Also, it is known that combustion reactions are exothermic in nature because heat is released during these reactions.
Which orbital block corresponds to the transition metals in the periodic table?
If you have exactly 2.00 moles each, of two different substances, then which of the following must be true about the two samples? They have the same mass. They have the same weight. They have the same number of particles. Both b and c.
If you have 2.00 moles each of two different substances, then they have the same number of particles.
What are moles?In the International System of Units, Mole is the base unit of the amount of any substance.
If two compounds have the same number of moles, their masses may differ based on the molar masses of the elements.
Both substances have the same number of particles.
Thus, the correct option is B, They have the same number of particles.
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"what is the pressure of a 34.8-l gas sample containing 7.45 mol of gas at 19.9°c? (r = 0.0821 l • atm/(k • mol), 1 atm = 760 torr)"
Answer:
The gas pressure is 5.15 atm
Explanation:
Given:
Volume of gas, V = 34.8 L
Moles of gas, n = 7.45 moles
Temperature, T = 19.9 C
To determine:
Pressure, P of the gas
Explanation:
Based on the ideal gas equation:
[tex]PV = nRT[/tex]
where P = pressure, V = volume, n = moles, T = temperature, R = gas constant
[tex]P = \frac{nRT}{V} \\\\P = \frac{7.45\ moles*0.0821\ Latm/mol-K*(19.9+273)\ K}{34.8\ L} =5.15\ atm[/tex]
Assuming that the density of vinegar is 1.005 g/mL, calculate the molarity of acetic acid in vinegar from your average value for the mass percentage of acetic acid in vinegar. Density of vinegar= 1.005 g/mL Average mass % acetic acid= 5.2%,
To calculate the molarity of acetic acid in vinegar, convert the average mass percentage of acetic acid to grams, then convert grams to moles, and finally divide the moles by the volume in liters. The molarity of acetic acid in vinegar is 0.866 M.
Explanation:To calculate the molarity of acetic acid in vinegar, we need to first convert the average mass percentage of acetic acid to grams. Assuming we have 100g of vinegar, the mass of acetic acid would be 5.2g (5.2% of 100g). Next, we need to convert grams of acetic acid to moles. The molar mass of acetic acid is 60.05 g/mol. Dividing the mass by the molar mass gives us the number of moles. Finally, we can calculate the molarity by dividing the moles by the volume in liters. Since the density of vinegar is given as 1.005 g/mL, we can assume the volume of 100g of vinegar is 100 mL, or 0.1 L.
Step 1: Convert mass percentage to grams: (5.2% x 100g) = 5.2gStep 2: Convert grams to moles: (5.2g / 60.05 g/mol) = 0.0866 molStep 3: Calculate molarity: (0.0866 mol / 0.1 L) = 0.866 MLearn more about Calculating molarity of acetic acid in vinegar here:https://brainly.com/question/32922378
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The molarity of the acetic acid in the vinegar is 0.871 M, calculated by finding the mass of acetic acid in a certain volume of vinegar and then using that to determine the number of moles of acetic acid and thus the molarity.
Explanation:To get the molarity (M) of acetic acid in vinegar, we need to first find the mass of acetic acid in a certain volume of vinegar since molarity (M) is defined as moles of solute/liters of solution. The given data implies that 5.2% of the vinegar's mass is due to acetic acid. Hence, given vinegar's density (1.005 g/mL), in 1000 ml (or 1 liter) of vinegar, mass of vinegar = density * volume = 1.005 g/mL * 1000 mL = 1005 g. Given that 5.2% of this mass is acetic acid, mass of acetic acid is 5.2/100 * 1005 = 52.26g.
The molecular mass of acetic acid (CH3COOH) is approximately 60 g/mol. So, the number of moles of acetic acid = mass of acetic acid / molecular mass = 52.26 g / 60 g/mol = 0.871 moles. Therefore, the molarity (M) = moles of solute/liters of solution = 0.871 moles / 1 L = 0.871 M.
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At 700 K, CCl4 decomposes to carbon and chlorine. The Kp for the decomposition is 0.76. Find the starting pressure of CCl4 at this temperature that will produce a atotal pressure of 1.9atm at equilibrium.
wrapping a hot dish of food in shiny aluminium foil seems to keep the dish warm longer than wrapping it in clear plastic film . aluminium is much better conductor of heat than plastics , so why does it impede the flow of heat so well?
For the balanced equation shown below, how many moles of O2 will react with 0.3020 moles of CO2?
2C2H5OH + 6O2 → 4CO2 + 6H2O
0.151 moles O2
0.201 moles O2
0.302 moles O2
0.453 moles O2
Answer : The number of moles of [tex]O_2[/tex] react will be, 0.453 moles
Solution : Given,
Moles of [tex]CO_2[/tex] = 0.3020 moles
The balanced chemical reaction is,
[tex]2C_2H_5OH+6O_2\rightarrow 4CO_2+6H_2O[/tex]
From the balanced reaction, we conclude that
As, 4 moles of [tex]CO_2[/tex] produces form 6 moles of [tex]O_2[/tex]
So, 0.3020 moles of [tex]CO_2[/tex] produces from [tex]\frac{6}{4}\times 0.3020=0.453moles[/tex] of [tex]O_2[/tex]
Therefore, the number of moles of [tex]O_2[/tex] react will be, 0.453 moles
A chemical weathering process in which polar water molecules surround individual ions
2. The electrolyte in automobile lead storage batteries is a 3.75 M sulfuric acid solution that has a density of 1.230 g/mL. Calculate the mass percent, molality, and mol fraction of the sulfuric acid.
i am so lost dont know how to get the kg of solvent,
To calculate the mass percent, molality, and mole fraction of sulfuric acid in a lead storage battery, you need to perform calculations involving the solution's molarity, density, and the molar mass of H₂SO₄. You must find the mass of the solution, then determine the mass and moles of the solute and solvent.
Explanation:To calculate the mass percent, molality, and mole fraction of sulfuric acid (H₂SO₄) in an automobile lead storage battery with 3.75 M sulfuric acid and a density of 1.230 g/mL, you need to perform several calculations.
Mass Percent.The mass percent of the solution is the mass of the solute (in this case, H₂SO₄) divided by the total mass of the solution multiplied by 100. Based on the volume of the solution and its molarity, you can find the number of moles of H₂SO₄, which helps to calculate mass, as you know the molar mass of H₂SO₄ is 98.079 g/mol.
Molality. Molality is the number of moles of solute per kilogram of solvent (water in this case). To find the molality, you would calculate the number of moles of sulfuric acid based on its molarity and then calculate the mass of the solvent in kilograms. Remember that the density and the volume of the solution can lead you to find the mass of the solution itself, from which you subtract the mass of the solute to get the mass of the solvent.
Mole Fraction.The mole fraction is the ratio of the number of moles of the solute to the total number of moles of all components in the solution. This requires you to know the moles of both the solute and the solvent.