A gas sample containing 1.45 mol at 25°C exerts a pressure of 408 torr. Some gas is added to the same container, and the temperature is increased to 50.°C. If the pressure increases to 800. torr, how many moles of gas were added to the container? Assume a constant-volume container.

Answer: Temperature is a measure of the kinetic energy of particles in a substance. As temperature increases, the atoms or molecules in a substance gain energy. As temperature decreases, the particles lose energy. A change in the energy of particles causes a change in their arrangement. A change in the arrangement of particles can lead to a physical change.

Explanation:

Answer:

Im 90% sure its 3.

Explanation:

Answer:

4

Explanation:

Answer : The final volume at STP is, 1000 L

Explanation :

According to the Boyle's, law, the pressure of the gas is inversely proportional to the volume of gas at constant temperature and moles of gas.

[tex]P\propto \frac{1}{V}[/tex]

or,

[tex]P_1V_1=P_2V_2[/tex]

where,

[tex]P_1[/tex] = initial pressure = 1520 mmHg = 2 atm    (1 atm = 760 mmHg)

[tex]P_2[/tex] = final pressure at STP = 1 atm

[tex]V_1[/tex] = initial volume = 500.0 L

[tex]V_2[/tex] = final volume at STP = ?

Now put all the given values in the above formula, we get:

[tex]2atm\times 500.0L=1atm\times V_2[/tex]

[tex]V_2=1000L[/tex]

Therefore, the final volume at STP is, 1000 L

The volume of the gas at STP is [tex]\(1000.0 \, \text{L}\)[/tex].

1. Convert initial pressure to atm:

  [tex]\[ P_1 = \frac{1520 \, \text{mm Hg}}{760 \, \text{mm Hg/atm}} = 2 \, \text{atm} \][/tex]

2. Apply the Combined Gas Law:

  [tex]\[ \frac{P_1 \cdot V_1}{T_1} = \frac{P_2 \cdot V_2}{T_2} \][/tex]

  Given:

  [tex]\[ V_1 = 500.0 \, \text{L} \][/tex]

  [tex]\[ P_1 = 2 \, \text{atm} \][/tex]

  [tex]\[ P_2 = 1 \, \text{atm} \][/tex]

  [tex]\[ T_1 = T_2 \][/tex] (temperature does not change)

  Substituting the values, we get:

  [tex]\[ \frac{(2 \, \text{atm} \cdot 500.0 \, \text{L})}{T} = \frac{(1 \, \text{atm} \cdot V_2)}{T} \][/tex]

3. Solve for [tex]\(V_2\)[/tex]:

  Cross-multiply and solve for [tex]\(V_2\)[/tex]:

  [tex]\[ 2 \cdot 500.0 = 1 \cdot V_2 \][/tex]

  [tex]\[ V_2 = \frac{2 \cdot 500.0}{1} \][/tex]

  [tex]\[ V_2 = 1000.0 \, \text{L} \][/tex]

OPTION A. A) Both gases have the same average kinetic energy.

In the given gas mixture of Neon (Ne) and Xenon (Xe) at Standard Temperature and Pressure (STP), both gases only share the same average kinetic energy. However, they do not contribute equally to the mixture's density, they do not share the same molecular speed, and the total volume of the mixture is not 22.4L.

The TRUE statement among the options given is A) Both gases have the same average kinetic energy. The average kinetic energy of gas molecules is determined by temperature, not the type of gas, according to kinetic molecular theory. Therefore, since both gases are at the same temperature (Standard Temperature and Pressure, STP), they will have the same average kinetic energy.

B) is incorrect since each gas contributes to the mixture's density based on its own molar mass, and Xenon's molar mass is much greater than Neon's.

Option C is not correct because molecular speed is influenced by molar mass. Neon, having a smaller molar mass, will have a higher average speed than Xenon.

Statement D) is incorrect because according to Avogadro's law, one mole of any gas at STP occupies a volume of 22.4L, and we have a total of 16 moles of gas (8.0 mol of Ne and 8.0 mol of Xe) which will occupy a volume of 16 times 22.4L.

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Answer: lithium + oxygen Right arrow. lithium oxide

lithium + oxygen proper arrow. lithium oxide This equation indicates lithium oxide is formed from the reaction between oxygen and lithium.

Lithium oxide is used as a flux in ceramic glazes and creates blues with copper and pinks with cobalt. Lithium oxide reacts with water and steam, forming lithium hydroxide, and needs to be isolated from them.

Lithium Oxide is an extraordinarily insoluble thermally stable Lithium source suitable for glass, optic, and ceramic programs. Lithium oxide is a white stable also referred to as lithia, it is produced whilst lithium metallic burns inside the presence of oxygen.

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In the periodic table, Francium has the largest atomic size, Chlorine has the highest electron affinity, Barium has the lowest ionization enthalpy in Group II, and gaseous elements at room temperature include noble gases and some non-metals like Fluorine and Oxygen.

The periodic table organizes elements in such a way that we can predict their properties based on their position. These properties, including atomic size, electron affinity, and ionization enthalpy, show clear patterns or trends within the table. As a tutor from the Brainly platform, let's address the specific properties asked in the question.

You purchase several rolls of fiberglass insulation and pay extra for installation. This is a service.

The majority of homes include fibreglass, an insulation substance made of incredibly thin glass fibres. It is frequently used in two forms of insulation: loose-fill and batts and rolls. Additionally, rigid boards or duct insulation are both options.

In accordance with the U.S. Department of Energy, manufacturers already make medium- and high-density fibreglass batt insulation materials with a little better R-Value than regular batts. Unfinished floors, ceilings, and walls can all be filled with fibreglass. It is set in place between beams, joists, and studs. You purchase several rolls of fiberglass insulation and pay extra for installation. This is a service.

Therefore, fiberglass insulation is a service.

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Answer:

testing

Explanation:

some scientist somewhere made acid and probably forgot the recipe/ingredients so they kept making it and used plastic to see if it would melt it

Answer:

2.4 L

Explanation:

Given data:

Mass of LiF = 19.6 g

Molarity of solution = 0.320 M

Volume of water used = ?

Solution:

Number of moles = mass/molar mass

Number of moles = 19.6 g/ 26 g/mol

Number of moles = 0.75 mol

Volume required:

Molarity = number of moles/ volume in L

0.320 M = 0.75 mol /  volume in L

Volume in L = 0.75 mol  /0.320 M

      M = mol/L

Volume in L = 2.4 L

Answer:

7.

Explanation:

A neutral solution has a pH=7.

A basic solution has a pH>7.

An acidic solution has a pH<7.

Answer:

7,7,7

Explanation:

Answer:

3. 3:2

Explanation:

in the reactants, 3 is the coefficient for the hydrogen atoms.

In the products, 2 is the coefficient for the ammonia atoms.

Answer:

I got .146 g of water

Explanation:

Refer to this equation:

Q= mcΔt

Q= .545 J

c= 4.186 J/g

Δt= .892

plug in values:

.545 J = m(4.186 J/g)(.892°C)

simplify:

.545 J = m(3.734 J/g°C)

.146 g

Answer:

The answer to your question is 0.41 moles

Explanation:

Data

moles of NaCl = ?

mass of NaCl = 24 g

Process

To solve this problem just calculate the molar mass of NaCl, and remember that the molar mass of any substance equals to 1 mol.

1.- Calculate the molar mass

NaCl = 23 + 35.5 = 58.5 g

2.- Use proportions and cross multiplication

               58.5 g of NaCl ------------------- 1 mol

               24.0 g               ------------------- x

                     x = (24 x 1) / 58.5

                     x = 0.41 moles

92.8 % is the percent yield when 2.87 g of aluminum are reacted with excess copper (II) sulfate and 9.2 g of copper are produced.

Explanation:

Mass of aluminum = 2.87 grams

mass of copper produced = 9.2 grams ( actual yield)

the balanced chemical reaction is given as:

2 Al + 3 CuSO4 ⇒ ( AL2(SO4)3 +3 Cu.

from the reaction it is found that

2 moles of aluminum reacted to give 3 moles of copper

so converting them in to mass.

number of moles of copper in 2.8 grams = [tex]\frac{2.8}{63.4}[/tex]

number of moles = 0.104 moles of copper

atomic mass of aluminum = 26.98 grams/mole

atomic mass of copper = 63.54 grams/mole

From the given data

2.87 grams Al gives 9.2 grams of Cu.

2 moles of aluminum reacted to give 3 moles of copper

0.104 moles of aluminum will give

[tex]\frac{3}{2}[/tex] =[tex]\frac{x}{0.104}[/tex]

2x = 0.132

x = 0.156 moles of Cu will be formed.

Hence theoretical yield should be  = 0.156 x 63.54

                                                           = 9.91 grams

Percent yield = [tex]\frac{actual yield}{theoretical yield}[/tex] x 100

                      = [tex]\frac{9.2}{9.91}[/tex] x 100

  percent yield = 92.8 % is the yield percent.

Answer:

i think its 1 liter of oxygen , a gas

Final answer:

One liter of oxygen gas is the most compressible among the options given, due to the significant spaces between gas molecules allowing for easier compression.

Explanation:

When considering the compressibility of various substances at room temperature, gases such as oxygen are the most compressible due to the large spaces between their molecules. In comparison, liquids like water and mercury are less compressible because their molecules are closer together, but they still offer some degree of compressibility. Solids like iron, however, are much less compressible because their atoms are tightly packed in a lattice structure. Of the options provided, one liter of oxygen gas would be the most compressible, as the spacing between gas molecules allows them to be pushed closer together far more easily than molecules in a liquid or atoms in a solid.

Answer:

The greater the change in free energy (ΔG0′), and the greater the energy released

Explanation:

Recall that the change in free energy is given by:

∆G°'= nFE°'

But E° is given by E°acceptor - E°donor

Hence the greater the difference between E°acceptor and E°donor, the greater the value of E° and consequently the greater the value of ∆G° and the energy released.

Note: E°acceptor and E°donor refer to reduction potentials of donor and acceptor

Answer:

6.58 atm total

3.29 atm NO2

3.29 atm O2

Explanation:

Balanced equation:

O3 + NO → NO2 + O2

There are equal numbers of moles of both reactants, so neither is in excess and either could be considered the limiting reactant.

( 1.30 mol NO) x (1 mol NO2 / 1 mol NO) =  1.30 mol NO2

( 1.30 mol NO) x (1 mol O2 / 1 mol NO) =  1.30 mol O2

Total pressure by using the formula;

P = nRT / V

= ( 1.30 mol +  1.30 mol) x (0.08205746 L atm/K mol) x (401.0 K) / (13.0 L)  

= 6.58 atm

Partial pressure for NO2;

(6.58 atm) x (1.30 mol NO2) / (1.30 mol + 1.30 mol)

= 3.29 atm NO2

Partial pressure for O2

6.58 atm total - 3.29 atm NO2

= 3.29 atm O2

1. The partial pressure of nitrogen dioxide ([tex]NO_2[/tex]) is equal to 3.29 atm.

2. The partial pressure of oxygen gas ([tex]O_2[/tex]) is equal to 3.29 atm.

3. The total pressure in the flask at the end of the chemical reaction is 6.58 atm.

Given the following data:

Scientific data:

To determine the partial pressure of each product and the total pressure in the flask at the end of the chemical reaction:

First of all, we would write a balanced chemical equation for the chemical reaction as follows:

                                  [tex]O_3 + NO \rightarrow NO_2+O_2[/tex]

Since the numbers of moles of reactants are equal, the total number of moles of products is:

[tex]n=1.3+1.3[/tex]

n = 2.6 moles

Now, we can find the total pressure in the flask at the end of the chemical reaction by using the ideal gas law equation;

[tex]PV=n RT[/tex]

Where;

Making P the subject of formula, we have;

[tex]P=\frac{nRT}{V}[/tex]

Substituting the parameters into the formula, we have;

[tex]P=\frac{2.6 \times 0.0821 \times 401}{13}\\\\P=\frac{85.597}{13}[/tex]

Total pressure, P = 6.58 atm.

Next, we would determine the partial pressure of each product:

[tex]Molefraction \;of \;a \;substance =\frac{No.\; of \; moles \;of \;substance}{Total \;no. \;of \; moles \;of \;substances}[/tex]

[tex]Molefraction \;of \;a \;substance =\frac{1.3}{2.6} \\\\Molefraction \;of \;a \;substance =0.5[/tex]

For [tex]NO_2[/tex]:

[tex]Partial \;pressure = Molefraction \times Total\;pressure\\\\Partial \;pressure = 0.5 \times 6.58[/tex]

Partial pressure of [tex]NO_2[/tex] = 3.29 atm.

For [tex]O_2[/tex]:

[tex]Partial \;pressure = Molefraction \times Total\;pressure\\\\Partial \;pressure = 0.5 \times 6.58[/tex]

Partial pressure of [tex]O_2[/tex] = 3.29 atm.

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Answer:

B. Single Replacement

Explanation:

Single replacement:

It is the reaction in which one elements replace the other element in compound.

AB + C → AC + B

Chemical equation:

2HgO + Cl₂ → HgCl + O₂

This is the single replacement reaction. In this reaction chlorine replace the oxygen from mercury oxide and form mercury chloride.

Other options are incorrect because,

Decomposition reaction:

It is the reaction in which one reactant is break down into two or more product.

AB → A + B

Synthesis reaction:

It is the reaction in which two or more simple substance react to give one or more complex product.

A + B → AB

Double replacement:

It is the reaction in which two compound exchange their ions and form new compounds.

AB + CD → AC +BD

Answer:

[tex]M=741\times (0.5)^{\frac{t}{5730}}[/tex]

Explanation:

by using well known formula for disintegration

[tex]M=M_0\times (0.5)^{\frac{t}{T}}[/tex]

Final answer:

To calculate the original mass of carbon-14 in an artifact aged 10,670 years, given it now contains 8.4 × 10⁽⁻⁹⁾ grams of carbon-14, we use the half-life of carbon-14 (5,730 years) and the formula for exponential decay. The original mass is found to be 33.6 × 10⁽⁻⁹⁾ grams.

Explanation:

The subject of the question involves using exponential decay to calculate the original mass of carbon-14 in an archaeological artifact, taking into account the half-life of carbon-14, which is 5,730 years. Given that a sample now contains 8.4 × 10-9 grams of carbon-14 and its age is 10,670 years, we can calculate the original amount of carbon-14 it contained. To find the original mass of carbon-14, we can use the formula for exponential decay, M = M0(1/2)t/T, where M is the final mass, M0 is the original mass, t is the time elapsed, and T is the half-life of the substance.

Since 10,670 years is exactly two half-lives of carbon-14 (2 × 5,730), we can calculate that the artifact originally contained 8.4 × 10-9 grams × 22 = 33.6 × 10-9 grams of carbon-14.

Answer:

volume of solution L =0.54 L

Explanation:

Given data:

Molarity of NaCl solution = 3.70 M

Mass of NaCl = 118 g

Solution:

First of all we will calculate the number of moles.

Number of moles = mass/ molar mass

Number of moles = 118 g/ 58.5 g

Number of moles = 2 mol

Now we will calculate the volume from molarity formula:

Molarity = number of moles / volume of solution L

3.70 M = 2 mol / volume of solution L

volume of solution L = 2 mol / 3.70 M

volume of solution L =0.54 L

Answer: The Answer is B. X: Sodium, Y: Potassium

Explanation: No Explanation I just Guessed. Hope This Help's Someone

Answer:

The answer is

X:Sodium Y:Potassium

Explanation:

I took the course and got it right

Answer:

5.03 moles

Explanation:

Find the molar mass of C5H12 and you will get 72.17 g/mol

Next to find the number of moles, you divide 362.8 by the molar mass and you get

(362.8 g)/(72.17 g/mol)= 5.03 moles

2 . The ratio of 1:2 in the mass of second element, oxygen in CO and CO2 verifies the law of proportion.

3. [tex]C_{15}[/tex][tex]H_{24}[/tex][tex]O_{5}[/tex]  is the molecular formula of the new malaria drug given.

Explanation:

Balanced chemical reaction:

C + O ⇒   C0

C + O2  ⇒  CO2

law of multiple formulation states that when two elements combine to form a compound the ratio of the mass of elements is a whole number.

Carbon reacts with oxygen to produce:

         Mass of carbon      mass of oxygen          ratio of O in CO2 to O in CO

CO =    12                                16                                      3:4

CO2 = 12                                 32                                     3:8

 CO    6 gm                              8                                     3:4

  CO2   6                                 16                                    3:8

The ratio of the mass of  the second element i.e oxygen is CO:CO2 is 1:2, hence it shows law of multiple proportions.      

3. given,

 (C5H8)nO5 = emperical formula

relative molecular mass = 284

molecular formula= ?  

The value of n will be calculated as:

(12x5)+ (1x8)n + (16x5) = 284

(60 +8)n  + 80 = 284

68n + 80 = 284

68n = 284 - 80

68n = 204

  n = 3

Multiplying the emperical formula by n

(C5H8)3O5

[tex]C_{15}[/tex][tex]H_{24}[/tex][tex]O_{5}[/tex] is the molecular formula of the drug.

The formation of different carbon oxide compounds with differing masses of oxygen that combine with a fixed mass of carbon demonstrates the law of multiple proportions with a small whole number ratio. To find the molecular formula of Alaxin, the relative molecular mass is divided by the mass of its empirical formula, yielding a molecular formula of C10H16O10.

The law of multiple proportions states that when two elements combine to form more than one compound, the masses of one element that combine with a fixed mass of the other are in the ratio of small whole numbers. To verify this with carbon and oxygen, we consider the two cases: carbon dioxide (CO2) and carbon monoxide (CO).

When 6.0g of carbon reacts with oxygen, we can get either 22.0g of carbon dioxide or 14.0g of carbon monoxide. The mass of oxygen that combines with the 6.0g of carbon can be calculated for each compound:

The ratio of the mass of oxygen in carbon dioxide to the mass of oxygen in carbon monoxide is 16.0g : 8.0g = 2:1, which is a small whole number ratio, thus verifying the law of multiple proportions.

To determine the molecular formula of Alaxin, given its relative molecular mass is 284:

For a reaction system at equilibrium, LeChatelier's principle can be used to predict the "effect of a stress on the system".

Option: C

Explanation:

Le Chatelier's theory can be implemented to forecast a system's behavior due to variations in pressure, temperature, or concentration that will lead in predictable and contested variations in the system adjustments to establish a new state of equilibrium. This means that adding heat to a process would favor the endothermic path of a reaction, because this decreases the amount of heat generated in the system.

Here shift in equilibrium take place when volume increase, the total pressure decreases, which have potential to reverse the reaction, while on increasing pressure of system, the total volume decreases of the gaseous system, which can shift an equilibrium in the direction of the fewer molecules.

For a reaction system at equilibrium, the Le principle can be used to predict the effect of a stress on the system.

The Le principle is an observation about chemical equilibria of reactions. Le principle can be used to predict the effect of a stress like changing concentration of a substance has on a reaction system at equilibrium.

If the concentration of a reaction species is increased at constant Temperature and Volume, the equilibrium system will shift in the direction that reduces the concentration of that substance so we can conclude that the Le principle can be used to predict the effect of a stress on the system.

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Answer:

Liquid B because of its higher vapor pressure due to the fact that evaporation rate is directly proportional to vapor pressure

Explanation:

The vapor pressure of  liquid at equilibrium is a function to the liquid's rate of evaporation. The evaporation rate and hence the vapor pressure is a measure of the propensity of the particles  of the liquid to leave the surface of the liquid and exist as vapor directly above the liquid. As high evaporation rate leads to high vapor pressure, a liquid with a higher vapor pressure will evaporate faster than one with a lower vapor pressure at the same temperature and pressure.

Therefore, liquid B with a vapor pressure of 18.04 kPa at 40° C will evaporate faster than liquid A with a lower vapor pressure of 7.37 kPa at the same 40°C.

Liquid B with a higher vapor pressure of 18.04 kPa at 40°C would evaporate faster than liquid A with 7.37 kPa, as higher vapor pressure indicates that the liquid is more volatile and its molecules can more easily escape into the gas phase.

At 40°C, between liquid A with a vapor pressure of 7.37 kPa and liquid B with a vapor pressure of 18.04 kPa, liquid B would evaporate faster. This is because vapor pressure is a measure of the tendency of molecules to escape from a liquid and enter the gas phase. A higher vapor pressure indicates that molecules can break away from the surface of the liquid more easily, which is indicative of a more volatile liquid. Therefore, liquid B, with its higher vapor pressure at the same temperature, is the more volatile and will evaporate more rapidly than liquid A.

Vapor pressure of a liquid is directly related to its intermolecular forces; liquids with weaker intermolecular forces have higher vapor pressures, and hence they evaporate faster. Conversely, greater intermolecular forces result in a lower vapor pressure and slower evaporation rate. For volatile liquids in a mixture, adding their partial pressures yields the total vapor pressure of the mixture

Answer:

Preceding accumulative aggregate of energy indispensable is disseminated as 5455 J.

Explanation:

Allotted the contiguous information:

Q: Not identified.

M: 224 g

S: 0.343 J/g°C

Final thermodynamics: 71°C

Initial thermodynamics: 0°C

ΔT = 71°C

We can equate as imminent:

Q = 224 g · 0.343 J/g°C · 71°C

Q ⇒ 5455 J

Hence, the pertaining preeminent albeit paramount indispensable consignment or quantity of energy obligated, concerning an augmentation in thermodynamics subject to the undisclosed metal by 71°C is 5,455 J.

The energy required to raise the temperature of the metal is 5365.256 J.

To calculate the energy required to raise the temperature of a substance, we use the formula:

q = m * c * ΔT

The energy required to raise the temperature of a substance can be calculated using the formula: q = mcΔT where q is the energy in joules, m is the mass in grams, c is specific heat capacity in J/(g•°C), and ΔT is the change in temperature in °C.

Given that the mass (m) of the metal is 224 g, the specific heat capacity (c) is 0.343 J/(g•°C), and the temperature change (ΔT) is 71°C, you can substitute these values into the formula:

Plugging in the values given:

q = (224 g) * (0.343 J/(g•°C)) * (71°C)

Simplifying the equation gives:

q = 5365.256 J

Therefore, the energy required to raise the temperature of 224 g of this metal by 71°C is 5365.256 J.

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Answer:

D) 2, 4, and 5

Explanation:

In order to fully comprehend the answer choices we must take a close look at the value of ΔH° = 31.05. The enthalpy change of the reaction is positive. A positive value of enthalpy of reaction implies that heat was absorbed in the course of the reaction.

If heat is absorbed in a reaction, that reaction is endothermic.

Since ∆Hreaction= ∆H products -∆H reactants, a positive value of ∆Hreaction implies that ∆Hproducts >∆Hreactants, hence the answer choice above.

Answer:

D

Explanation: