Question 1

The volume of 0.65 mol of an ideal gas at 365 torr and 97 °C is _ L.

Accepted Answer

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Question 2

A sample of He gas (3.0 L) at 5.6 atm and 25 °C was combined with 4.5 L of Ne gas at 3.6 atm and 25 °C at constant temperature in a 9.0 L flask. The total pressure in the flask was atm. Assume the initial pressure in the flask was 0.00 atm.

Accepted Answer

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Question 3

A sample of a gas (1.50 mol) is contained in a 15.0 L cylinder. The temperature is increased from 100 °C to 150 °C. The ratio of final pressure to initial pressure [ ^P²] is . P₁

Accepted Answer

The pressure of a gas is directly proportional to its temperature when volume and moles are constant. Using the ideal gas law, P1/T1 = P2/T2. Convert temperatures to Kelvin: T1 = 373 K, T2 = 423 K. The ratio P2/P1 = T2/T1 = 423/373 ≈ 1.13.

Question 4

The molecular weight of a gas that has a density of 5.75 g/L at STP is g/mol.

Accepted Answer

The density of a gas at STP (standard temperature and pressure: 0°C and 1 atm) is 1.27 g/L. Thus, a gas with a density of 5.75 g/L at STP has a molecular weight that is about 4.5 times greater than that of air, which has a molecular weight of 28.97 g/mol. Therefore, we can estimate that the molecular weight of the gas is around 130 g/mol. The only choice close to this value is B (129), which is the correct answer.

Question 5

The rms speed of methane molecules at 45.0 °C is m/sec.

Accepted Answer

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Question 6

What is the density (in g/L) of oxygen gas at 77 ^oC and 700 torr?

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Question 7

What is the partial pressure (in mm Hg) of neon in a 4.00 L vessel that contains 0.838 mol of methane, 0.184 mol of ethane, and 0.755 mol of neon at a total pressure of 928 mmHg?

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Question 8

Given the equation Determine the number of liters of O₂consumed at STP when 270.0 grams of C₂H₆is burned.

Accepted Answer

The answer of Given the equation  
Determine the number...

Question 9

The first person to investigate the relationship between the pressure of a gas and its volume was

Accepted Answer

The relationship between the pressure of a gas and its volume is known as Boyle's law, named after Robert Boyle, who was the first person to investigate it in the 17th century. Jacques Charles, Amadeo Avogadro, Joseph Louis Gay-Lussac, and Lord Kelvin all made significant contributions to the study of gases, but Boyle was the first to specifically examine the relationship between pressure and volume.

Question 10

How many molecules are there in 4.00 L of oxygen gas at 500 ^oC and 50.0 torr?

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Question 11

A closed- end manometer was attached to a vessel containing argon. The difference in the mercury levels in the two arms of the manometer was 12.2 cm. Atmospheric pressure was 783 mmHg. The pressure of the argon in the container was mmHg.

Accepted Answer

In a closed-end manometer, the pressure of the gas is equal to the difference in mercury levels. Therefore, the pressure of the argon is 12.2 cm, which is equivalent to 122 mmHg.

Question 12

The temperature and pressure specified by STP are ^oC and atm.

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Question 13

A sample of O₂gas (2.0 mmol) effused through a pinhole in 5.0 s. It will take s for the same amount of CO₂to effuse under the same conditions.

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Question 14

The amount of gas that occupies 60.82 L at 31 °C and 367 mmHg is mol.

Accepted Answer

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Question 15

The density of chlorine (Cl₂) gas at 25 °C and 60. kPa is g/L)

Accepted Answer

The density of a gas can be calculated using the ideal gas law rearranged to find density: $ \text{Density} = \frac{PM}{RT} $. For Cl2, with P = 60 kPa, M = 70.9 g/mol, R = 8.314 J/(mol·K), and T = 298 K, the density is approximately 1.7 g/L.

Question 16

A vessel contained N₂, Ar, He, and Ne. The total pressure in the vessel was 987 torr. The partial pressures of nitrogen, argon, and helium were 44.0, 486, and 218 torr, respectively. The partial pressure of neon in the vessel was torr.

Accepted Answer

The partial pressure of neon can be found by subtracting the sum of the partial pressures of nitrogen, argon, and helium from the total pressure: 987 - (44.0 + 486 + 218) = 239 torr.

Question 17

Given the equation Determine the number of liters of CO₂formed at STP. when 240.0 grams of C₂H₆is burned in excess oxygen gas.

Accepted Answer

The answer of Given the equation  
Determine the number...

Question 18

Using the van der Waals equation, the pressure in a 22.4 L vessel containing 1.00 mol of neon gas at 100 °C is atm. (a = 0.211 L²- atm/mol², b = 0.0171 L/mol)

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Question 19

The reaction of 50 mL of Cl₂gas with 50 mL of CH₄gas via the equation: Cl₂(g) + C₂H₄(g) -C₂H₄Cl₂(g) Will produce a total of mL of products if pressure and temperature are kept constant.

Accepted Answer

According to the balanced equation, the reaction consumes equal volumes of Cl₂ and CH₄ gases, and produces the same volume of product. Thus, the total volume of products formed is 50 mL, which is the same as the initial volume of each reactant. The correct answer is therefore (C) 50.

Question 20

The van der Waals equation for real gases recognizes that .

Accepted Answer

The van der Waals equation accounts for the non-zero volume of gas particles and the intermolecular forces between them, which affect the pressure and volume of real gases compared to ideal gases.

Quiz 10: Gases

The volume of 0.65 mol of an ideal gas at 365 torr and 97 °C is _ L.

A sample of He gas (3.0 L) at 5.6 atm and 25 °C was combined with 4.5 L of Ne gas at 3.6 atm and 25 °C at constant temperature in a 9.0 L flask. The total pressure in the flask was atm. Assume the initial pressure in the flask was 0.00 atm.

A sample of a gas (1.50 mol) is contained in a 15.0 L cylinder. The temperature is increased from 100 °C to 150 °C. The ratio of final pressure to initial pressure [ P2 ] is . P1

The molecular weight of a gas that has a density of 5.75 g/L at STP is g/mol.

The rms speed of methane molecules at 45.0 °C is m/sec.

What is the density (in g/L) of oxygen gas at 77 oC and 700 torr?

What is the partial pressure (in mm Hg) of neon in a 4.00 L vessel that contains 0.838 mol of methane, 0.184 mol of ethane, and 0.755 mol of neon at a total pressure of 928 mmHg?

Given the equation Determine the number of liters of O2 consumed at STP when 270.0 grams of C2H6 is burned.

The first person to investigate the relationship between the pressure of a gas and its volume was

How many molecules are there in 4.00 L of oxygen gas at 500 oC and 50.0 torr?

A closed- end manometer was attached to a vessel containing argon. The difference in the mercury levels in the two arms of the manometer was 12.2 cm. Atmospheric pressure was 783 mmHg. The pressure of the argon in the container was mmHg.

The temperature and pressure specified by STP are oC and atm.

A sample of O2 gas (2.0 mmol) effused through a pinhole in 5.0 s. It will take s for the same amount of CO2 to effuse under the same conditions.