The pressure of a sample of CH4 gas (6.022 g)in a 30.0 L vessel at 402 K is ________ atm.

A) 2.42 B) 6.62 C) 0.413 D) 12.4 E) 22.4 A) 2.42 B) 6.62 C) 0.413 D) 12.4 E) 22.4

The root-mean-square speed of N2 at 33.5 °C is ________ m/sec.

A) 522 B) 51.9 C) 173 D) 302 E) 16.5 A) 522 B) 51.9 C) 173 D) 302 E) 16.5

The reaction of 50 mL of Cl2 gas with 50 mL of CH4 gas via the equation: Cl2 (g) + CH4 (g) → HCl (g) + CH3Cl (g) Will produce a total of ________ mL of products if pressure and temperature are kept constant.

A) 100 B) 50 C) 200 D) 150 E) 250 A) 100 B) 50 C) 200 D) 150 E) 250

A vessel contains a mixture of 34.9 grams of H2 (g)and 17.7 grams of CH4. If the total pressure inside the vessel is measured at 2.92 atm, the partial pressure of H2 (g)must be _____ atm.

A) 2.75 B) 50.5 C) 0.175 D) 53.8 E) 5.53 A) 2.75 B) 50.5 C) 0.175 D) 53.8 E) 5.53

Exam 10: Gases | Examlex

A sample of H₂ gas (2.0 L)at 3.5 atm was combined with 1.5 L of N₂ gas at 2.6 atm pressure at a constant temperature of 25 °C into a 7.0 L flask. The total pressure in the flask is ________ atm. Assume the initial pressure in the flask was 0.00 atm and the temperature upon mixing was 25 °C.

(Multiple Choice)

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Question 121

The pressure of a sample of CH₄ gas (6.022 g)in a 30.0 L vessel at 402 K is ________ atm.

(Multiple Choice)

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Question 122

The root-mean-square speed of N₂ at 33.5 °C is ________ m/sec.

(Multiple Choice)

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Question 123

The pressure in a 12.2 L vessel that contains 2.34 g of carbon dioxide, 1.73 g of sulfur dioxide, and 3.33 g of argon, all at 42 °C is ________ mm Hg.

(Multiple Choice)

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Question 124

One significant difference between gases and liquids is that ________.

(Multiple Choice)

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Question 125

SO₂ (5.00 g)and CO₂ (5.00 g)are placed in a 750.0 mL container at 50.0 °C. The partial pressure of SO₂ in the container was ________ atm.

(Multiple Choice)

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Question 126

Which one of the following is a valid statement of Avogadro's law?

(Multiple Choice)

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Question 127

A sample of oxygen gas was found to effuse at a rate equal to two times that of an unknown gas. The molecular weight of the unknown gas is ________ g/mol.

(Multiple Choice)

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Question 128

The reaction of 50 mL of Cl₂ gas with 50 mL of CH₄ gas via the equation: Cl₂ (g) + CH₄ (g) → HCl (g) + CH₃Cl (g) Will produce a total of ________ mL of products if pressure and temperature are kept constant.

(Multiple Choice)

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Question 129

A vessel contains a mixture of 34.9 grams of H₂ (g)and 17.7 grams of CH₄. If the total pressure inside the vessel is measured at 2.92 atm, the partial pressure of H₂ (g)must be _____ atm.

(Multiple Choice)

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Question 130

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

(Multiple Choice)

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Question 131

A mixture of two gases was allowed to effuse from a container. One of the gases escaped from the container 1.43 times as fast as the other one. The two gases could have been ________.

(Multiple Choice)

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Question 132

CO (5.00 g)and CO₂ (5.00 g)were placed in a 750.0 mL container at 50.0 °C. The partial pressure of CO in the container was ________ atm.

(Multiple Choice)

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Question 133

Of the following, only ________ is impossible for an ideal gas.

(Multiple Choice)

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Question 134

A balloon originally had a volume of 4.39 L at 44 °C and a pressure of 729 torr. The balloon must be cooled to ________ °C to reduce its volume to 3.99 L (at constant pressure).

(Multiple Choice)

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Question 135

CO (5.00 g)and CO₂ (5.00 g)were placed in a 750.0 mL container at 50.0 °C. The total pressure in the container was ________ atm.

(Multiple Choice)

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Question 136

The volume of HCl gas required to react with excess magnesium metal to produce 6.82 L of hydrogen gas at 2.19 atm and 35.0 °C is ________ L.

(Multiple Choice)

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Question 137

The effusion rate of a gas is proportional to the square root of its molar mass.

(True/False)

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Question 138

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

(Short Answer)

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Question 139

Using the van der Waals equation, the pressure in a 22.4 L vessel containing 1.50 mol of chlorine gas at 0.00 °C is ________ atm. (a = 6.49 L²-atm/mol², b = 0.0562 L/mol)

(Multiple Choice)

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Question 140

Showing 121 - 140 of 175

Exam 10: Gases

A sample of H2 gas (2.0 L)at 3.5 atm was combined with 1.5 L of N2 gas at 2.6 atm pressure at a constant temperature of 25 °C into a 7.0 L flask. The total pressure in the flask is ________ atm. Assume the initial pressure in the flask was 0.00 atm and the temperature upon mixing was 25 °C.

The pressure of a sample of CH4 gas (6.022 g)in a 30.0 L vessel at 402 K is ________ atm.

The root-mean-square speed of N2 at 33.5 °C is ________ m/sec.

The pressure in a 12.2 L vessel that contains 2.34 g of carbon dioxide, 1.73 g of sulfur dioxide, and 3.33 g of argon, all at 42 °C is ________ mm Hg.

One significant difference between gases and liquids is that ________.

SO2 (5.00 g)and CO2 (5.00 g)are placed in a 750.0 mL container at 50.0 °C. The partial pressure of SO2 in the container was ________ atm.

Which one of the following is a valid statement of Avogadro's law?

A sample of oxygen gas was found to effuse at a rate equal to two times that of an unknown gas. The molecular weight of the unknown gas is ________ g/mol.

The reaction of 50 mL of Cl2 gas with 50 mL of CH4 gas via the equation: Cl2 (g) + CH4 (g) → HCl (g) + CH3Cl (g) Will produce a total of ________ mL of products if pressure and temperature are kept constant.

A vessel contains a mixture of 34.9 grams of H2 (g)and 17.7 grams of CH4. If the total pressure inside the vessel is measured at 2.92 atm, the partial pressure of H2 (g)must be _____ atm.

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

A mixture of two gases was allowed to effuse from a container. One of the gases escaped from the container 1.43 times as fast as the other one. The two gases could have been ________.

CO (5.00 g)and CO2 (5.00 g)were placed in a 750.0 mL container at 50.0 °C. The partial pressure of CO in the container was ________ atm.

Of the following, only ________ is impossible for an ideal gas.

A balloon originally had a volume of 4.39 L at 44 °C and a pressure of 729 torr. The balloon must be cooled to ________ °C to reduce its volume to 3.99 L (at constant pressure).

CO (5.00 g)and CO2 (5.00 g)were placed in a 750.0 mL container at 50.0 °C. The total pressure in the container was ________ atm.

The volume of HCl gas required to react with excess magnesium metal to produce 6.82 L of hydrogen gas at 2.19 atm and 35.0 °C is ________ L.

The effusion rate of a gas is proportional to the square root of its molar mass.

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

Using the van der Waals equation, the pressure in a 22.4 L vessel containing 1.50 mol of chlorine gas at 0.00 °C is ________ atm. (a = 6.49 L2-atm/mol2, b = 0.0562 L/mol)

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A sample of H₂ gas (2.0 L)at 3.5 atm was combined with 1.5 L of N₂ gas at 2.6 atm pressure at a constant temperature of 25 °C into a 7.0 L flask. The total pressure in the flask is ________ atm. Assume the initial pressure in the flask was 0.00 atm and the temperature upon mixing was 25 °C.

The pressure of a sample of CH₄ gas (6.022 g)in a 30.0 L vessel at 402 K is ________ atm.

The root-mean-square speed of N₂ at 33.5 °C is ________ m/sec.

SO₂ (5.00 g)and CO₂ (5.00 g)are placed in a 750.0 mL container at 50.0 °C. The partial pressure of SO₂ in the container was ________ atm.

The reaction of 50 mL of Cl₂ gas with 50 mL of CH₄ gas via the equation: Cl₂ (g) + CH₄ (g) → HCl (g) + CH₃Cl (g) Will produce a total of ________ mL of products if pressure and temperature are kept constant.

A vessel contains a mixture of 34.9 grams of H₂ (g)and 17.7 grams of CH₄. If the total pressure inside the vessel is measured at 2.92 atm, the partial pressure of H₂ (g)must be _____ atm.

CO (5.00 g)and CO₂ (5.00 g)were placed in a 750.0 mL container at 50.0 °C. The partial pressure of CO in the container was ________ atm.

CO (5.00 g)and CO₂ (5.00 g)were placed in a 750.0 mL container at 50.0 °C. The total pressure in the container was ________ atm.

Using the van der Waals equation, the pressure in a 22.4 L vessel containing 1.50 mol of chlorine gas at 0.00 °C is ________ atm. (a = 6.49 L²-atm/mol², b = 0.0562 L/mol)