What is the pressure in atmospheres exerted by a column of mercury that is 100.m high? (density of mercury = 13.5951 g/cm3,gravitational constant = 9.80665 m/s2,1 atm = 101,325 Pa = 760 torr = 760 mmHg)

A) 1.4 × 1010 atm B) 0.013 atm C) 0.73 atm D) 1.37 atm E) 132 atm A) 1.4 × 1010 atm B) 0.013 atm C) 0.73 atm D) 1.37 atm E) 132 atm

Consider the following reaction. H2(g)+ I2(s)→ 2 HI(g) If the cylinder with a movable piston below contains 1 mol H2(g)and 1 mol I2(s),which represents the cylinder after the reaction is complete?

A) B) C) D) E) None of the above A) B) C) D) E) None of the above

The pressure of hydrogen sulfide gas in a container is 3.565 ×104 Pa.What is this pressure in torr? (1 atm = 101,325 Pa = 760 torr)?

A) 46.91 torr B) 267.4 torr C) 351.8 torr D) 3612 torr E) 2.709 ×104 torr A) 46.91 torr B) 267.4 torr C) 351.8 torr D) 3612 torr E) 2.709 ×104 torr

What is the volume occupied by 35.2 g of methane gas (CH4)at 25°C and 1.0 atm? (R = 0.08206 L • atm/K • mol)

A) 0.0186 L B) 4.5 L C) 11.2 L D) 49.2 L E) 53.7 L A) 0.0186 L B) 4.5 L C) 11.2 L D) 49.2 L E) 53.7 L

Exam 10: Gases | Examlex

What is the pressure in atmospheres exerted by a column of mercury that is 100.m high? (density of mercury = 13.5951 g/cm³,gravitational constant = 9.80665 m/s²,1 atm = 101,325 Pa = 760 torr = 760 mmHg)

(Multiple Choice)

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Question 101

1.000 atm of oxygen gas,placed in a container having a pinhole opening in its side,leaks from the container 2.14 times faster than does 1.000 atm of an unknown gas placed in this same apparatus.Which of the following species could be the unknown gas?

(Multiple Choice)

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Question 102

A sample of hydrogen gas exerts a pressure of 466 torr in a container.What is this pressure in atmospheres? (1 atm = 1.01325 ×10⁵ Pa = 760 torr)

(Multiple Choice)

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Question 103

Consider the following reaction. H₂(g)+ I₂(s)→ 2 HI(g) If the cylinder with a movable piston below contains 1 mol H₂(g)and 1 mol I₂(s),which represents the cylinder after the reaction is complete?

(Multiple Choice)

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Question 104

A flask with a volume of 3.16 L contains 9.33 g of an unknown gas at 32.0°C and 1.00 atm. What is the molar mass of the gas? (R = 0.08206 L • atm/K • mol)

(Multiple Choice)

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Question 105

At -3°C,2.5 moles of a gas in a 0.50-L container exert a pressure of 135 atm.Under these conditions,is the gas behaving like an ideal gas?

(Essay)

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Question 106

What are the units of the constant b in the van der Waals equation?

(Multiple Choice)

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Question 107

Assuming ideal behavior,what is the density of argon gas at STP? (R = 0.08206 L • atm/K • mol)

(Multiple Choice)

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Question 108

Gases form heterogeneous mixtures or solutions with one another.

(True/False)

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Question 109

When active metals such as magnesium are immersed in acid solution,hydrogen gas is evolved. Calculate the volume of H₂(g)at 30.1°C and 0.85 atm that can be formed when 275 mL of 0.725 M HCl solution reacts with excess Mg to give hydrogen gas and aqueous magnesium chloride. Mg(s)+ 2HCl(aq)→ MgCl₂(aq)+ H₂(g) (R = 0.08206 L • atm/K • mol)

(Multiple Choice)

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Question 110

The pressure of hydrogen sulfide gas in a container is 3.565 ×10⁴ Pa.What is this pressure in torr? (1 atm = 101,325 Pa = 760 torr)?

(Multiple Choice)

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Question 111

What is the volume occupied by 35.2 g of methane gas (CH₄)at 25°C and 1.0 atm? (R = 0.08206 L • atm/K • mol)

(Multiple Choice)

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Question 112

___________ is the formula to determine the molar mass of a compound using the ideal gas law.

(Short Answer)

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Question 113

The rate of diffusion of a gas is inversely proportional to its molar mass.

(True/False)

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Question 114

A gaseous compound is 30.4% nitrogen and 69.6% oxygen by mass.A 5.25-g sample of the gas occupies a volume of 1.00 L and exerts a pressure of 1.26 atm at -4.0°C.What is its molecular formula? (R = 0.08206 L • atm/K • mol)

(Multiple Choice)

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Question 115

___________ is the formula to determine the amount of a reactant or product in units of moles using the ideal gas law.

(Short Answer)

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Question 116

What is the final temperature of a gas that expands from a volume of 22.4 L at 278 K to a volume of 38.3 L?

(Multiple Choice)

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Question 117

What mass of KClO₃ must be decomposed to produce 126 L of oxygen gas at 133°C and 0.880 atm? (The other reaction product is solid KCl.) (R = 0.08206 L • atm/K • mol)

(Multiple Choice)

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Question 118

Nitrogen will behave most like an ideal gas

(Multiple Choice)

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Question 119

What volume of CO₂ gas at 645 torr and 800.K could be produced by the decomposition of 45.0 g of CaCO₃? CaCO₃(s)→ CaO(s)+ CO₂(g) (R = 0.08206 L • atm/K • mol)

(Multiple Choice)

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Question 120

Showing 101 - 120 of 131

Exam 10: Gases

What is the pressure in atmospheres exerted by a column of mercury that is 100.m high? (density of mercury = 13.5951 g/cm3,gravitational constant = 9.80665 m/s2,1 atm = 101,325 Pa = 760 torr = 760 mmHg)

1.000 atm of oxygen gas,placed in a container having a pinhole opening in its side,leaks from the container 2.14 times faster than does 1.000 atm of an unknown gas placed in this same apparatus.Which of the following species could be the unknown gas?

A sample of hydrogen gas exerts a pressure of 466 torr in a container.What is this pressure in atmospheres? (1 atm = 1.01325 ×105 Pa = 760 torr)

Consider the following reaction. H2(g)+ I2(s)→ 2 HI(g) If the cylinder with a movable piston below contains 1 mol H2(g)and 1 mol I2(s),which represents the cylinder after the reaction is complete?

A flask with a volume of 3.16 L contains 9.33 g of an unknown gas at 32.0°C and 1.00 atm. What is the molar mass of the gas? (R = 0.08206 L • atm/K • mol)

At -3°C,2.5 moles of a gas in a 0.50-L container exert a pressure of 135 atm.Under these conditions,is the gas behaving like an ideal gas?

What are the units of the constant b in the van der Waals equation?

Assuming ideal behavior,what is the density of argon gas at STP? (R = 0.08206 L • atm/K • mol)

Gases form heterogeneous mixtures or solutions with one another.

The pressure of hydrogen sulfide gas in a container is 3.565 ×104 Pa.What is this pressure in torr? (1 atm = 101,325 Pa = 760 torr)?

What is the volume occupied by 35.2 g of methane gas (CH4)at 25°C and 1.0 atm? (R = 0.08206 L • atm/K • mol)

___________ is the formula to determine the molar mass of a compound using the ideal gas law.

The rate of diffusion of a gas is inversely proportional to its molar mass.

A gaseous compound is 30.4% nitrogen and 69.6% oxygen by mass.A 5.25-g sample of the gas occupies a volume of 1.00 L and exerts a pressure of 1.26 atm at -4.0°C.What is its molecular formula? (R = 0.08206 L • atm/K • mol)

___________ is the formula to determine the amount of a reactant or product in units of moles using the ideal gas law.

What is the final temperature of a gas that expands from a volume of 22.4 L at 278 K to a volume of 38.3 L?

What mass of KClO3 must be decomposed to produce 126 L of oxygen gas at 133°C and 0.880 atm? (The other reaction product is solid KCl.) (R = 0.08206 L • atm/K • mol)

Nitrogen will behave most like an ideal gas

What volume of CO2 gas at 645 torr and 800.K could be produced by the decomposition of 45.0 g of CaCO3? CaCO3(s)→ CaO(s)+ CO2(g) (R = 0.08206 L • atm/K • mol)

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What is the pressure in atmospheres exerted by a column of mercury that is 100.m high? (density of mercury = 13.5951 g/cm³,gravitational constant = 9.80665 m/s²,1 atm = 101,325 Pa = 760 torr = 760 mmHg)

A sample of hydrogen gas exerts a pressure of 466 torr in a container.What is this pressure in atmospheres? (1 atm = 1.01325 ×10⁵ Pa = 760 torr)

Consider the following reaction. H₂(g)+ I₂(s)→ 2 HI(g) If the cylinder with a movable piston below contains 1 mol H₂(g)and 1 mol I₂(s),which represents the cylinder after the reaction is complete?

The pressure of hydrogen sulfide gas in a container is 3.565 ×10⁴ Pa.What is this pressure in torr? (1 atm = 101,325 Pa = 760 torr)?

What is the volume occupied by 35.2 g of methane gas (CH₄)at 25°C and 1.0 atm? (R = 0.08206 L • atm/K • mol)

What mass of KClO₃ must be decomposed to produce 126 L of oxygen gas at 133°C and 0.880 atm? (The other reaction product is solid KCl.) (R = 0.08206 L • atm/K • mol)

What volume of CO₂ gas at 645 torr and 800.K could be produced by the decomposition of 45.0 g of CaCO₃? CaCO₃(s)→ CaO(s)+ CO₂(g) (R = 0.08206 L • atm/K • mol)