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Exam 10: Gases

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Question 61

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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

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Question 62

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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

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Question 63

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___________ 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?

Nitrogen will behave most like an ideal gas

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

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?

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)

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?

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)

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

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)

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)

Gases form heterogeneous mixtures or solutions with one another.

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)

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)

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)