3.4 Ideal Gas Law

Multiple Choice

Gases have...

• A definite shape and volume

• A definite shape but no definite volume

• No definite shape but a definite volume

• No definite shape or volume

Multiple Choice

760 mmHg is equal to

• 1 torr

• 760 atm

• 760 torr

• 101 Pa

Multiple Choice

What does STP (standard temperature and pressure) stand for?

• 0.0 degree Celcius and 1 atm

• 1.0 mmHg and 273 degree Kelvin

• 1.0 degree Celcius and 0 atm

• 1.0 atm 273 degree Celcius

Multiple Choice

IF we are using Boyles' law and our Pressure goes UP, what must our volume do?

• Go UP

• Go DOWN

• Stay the same

• Wrong law.

Multiple Choice

Which container will have a lower pressure?

• left
• right
• they both have the same pressure
• I don't know

Multiple Choice

What is the formula Charles' Law?

• V = T
• VT = VT
• T₁ / V_{1 =} T₂ / V₂
• V₁ / T₁ = V₂ / T₂

Multiple Choice

Which law helps us find the moles of gas in a sample?

• Charles Law
• Boyle's Law
• Combined Gas Law
• Ideal Gas Law

Multiple Choice

A gas mixture at 0°C and 1.0 atm contains 0.010 mol of H2 , 0.015 mol of O2 , and 0.025 mol of N2 . Assuming ideal behavior, what is the partial pressure of hydrogen gas (H2 ) in the mixture?

• about 0.010 atm, bc there is 0.010 mol H2

• about 0.050 atm, bc there is 0.050 mol of gases at 0C and 1.0 atm.

• About 0.20 atm, because H2

  comprises 20% of the total number of moles of gas.

• About 0.40 atm, because the mole ratio of H2 :O2 :N2 is 0.4:0.6:1.

Multiple Choice

An equimolar mixture of N2 (g) and Ar(g) is kept inside a rigid container at a constant temperature of 300 K. The initial partial pressure of Ar in the mixture is 0.75 atm. An additional amount of Ar was added to the container, enough to double the number of moles of Ar gas in the mixture. Assuming ideal behavior, what is the final pressure of the gas mixture after the addition of the Ar gas?

• 0.75atm, because increasing the partial pressure of Ar decreases the partial pressure of N2

• 1.13atm, because 33% of the moles of gas are N2 .

• 1.50atm, because the number of moles of N2 did not change.

• 2.25atm, because doubling the number of moles of Ar doubles its partial pressure