Chapter 8: Gases

A scuba diver $60ft$below the ocean surface inhales $50.0mL$of compressed air from a ccuba tank at a pressure of $3.00atm$and a temperature of $8°C$. What is the final pressure of air, in atmospheres, in the lungs when the gas expands to $150.0mL$at a body temperature of $37°C$, if the amount of gas does not change?

What happens to the volume of a bicycle tire or a basketball when you use an air pump to add air?

Sometimes when you blow up a balloon and release it, it flies around the room. What is happening to the air in the balloon and its volume?

A sample containing$1.50molesofNe$gas has an initial volume of $8.00L$. What is the final volume, in liters, when each of the following occurs and pressure and temperature do not change?

a. A leak allows one-half of $Ne$atoms to escape.

b. A sample of$3.50molesofNe$is added to the $1.50molesofNe$gas in the container.

c. A sample of $25.0g$of $Ne$is added to the $1.50molesofNe$gas in the container.

Which of the following statements describe the pressure of a gas?
a. the force of the gas particles on the walls of the container
b. the number of gas particles in a container
c. $4.5L$ of helium gas
d. $750$Torr
e. $28.8Ib/i{n}^2$

Use the molar volume to calculate each of the following at STP:

a. the number of moles of O₂in 44.8 L of O₂ gas.

b. the volume in liters, occupied by 2.50 moles of N₂ gas.

c. the volume, in liters, occupied by 50.0 g of Ar gas.

d. the number of grams of H₂ in 16.20 mL of H₂ gas.

A typical air sample in the lungs contains oxygen at $100mmHg$, nitrogen at $573mmHg$,n carbon dioxide at $40mmHg$, and water vapor at $47mmHg$. Why are these pressures called partial pressures?

Suppose a mixture contains helium and oxygen gases. If the partial pressure of helium is the same as the partial pressure of oxygen, what do you know about the number of helium atoms compared to the number of oxygen molecules? Explain.

In a gas mixture, the partial pressures are nitrogen $425Torr$, oxygen $115Torr$, and helium $225Torr$. What is the total pressure, in Torr, exerted by the gas mixture?

In a gas mixture, the partial pressure are argon $415mmHg$, neon $75mmHg$, and nitrogen $125mmHg$. What is the total pressure, in $mmHg$, exerted by the gas mixture?