Homework Answers

A flask of 7L contains a mixture of 6g of O2 and 15g of N2 at 30°C.What is the partial pressure of the oxygen gas?

[1] 0.67 atm

[2] 1.9 atm

[3] 2.59 atm

[4] 22.1 atm

[5] None of the above

A 1.00 L flask contains 2.073 g O2 and 20.13 g N2 at 25.0°C. What is the total pressure? [1] 0.856 atm

[2] 1.09 atm

[3] 19.2 atm

[4] 22.2 atm

[5] None of the above 

For a gas, which two variables are inversely proportional to each other (if all other conditions remain constant)?

[1] Pressure and temperature

[2] Pressure and volume

[3] Volume and temperature

[4] Amount (number of moles) and volume

[5] Pressure, temperature and volume 

A 3.20 mol sample of a gas occupies a volume of 350 mL at 300.0 K. What is its pressure?

[1] 1.32 atm

[2] 67.0 atm

[3] 184 atm

[4] 225 atm

5] 312 atm 

What is the partial pressure of oxygen in a container that contains 2.0 mol of oxygen, 3.0 mol of nitrogen, and 1.0 mol of carbon dioxide when the total pressure is 900 Torr?

[1] 100 Torr

[2] 200 Torr

[3] 300 Torr

[4] 400 Torr

[5] None of the above

The properties of a real gas are most likely to deviate from those properties predicted for an ideal gas when

[1] the pressure is low

[2] the temperature is high

[3] the pressure is high and the temperature is low

[4] the pressure is low and the temperature is high

[5] it is a diatomic gas

Consider the reaction: H2 (g) + Br2 (g) ⇆ 2HBr (g

Suppose that the value of the equilibrium constant is very large, which species will predominate at equilibrium?

[1] H2

[2] Br2

[3] HBr

[4] Both H2 and Br2

[5] All species will have the same concentration.

The expression for Kc for this reaction is:

[1] Kc= [H2][Br2] / [HBr]2

[2] Kc= [H2][Br2] / [HBr]

[3] Kc= [HBr]2 / [H2][Br2]

[4] Kc= 2[HBr] / [H2][Br2]

[5] Kc= [HBr] / [H2][Br2]