AP Chemistry Gases Chapter 5 Harshini

When a sample of carbon dioxide gas in a closed container of constant volume at 0.5 atm and 200 K is heated until its temperature reaches 400 K, its new pressure is closest to

• 0.25 atm

• 0.50 atm

• 1.0 atm

• 1.5 atm

A 0.33 mole sample of CaCO3(s) is placed in a 1 L evacuated flask, which is then sealed and heated. The CaCO3(s) decomposes completely according to the balanced equation below. The total pressure in the flask, measured at 300 K is closest to which of the following? (The gas constant, R = 0.082 L atm/mol K)

CaCO3(s) → CaO(s) + CO2(g)

• 2.0 atm

• 4.1 atm

• 8.1 atm

• 16 atm

The reaction below takes place in a closed, rigid vessel. The initial pressure of N2(g) is 1.0 atm, and that of O2(g) is 1.5 atm. No N2O4(g) is initially present. The experiment is carried out at a constant temperature. What is the total pressure in the container when the partial pressure of N2O4 reaches 0.75 atm?

N2 + 2O2 → N2O4

• 0.25 atm

• 0.75 atm

• 1.0 atm

• 2.0 atm

A 1.53-L sample of SO2 at a pressure of 5.6 x 10^3 Pa. The pressure is changed to 1.5 x 10^4 Pa at a constant temp, what is the new volume?

• 4.098 L

• 0.3 L

• 6.66 x 10^5 L

• 0.57 L

A gaseous mixture of oxygen and nitrogen is maintained at a constant temperature. Which of the following MUST be true regarding the two gases?

• Their average kinetic energies will be the same.

• Their average molecular speeds will be the same.

• Their partial pressures will be the same.

• Their total masses will be the same

A sample of gas at 15°C and 1 atm has a volume of 2.58 L. What volume will this gas occupy at 38°C and 1 atm?

• 34.716 L

• 2.79 L

• 0.3434 L

• 1.582 L

A sample of Ammonia gas with a volume of 7.0 mL & pressure of gas is compressed to 2.7 mL at constant temp and 1.68 atm?

• 4.4 atm

• 11.25 atm

• 0.648 atm

• 31.752 atm

An 11.2 L-sample contains 0.5 moles of N2. At same pressure & temp., how many moles of gas would be in a 20-L sample?

a. 448 moles N2

b. 0.89 moles N2

c. 0.0022 moles N2

d. 112 moles N2

• 448 moles N2

• 0.89 moles N2

• 0.0022 moles N2

• 112 moles N2

Chlorine gas and fluorine gas will combine to form one gaseous product. One L of Cl2 reacts with 3 L of F2 to produce 2 L of product. assuming constant temperature and pressure condition, what is the formula of the product?

• ClF

• ClF2

• (Cl2)F

• ClF3

A mixture of helium and neon gases has a total pressure of 1.2 atm. if the mixture contains twice as many moles of helium as neon, what is the partial pressure due to neon?

• 0.2 atm

• 0.3 atm

• 0.4 atm

• 0.8 atm