# Gas Laws 1 (Worksheet)

#### Q1.

A sample of 0.50 moles of gas is placed in a container of volume of 2.5 L. What is the pressure of the gas in torr if the gas is at 25^{o}C?

#### Q2.

A sample of gas is placed in a container at 25^{o}C and 2 atm of pressure. If the temperature is raised to 50^{o}C, what is the new pressure?

#### Q3.

At 1 atm of pressure water boils at 100^{o}C, if the sample was placed under 2 atm of pressure, what would be the temperature? (This would be like a pressure cooker).

#### Q4.

At what temperature would water boil if the pressure is 600 torr? (Use information from problem 3: this shows why food doesn't cook well at higher elevations)

#### Q5.

Calculate the volume of 40.6 g of \(F_2\) at STP.

#### Q6.

A sample of 2.0 moles of hydrogen gas is placed in a container with a volume of 10.4 L. What is the pressure of the gas in torr if the gas is at 25^{o}C?

#### Q7.

The tire pressure is 32 psi. What is the pressure in torr if 1 atm = 14.7 psi?

#### Q8.

A gas is placed in a balloon with a volume of 3.0 L at 28^{o}C and 900 torr. What would be the new volume for the gas if placed under STP?

#### Q9.

How many moles of gas would occupy a volume of 14 L at a pressure of 700 torr and a temperature of 30^{o}C?

#### Q10.

Calculate the volume of 24.0 g of \(HCl\) at STP.

#### Q11.

What is the volume of one mole of acetylene gas at STP?

#### Q12.

What is the volume of 0.75 mol of gas at 72^{o}C and 2 atm?

#### Q13.

After eating beans, a student collects a sample of gas at 0.97 atm and 26^{o}C which occupies a volume of 3.5 L, calculate its volume at STP.

#### Q14.

Ammonia \(NH_3\) is placed in 1.5 L flask at 25^{o}C. If the pressure of the gas is 0.899 atm, what is the density?

#### Q15.

A mixture of \(Ar\) and \(CO\) gases is collected over water at 28^{o}C and an atmospheric pressure of 1.05 atm. If the partial pressure of \(Ar\) is 600 torr, what is the partial pressure of \(CO\)? (vapor pressure of water at 28^{o}C is 28.3 mmHg)

#### Q16.

Determine the partial pressures of each of the gases in the following mixture: 17.04 g \(NH_3\), 40.36 g \(Ne\) and 19.00 g \(F_2\). The gases are at 1.5 atm of pressure.

#### Q17.

Potassium chlorate decomposes under heat as follows:

\[2KClO_{3\,(s)} \rightarrow 2KCl_{(s)} + 3O_{2\,(g)}\]

The oxygen gas is collected over water at 25^{o}C. The volume of gas is 560 mL measured at 1 atm. Calculate the number of grams of \(KClO_3\) used in the reaction (vapor pressure of water = 0.0313 atm).