# 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 25oC?

## Q2.

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

## Q3.

At 1 atm of pressure water boils at 100oC, 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 25oC?

## 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 28oC 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 30oC?

## 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 72oC and 2 atm?

## Q13.

After eating beans, a student collects a sample of gas at 0.97 atm and 26oC 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 25oC. 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 28oC 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 28oC 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 25oC. 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).