# Gases I (Worksheet)

- Page ID
- 20057

## Q1.

The typical atmospheric pressure on top of Mt. Everest is about 265 torr. Convert this pressure to:

- atm
- mmHg
- pascals

## Q2.

A fixed quantity of gas at 23°C exhibits a pressure of 735 torr and occupies a volume of 5.22 L

- Calculate the volume the gas will occupy if the pressure is increased to 1.88 atm while temp is held constant.
- Calculate the volume the gas will occupy if the temperature is increased to 165 °C while the pressure is held constant.

## Q3.

Calculate the number of molecules in a deep breath of air whose volume is 2.50L at body temperature, 37°C and a pressure of 735 torr.

## Q4.

A scuba diver’s tank contains 0.29 kg of \(O_2\) compressed into a volume of 2.3 L.

- Calculate the gas pressure inside the tank at 9°C
- What volume would this oxygen occupy at 26°C and 0.95 atm?

## Q5.

A mixture containing 0,538 mol He (g), 0.315 mol Ne (g), and 0.103 mol Ar (g) is confined in a 7.00 L vessel at 25°C.

- Calculate the partial pressure of each of the gases in the mixture
- Calculate the total pressure

## Q6.

A sample of 4.00 mL of diethylether (\(C_2H_5OC_2H_5\), density = 0.7134 g/mL) is introduced into a 5.00 L vessel that already contains a mixture of \(N_2\) and \(O_2\), whose partial pressures are \(pN_2 = 0.715 \; atm\) and \(pO_2 = 0.208\; atm\). The temperature is held at 35.0 °C and the diethylether totally evaporates.

- Calculate the partial pressure of the diethylether.
- Calculate the total pressure of the container.