Question

A 0.245-L flask contains 0.467 mol co2 at 159 °c. Calculate the pressure using the ideal gas law.

Answer 1

Answer:

Pressure, P = 67.57 atm

Explanation:

Given the following data;

• Volume = 0.245 L
• Number of moles = 0.467 moles
• Temperature = 159°C
• Ideal gas constant, R = 0.08206 L·atm/mol·K

Conversion:

We would convert the value of the temperature in Celsius to Kelvin.

T = 273 + °C

T = 273 + 159

T = 432 Kelvin

To find the pressure of the gas, we would use the ideal gas law;

PV = nRT

Where;

• P is the pressure.
• V is the volume.
• n is the number of moles of substance.
• R is the ideal gas constant.
• T is the temperature.

Making P the subject of formula, we have;

$P = \frac {nRT}{V}$

Substituting into the formula, we have;

$P = \frac {0.467*0.08206*432}{0.245}$

$P = \frac {16.5551}{0.245}$

Pressure, P = 67.57 atm