if I have 22.1 grams of CO2 gas at - 188 degrees Celsius and 165 ml what is the pressure of the gas in kPa

P = 2.145kPa

Explanation:

Mass = 22.1g

Molar mass of CO2 = 44g/mol

Vol = 165mL = 0.165L

T = - 188°C = (-188 + 273.15) K = 85.15K

R = 8.314J/mol. K

From ideal gas equation,

PV = nRT

P = pressure of the ideal gas

V = volume the gas occupies

n = number of moles if the gas

R = ideal gas constant

T = temperature of the gas

n = number of moles

n = mass / molar mass

n = 22.1 / 44 = 0.50moles

PV = nRT

P = nRT / V

P = (0.5 * 8.314 * 85.15) / 0.165

P = 2145.26Pa = 2.145kPa

Pressure of the gas is 2.145kPa