What is the volume of a 7.75 g sample of carbon monoxide gas at a temperature of -19.7 ^{o}C and a pressure of 764.7 mmHg?

What is the pressure exerted by 2.48 g of nitrogen with a volume of 2925.6 mL at a temperature of 22.3^{o}C?

1st Question)

Use the ideal gas equation: PV = nRT

Isolate Volume in the equation: V = nRT/P

Convert grams of Carbon Monoxide gas to moles: 7.75 g / 28.01 g/mole = 0.2767 moles CO

Convert Celsius to Kelvin: -19.7 C = 253.45 Kelvin

Convert mmHg to Atm: 764.7 mmHg = 1.006 atm

R is the constant, R = 0.08206

Plug in everything to V = nRT/P

V = (0.2767*0.08206*253.45) / (1.006)

Volume is 5.719 Liters CO (g)

2nd Question)

Isolate Presssure in the equation: P = nRT/V

Convert grams of Nitrogen gas to moles: 2.48 g / 28.01 g/mole = 0.0885 moles N2

Convert Celsius to Kelvin: 22.3 C = 295.45 Kelvin

Convert mL to Liters: 2925.6 mL = 2.9256 L

Plug in everything to P = nRT/V

P = (0.0885*0.08206*295.45) / (2.9256)

Pressure is 0.733 Atm N2 (g)

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