What is the volume of a 7.75 g sample of carbon monoxide gas at a temperature of -19.7 oC 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 22.3oC?
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)
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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