What weight of nitrogen gas will occupy a volume of 1.25 L at a pressure of 1.0 atm and a temperature of 200.°C?

Question

Quizplus · Accepted Answer

To solve this, we can use the ideal gas law equation: PV = nRT, where P is the pressure in atmospheres (atm), V is the volume in liters (L), n is the number of moles of gas, R is the ideal gas constant (0.0821 L·atm/mol·K), and T is the temperature in Kelvin (K). First, convert the temperature from Celsius to Kelvin: T = 200°C + 273 = 473K. Then, solve for n (moles of nitrogen gas): n = PV / RT = (1.0 atm)(1.25 L) / (0.0821 L·atm/mol·K)(473K) ≈ 0.032 moles. The molar mass of nitrogen gas (N2) is approximately 28 g/mol, so the weight of the nitrogen gas is: weight = n × molar mass = 0.032 moles × 28 g/mol ≈ 0.90 g.

What Weight of Nitrogen Gas Will Occupy a Volume of 1.25