A 250.0-mL sample of ammonia, NH₃(g), exerts a pressure of 833 torr at 42.4°C. What mass of ammonia is in the container? (R = 0.08206 L • atm/K • mol, 1 atm = 760 torr)

Question

Quizplus · Accepted Answer

First, convert the pressure from torr to atm: 833 torr * (1 atm / 760 torr) = 1.096 atm. Convert the temperature to Kelvin: 42.4°C + 273.15 = 315.55 K. Use the ideal gas law: PV = nRT. Solve for n (moles of NH3): n = PV / RT = (1.096 atm * 0.250 L) / (0.08206 L•atm/K•mol * 315.55 K) = 0.01057 mol. The molar mass of NH3 is 17.03 g/mol, so the mass is 0.01057 mol * 17.03 g/mol = 0.180 g.

A 2500-ML Sample of Ammonia, NH3(g), Exerts a Pressure of 833

A 2500-ML Sample of Ammonia, NH₃(g), Exerts a Pressure of 833