A 250.0-mL sample of ammonia, NH₃(g), exerts a pressure of 833 torr at 42.4$\degree$C. What mass of ammonia is in the container?

Question

Quizplus · Accepted Answer

Using the ideal gas law, PV = nRT, convert pressure to atm (833 torr = 1.096 atm), volume to liters (0.250 L), and temperature to Kelvin (315.55 K). Solve for n (moles of NH3), then multiply by the molar mass of NH3 (17.03 g/mol) to find the mass.

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