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? A)0.0787 g B)0.180 g C)8.04 g D)17.0 g E)59.8 g

Question

Quizplus · Accepted Answer

To find the mass of ammonia, use the ideal gas law: PV = nRT. Convert pressure to atm (833 torr = 1.096 atm), volume to liters (250.0 mL = 0.250 L), and temperature to Kelvin (42.4°C = 315.55 K). R is 0.0821 L·atm/mol·K. Solve for n (moles of NH3): n = PV/RT = (1.096 atm)(0.250 L) / (0.0821 L·atm/mol·K)(315.55 K) = 0.0106 mol. The molar mass of NH3 is 17.03 g/mol, so mass = n × molar mass = 0.0106 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