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

To solve this, let's assume ideal gas behavior.

PV=nRT

Let's solve for n. Convert units to SI units first.

Pressure = 833 torr (101325 Pa/760 torr) = 111,057.53 Pa

Volume = 250 mL (1 L/1000 mL) (1 m³/1000 L) = 2.5*10⁻⁴ m³

Temperature = 42.4 + 273 = 315.4 K

n = (8,314 J/mol·K) (315.4 K) / (111057.53 Pa) (2.5*10⁻⁴ m³)

n = 94.45 mol

The molar mass of ammonia is 17.031 g/mol.

Mass = 94.45*17.031 = 1,608.51 g ammonia