If a 4.00 L container is filled with N₂ to a pressure of 895 torr at 53.0$\degree$C, calculate the mass of the nitrogen in the container.

Question

Quizplus · Accepted Answer

Using the ideal gas law, PV = nRT, we can solve for n (moles of N2). Convert pressure to atm (895 torr = 1.177 atm) and temperature to Kelvin (53°C = 326 K). R = 0.0821 L·atm/mol·K. n = (1.177 atm * 4.00 L) / (0.0821 L·atm/mol·K * 326 K) = 0.176 mol. The molar mass of N2 is 28.02 g/mol, so mass = 0.176 mol * 28.02 g/mol = 4.93 g.

If a 400 L Container Is Filled with N2 to a Pressure

If a 400 L Container Is Filled with N₂ to a Pressure