If a 7.00 gram sample of molecular nitrogen at 10. °C occupies 2.50 L, what is the pressure of the sample?
A) 1.28 atm
B) 2.32 atm
C) 2.56 atm
D) 4.65 atm

Question

Quizplus · Accepted Answer

Using the ideal gas law, PV = nRT, where n = mass/molar mass. For N2, molar mass = 28.02 g/mol. Calculate n = 7.00 g / 28.02 g/mol = 0.25 mol. Convert temperature to Kelvin: 10°C = 283 K. Use R = 0.0821 L·atm/mol·K. Solve for P: P = nRT/V = (0.25 mol)(0.0821 L·atm/mol·K)(283 K) / 2.50 L = 2.32 atm.

If a 700 Gram Sample of Molecular Nitrogen at 10