Final answer:
The pressure for 0.387 mole of nitrogen gas at 56.0 °C occupying 5.85 L can be calculated with the ideal gas law PV = nRT, with the given values leading to solving for P using the temperature in Kelvin and the number of moles, volume, and the constant R.
Step-by-step explanation:
The pressure at which 0.387 mole of nitrogen gas at 56.0 °C would occupy 5.85 L can be calculated using the ideal gas law, which is PV = nRT, where P is pressure, V is volume, n is the number of moles of the gas, R is the ideal gas constant (0.0821 L.atm.mol⁻¹.K⁻¹), and T is the temperature in Kelvin.
First, convert the temperature from Celsius to Kelvin by adding 273.15: 56.0 °C + 273.15 = 329.15 K. Then, rearrange the ideal gas law to solve for pressure: P = (nRT) / V.
Using the values provided: P = (0.387 mol)(0.0821 L.atm.mol⁻¹.K⁻¹)(329.15 K) / 5.85 L