1.00 mol of oxygen gas (O₂) is heated at constant pressure of 1.00 atm from 10.0°C to 25.0°C. From the first law, calculate the change of internal energy of the gas in this process. A) 312 J B) 291 J C) 365 J D) 155 J

Question

Quizplus · Accepted Answer

The change in internal energy for an ideal gas at constant pressure is given by:ΔU = nCvΔTwhere n is the number of moles of gas, Cv is the molar specific heat at constant volume, and ΔT is the change in temperature.For oxygen gas, Cv = 20.9 J/mol·K. Therefore,ΔU = (1.00 mol)(20.9 J/mol·K)(25.0°C - 10.0°C) = 312 J

100 Mol of Oxygen Gas (O2) Is Heated at Constant

100 Mol of Oxygen Gas (O₂) Is Heated at Constant