If 1.00 mol of oxygen is heated at constant pressure of 1.00 atm from 10.0$^{\circ}$C to 25.0$^{\circ}$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 of 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, Cv = 20.8 J/mol·K. Therefore,ΔU = (1.00 mol)(20.8 J/mol·K)(25.0°C - 10.0°C) = 312 J

If 100 Mol of Oxygen Is Heated at Constant Pressure of of 1.00