5.00 moles of CO2(g) is in a rigid container with a volume of 3.00 liters. The i

Question

5.00 moles of CO2(g) is in a rigid container with a volume of 3.00 liters. The initial
temperature is 291 K and the initial pressure is 33.3 bar. Then 4.95 kJ of energy is added to
the gas as heat; this raises the temperature to 325 K and raises the pressure to 38.3 bar.
CO2(g) can NOT be treated as an ideal gas under these conditions.
[6] Calculate )U and )H for the system during this process

Explanation / Answer

CH4 (g) + 2O2(g) --> CO2(g) + 2H20(l); dH reaction = (dHf products) - (dHf reactants) dH reaction = [CO2 & 2 H2O)] - [CH4 & 2 O2)] -889.1 = [-393.3 & 2(-285.8)] - [CH4 & 2(zero)] -889.1 = (-964.9) - CH4 CH4 = (-964.9) + 889.1 dHf of CH4(g) = - 75.8 kJ/mol

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