At 100°C, 1.00 mol of liquid water is allowed to expand isothermally into an evacuated vessel of such a volume that the final pressure is 0.500 atm. The amount of heat absorbed in the process was found to be 30.0 kJ/mol. Assume ideal behaviour of the gas.
What are w, ΔU, ΔH, ΔS, and ΔG
Data:
ΔvapH = 40600 J/mol (at 1.00 atm)
Hint: Employ a step-wise approach to be able to use the given data at the provided pressure.
At 100°C, 1.00 mol of liquid water is allowed to expand isothermally into an evacuated vessel...
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The Standard enthalpy of vaporization of water at 100.0
oC is 40.66 KJ*mol-1. The Cp,m
values for the liquid and the vapor water are, respectively, 75.3
and 33.58 J*K-1*mol-1. Assume that the heat
capacities are independent of temperature, and that the vapor
behaves as an ideal gas.
a) Calculate
sys in taking one mole of liquid water at 25.0
oC and 1.00 atm to gaseous water at 95.0 oC
and 0.500 atm.
b) Assume that the temperature and pressure of...
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I
need help figuring out #5.35, 5.37, 5.45, 5.57, and 5.71
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