For the vaporization of water at 1.00 atm, $\Delta$ H = 43.54 kJ/mol at 298 K and $\Delta$ H = 40.68 kJ/mol at 373 K
The constant-pressure heat capacity of liquid water is 75.3 J/mol • K. Calculate the constant-pressure heat capacity for H₂O(g) .

Question

For the vaporization of water at 1.00 atm,

\Delta

H = 43.54 kJ/mol at 298 K and

\Delta

H = 40.68 kJ/mol at 373 K
The constant-pressure heat capacity of liquid water is 75.3 J/mol • K. Calculate the constant-pressure heat capacity for H₂O(g) .

Quizplus · Accepted Answer

The Answer of For the vaporization of water at 1.00 atm, $\Delta$H = 43.54 kJ/mol at 298 K and $\Delta$H = 40.68 kJ/mol at 373 K The constant-pressure heat capacity of liquid water is 75.3 J/mol • K. Calculate the constant-pressure heat capacity for H₂O(g).

For the Vaporization of Water at 1 Δ\DeltaΔ H = 4354 KJ/mol at 298 K And 1.00

For the Vaporization of Water at 1 $\Delta$ H = 4354 KJ/mol at 298 K And 1.00