How do you calculate the change in Gibbs free energy (∆G) for the following reactions at 25 °C?

#Ca(s) + 2H_2O(l) → Ca(OH)_2(s) + H_2(g)#
∆H = -411.6 kJ/mol
∆S = 31.8 J/mol∙K?

1 Answer
Apr 25, 2016

Answer:

You can do it like this:

Explanation:

Use this relationship which arises from the 2nd law of thermodynamics:

#DeltaG=DeltaH-TDeltaS#

#DeltaH# is the enthalpy change

#T# is the absolute temperature

#DeltaS# is the entropy change

Putting in the values:

#DeltaG=-411xx10^(3)-(298xx31.8)#

#DeltaG=-411xx10^(3)-(9.476xx10^(3))#

#DeltaG=-421.07" ""kJ/mol"#