question archive Knowing the following data: R = 0
Knowing the following data: R = 0
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Knowing the following data:
R = 0.0083145 kJ/mol K
ΔH = -41.2 kJ/mol
ΔS = -0.135 kJ/mol K
Determine ΔG (in kJ/mol) at 198.3 K when:
[H2] = 2.35 M
[CO2] = 2.66 M
[CO] = 0.673 M
[H2O] = 0.185 M
Here is the reaction:
CO (g) + H2O (g) ? CO2 (g) + H2 (g)
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Answer- ΔG = -14.4295 kJ/mol
?ΔG is negative, means the reaction is spontaneous
ΔG is calculated using formula,
ΔG = ΔH-TΔS
Where
ΔG = change in free energy
ΔH = change in enthalpy
ΔS = change in entropy
T = temperature
Please see the attached file for the complete solution
