Question

Calculate the entropy change ∆S per mole for following reaction. Cumbustion of Hydrogen in a
fuel cell at 298K.



●H2
(g)+
½O2
(g) − → H2O(g)[∆H = 241.60KJ, ∆G= 288.40KJ]​

Answer 1

Answer:

ΔG = ΔH - TΔS

Putting in the values,

−288.40 = −241.6 − 298 × ΔS

$ΔS = \frac{ - 288.4 + 241.6}{ - 298}$

= 0.157 kJ K−¹ mol−¹

Answer 2

Answer:

AG AH-TAS

Putting in the values,

-288.40=-241.6 - 298 × AS

AS -288.4+241.6 -298

= 0.157 kJ K-¹ mol-¹