9. Calculate ΔG0 at 820C for reactions in which
(a) ΔH0= 293 kJ; ΔS0 = -695 J/K
(b) ΔH0= -1137 kJ; ΔS0= 0.496 kJ/K
G^{0} = H^{0} -TS^{0}
We use this formula for both the below questions
T = 82^{0}C = (82+273)K = 355K
(a) H^{0} = 293kJ = 293000J [Since 1kJ = 1000J]
G^{0} = H^{0} -TS^{0}
G^{0} = 293000J - (355K x -695J/K)
G^{0} = 293000J + 246725J = 539725J
(b) H^{0} = -1137kJ
G^{0} = H^{0} -TS^{0}
G^{0} = -1137kJ - (355K x 0.496kJ/K)
G^{0} = -1137kJ - 176.08kJ
G^{0} = 1313.08kJ = 131080J
9. Calculate ΔG0 at 820C for reactions in which (a) ΔH0= 293 kJ; ΔS0 = -695...
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