What is the value of the equilibrium constant, K, for an equilibrium reaction occurring at 58.0 degrees Celsius given that the value of deltaS is 126.98 J/mol and the value of deltaH is 176.93 kJ/mol?
G =
H -
T
S
= 176.93 kJ/ mol - 331*0.12698 kJ/ mol
= -154.19 kJ/ mol
= -154.19 *103 J/mol
G = -RTlnK
K = -G/ RT = 154.19
*103 J mol-1/ 331 * 8.315
JK-1mol-1
= 154.19 *103 J mol-1 /2751.93
= 56.03
value of equilibrium constant = 56.03
What is the value of the equilibrium constant, K, for an equilibrium reaction occurring at 58.0...
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