Step 1
At constant temperature and pressure, the change in Gibbs free energy is defined as ΔG = ΔH − T ΔS
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Step 2
When ΔG < 0 (negative) the reaction will proceed spontaneously
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Step 3
Information provided:
Delta H = ΔH = - 57.2KJ
Delta S = ΔS = - 0.176 KJ/K
T = 25 °C + 273 = 298 K
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Step 4
Procedue:
ΔG = ΔH − T ΔS = -57.2 kJ - (-0.176 kJ/K) x 298 K = - 4.752 kJ
Therefore, the reaction will occur spontaneously.
Answer: Yes, it wil (because of the procedure)
