if the free energy change G for a reaction is -146.11Kj/mol the reaction is
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If the ΔG (change in Gibbs Free Energy) of the reaction was -31.45 kJoules, you would know that the reaction is spontaneous, releasing energy. The products have more free energy than the reactants. The reaction most likely is coupled to another exergonic reaction. The reaction requires an energy input of 31.45 kJoules to produce a product.
Anna D.
If the of a reaction is -40.0 KJ/mol and the is -140.0 J/mol-K at 298 K. Then at 298 K, will the reaction be spontaneous or non-spontaneous?
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The change in the free energy under standard conditions is -55.9 kJ/mol. Is this reaction spontaneous as written under standard conditions?
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