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7 October, 17:17

If under a given set of conditions the reaction?→? A→B occurs with Δ?=-14 kJ/mol,ΔG=-14 kJ/mol, and the reaction?→? C→B occurs with Δ?=+16 kJ/molΔG=+16 kJ/mol, then

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  1. 7 October, 19:27
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    Reaction A to B is feasible and exothermic, C to B is not feasible and would be endothermic, given this, the reaction that is feasible is B to C, because the opposite direction of the reaction changes the sign of ΔG and ΔH.

    Explanation:

    When ΔG 0, the reaction cannot occur.

    When ΔH 0, it meas that the reaction is endothermic, so it needs energy to be feasible.
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