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    E(g) + 2F(g) 2G(g) ΔH = –50 kJ mol–1

    The mixture in Question 1 (c) was allowed to reach equilibrium at temperature T2 in the original container of volume 1.50 dm3. The value of Kc for the equilibrium was found to have increased. State and explain which of T1 or T2 is the higher temperature.

    I answered as T1 but idk why it's right, I know a higher Kc means more product so T2 is endothermic in the forward. If the forward of a reaction is endothermic and the forward of another is exothermic does that mean the exothermic has a higher temperature?
 
 
 
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