CCC Matter and Energy The dashed curve shows
1 answer:
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Answer:
a) Equilibrium will shift to the left i.e. reactants
b) K will increase with increase in temperature
Explanation:
The given reaction is:
C6H12O6 + 6 O2 ↔ 6 CO2 + 6 H2O ΔH = -2816 kJ/mol
a) As per Le Chatelier's principle, for a reaction at equilibrium any changes in temperature, pressure or concentration will shift the equilibrium in a direction so as to undo the effect of the induced change.
The given reaction is exothermic (since ΔH is negative) i.e. it accompanied by the release of heat and hence an increase in temperature. Therefore, if the temperature is increased the equilibrium will shift in the opposite direction i.e. towards the left or towards the reactants.
b) The equilibrium constant (K) and temperature T are related via the Van't Hoff equation:
In the given reaction, ΔH is negative and the condition is T2>T1
Therefore, K2 > K1
The value of equilibrium constant will increase with increase in temperature
