Predict how the value of the equilibrium constant of the reaction below changes with increasing temperature. 2H2(g)+O2(g)⇌2H2O(g) $$ΔH°rxn=−241.8 kJmol
Predict how the value of the equilibrium constant of the reaction below changes with increasing temperature.
Choose one:
A. K increases since it is exothermic to the right and this will generate heat to increase the temperature.
B. K decreases since the higher energy favors the reactants which contain more energy.
C. K decreases since there are 3 moles of gas on the left compared to 2 moles of gas on the right, and an increasing temperature means an increasing number of moles of gas.
D. K increases since there are 2 moles of gas on the right compared to 3 moles of gas on the left, and an increasing temperature requires a decreasing number of moles of gas.
E. There is no change in the equilibrium; the reaction just goes faster.
F. It is impossible to say without further information.
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