Predict how the value of the equilibrium constant of the reaction below changes

Question

Predict how the value of the equilibrium constant of the reaction below changes with increasing temperature. 2H2 (g) + O2 (g) 2H2O(g) kJ mol AH-241.8 rxn Choose one: K increases since it is exothermic to the right and this will generate heat to increase the temperature. K decreases since the higher energy favors the reactants which contain more energy. 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. 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. There is no change in the equilibrium; the reaction just goes faster. O It is impossible to say without further information.

Explanation / Answer

1.

(b) K decreases since the forward reaction is exothermic increase in temperature favours endothermic reaction i.e backward reaction in this case and hence K decreases.

2.

PART(1)

Kc1 = (1/2) * Kc = (1/2) * 2.37 * 10-3 = 1.185 * 10-3

PART (2)

Kc2 = 1 / Kc = 1 / ( 2.37 * 10-3) = 4.22 * 102

PART (3)

Kc3 = (1/2)*Kc2 = (1/2)*4.22 * 102 = 2.11 * 102

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