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Consider the following reaction N2O4(g) 2NO2(g); Hb0 = +58 kJ For each of the following cases (a, b), the direction in which equilibrium shifts is: (a) Temperature is decreased (b) Pressure is increased by adding N2 at constant T
- (a) towards reactant, (b) no change
- (a) towards product, (b) towards reactant
- (a) towards product, (b) no change
- (a) towards reactant, (b) towards product
Correct answer: (a) towards reactant, (b) no change
Solution
When the temperature is decreased, the equilibrium shifts towards the reactants to produce heat, as the reaction is endothermic. Increasing pressure by adding N2 does not affect the equilibrium since it does not change the total number of gas molecules in the reaction.
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