Consider the following exothermic reaction \(2SO_{2(g)} + O_{2(g)} = 2SO_{3(g)}\) . If the temperature of the reaction is reduced from 800ºC to 500ºC, and no other change takes place, then
the reaction rate increases
concentration of SO3 decreases
concentration of SO3 increases
SO2 gas becomes unreactive
O2 gas becomes unreactive
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the increase in the temperature of the system favours the reactant side yl decreases favours the product side
For an exothermic reaction the forward reaction is exothermic and is favoured by decrease in temperature.while the backward reaction is endothermic and is favoured by increase in temperature
An exothermic reaction releases heat, so adding heat will give more heat to be released and reducing it will do the opposite.
in d conditions stated i.e 2 moles of SO3 frm 3 moles of SO2 n O2, a decrease in temp. favours d forward rxtn being an exothermic system
