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Which of the following changes will shift the reaction towards the product?
$I_{2(g)} \rightleftharpoons 2I_{(g)}$ $\Delta H_r^o(298 \ K) = +150 \ kJ$
$I_{2(g)} \rightleftharpoons 2I_{(g)}$ $\Delta H_r^o(298 \ K) = +150 \ kJ$
- AIncrease in concentration of $I$
- BDecrease in concentration of $I_2$
- CIncrease in temperature
- DIncrease in total pressure
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