Medium
The reaction $CaCO_3 \rightleftharpoons CaO + CO_{2(g)}$ goes to completion in a lime kiln because:
- AOf the high temperature
- B$CaO$ is more stable than $CaCO_3$
- C$CaO$ is not dissociated
- D$CO_2$ escapes continuously
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For the following reaction,which change will shift the equilibrium towards the product?
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$I_{2(g)} \rightleftharpoons 2I_{(g)}; \Delta H_r^o(298 \ K) = +150 \ kJ$
Raising the temperature of an equilibrium system:
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