Easy
For the following balanced reaction occurring at a constant temperature,what will be the change in the concentration of $CO$ if the volume of the system is decreased?
$2CO_{(g)} \rightleftharpoons O_{2(g)} + 2CO_{2(g)}$
$2CO_{(g)} \rightleftharpoons O_{2(g)} + 2CO_{2(g)}$
- AIt will increase.
- BIt will decrease.
- CIt will remain constant.
- DIt will become zero.
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On heating a mixture of $SO_2Cl_2$ and $CO$,two equilibria are simultaneously established: $SO_2Cl_{2(g)} \rightleftharpoons SO_{2(g)} + Cl_{2(g)}$ and $CO_{(g)} + Cl_{2(g)} \rightleftharpoons COCl_{2(g)}$. On adding more $SO_2$ at equilibrium,what will happen?
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View SolutionDescribe the effect of:
$(a)$ Addition of $H_2$
$(b)$ Addition of $CH_3OH$
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$(d)$ Removal of $CH_3OH$ on the equilibrium of the reaction:
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