JEE MAIN - Chemistry (2018 - 15th April Evening Slot - No. 18)
At a certain temperature in a $$5$$ $$L$$ vessel, 2 moles of carbon monoxide and 3 moles of chlorine were allowed to reach equilibrium according to the reaction,
CO + Cl2 $$\rightleftharpoons$$ COCl2
At equilibrium, if one mole of CO is present then equilibrium constant (Kc) for the reaction is :
CO + Cl2 $$\rightleftharpoons$$ COCl2
At equilibrium, if one mole of CO is present then equilibrium constant (Kc) for the reaction is :
2
2.5
3
4
Explanation
| CO | + | Cl2 | $$\rightleftharpoons$$ | COCl2 | |
|---|---|---|---|---|---|
| Initially number of moles | 2 | 3 | 0 | ||
| At equilibrium number of moles | 1 | 2 | 1 |
The equilibrium constant,
Kc = $${{\left[ {COC{l_2}} \right]} \over {\left[ {CO} \right]\left[ {C{l_2}} \right]}}$$
= $${{\left( {{1 \over 5}} \right)} \over {\left( {{1 \over 5}} \right) \times \left( {{2 \over 5}} \right)}}$$
= $${5 \over 2}$$
= 2.5
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