The forward reaction in this equilibrium is endothermic
COCl$_2$(g) $\rightleftharpoons$ CO(g) + Cl$_2$(g)
Which statement is correct?
1 )
If the total pressure is increased at constant temperature, the proportion of COCl$_2$ in the equilibrium mixture will decrease
2 )
Use of a catalyst will increase the proportion of COCl$_2$ in the equilibrium mixture at constant temperature and pressure
3 )
Reducing the equilibrium concentration of CO will increase the value of the equilibrium constant
Raising the temperature from 373 K to 473 K will increase the value of the equilibrium constant
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