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# If Q$/{{\text{K}}_{\text{c}}}>1$ , then the reaction proceeds left to right but if Q$/{{\text{K}}_{\text{c}}}>1$, then the reaction proceeds right to left. If true enter 1, false enter 0.

Last updated date: 13th Jun 2024
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Hint:Check for the value of reaction quotient Q. If it is less than ${{\text{K}}_{\text{c}}}$, then the reaction proceeds in the forward direction.

When Q/${{\text{K}}_{\text{c}}}$ is less than one, it means value of ${{\text{K}}_{\text{c}}}$ is more than Q which means the concentration of products is lower than the equilibrium concentration. So, the equilibrium will shift in the forward direction i.e. from left to right.
And when by Q$/{{\text{K}}_{\text{c}}}>1$,, it means the value of ${{\text{K}}_{\text{c}}}$ is less than Q so that concentration of products is more than the equilibrium concentration. So, to attain equilibrium the reaction will proceed in a backward direction that is from right to left.
Q can be used to determine in which direction a reaction will shift to reach equilibrium if ${{\text{K}}_{\text{c}}}>1$ the reaction will proceed in the reverse direction, i.e. converting products into reactants. If Q = ${{\text{K}}_{\text{c}}}$ then the system is already at equilibrium.
The value of ${{\text{K}}_{\text{c}}}$,the equilibrium constant may depend on the temperature but not on the amount of the compound and nor on the pressure. The value of Q depends only on the partial pressure and the concentrations. If there is a change in either Q or ${{\text{K}}_{\text{c}}}$ the reaction will go in the direction which will re-establish the condition of the reaction quotient being equal to equilibrium constant.