A reaction with reaction equilibrium qotient Q_c and equilibrium constant K_c,will proceed in the direction of the product when

a. Q_c=K_c

b Q_cc

c Q_cK_c

d Q_c=0

Q. A reaction with reaction quotient $Q_C$ and equilibrium constant $K_C$, will proceed in the direction of the products when:

Q. Assertion :Assertion : If reaction quotient, $Q_c$ for a particular reaction is greater than $K_c$ the reaction will proceed in the direction of reactants. Reason: Reason : Reaction quotient is defined in the same way as the equilibrium constant $K_c$ except that the concentrations in $Q_c$ are not necessarily equilibrium values.

Q. Assertion :Reaction quotient is defined in the same way as equilibrium constant at any stage of the reaction. Reason: If $Q_c$ (reaction quotient) $<K_c$ (equilibrium constant reaction moves in direction of reactants).

Q. In the reaction $R\left(g\right)\rightleftharpoons P\left(g\right)$
In which of the following conditions the reaction will move towards backward direction to attain equilibrium?
Here $Q_c$ is the reaction quotient at a given time t and $K_c$ is the equilibrium contsnt

Q. Consider the following reaction and its equilibrium constant:
$N_2{O}_4\left(g\right)\rightleftharpoons 2N{O}_2\left(g\right)Kc=5.85\times {10}^{-3}$

A reaction mixture at a particular time, t contains: $\left[N{O}_2\right]=0.025Mand\left[N_2{O}_4\right]=0.033M.$ Calculate $Qc$, and determine the direction in which the reaction will proceed.