what is the basic and functional diff between Q_{c }and K_{c }? where Q_c and K_c is defined in the same way

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. At ${445}^{\circ }C,K_c$ for the following reaction is 0.020.
$2HI\left(g\right)\rightleftharpoons H_2\left(g\right)+I_2\left(g\right)$
A mixture of $H_2,I_2$, and HI in a vessel at ${445}^{\circ }C$ has the following concentrations: $\left[HI\right]=2.0M,\left[H_2\right]=0.50Mand\left[I_2\right]=0.10M$. Which one of the following statements concerning the reaction quotient, $Q_c$, is TRUE for the above system?

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