The reaction quotient $Q_{C}$ is useful in predicting the direction of the reaction. Which of the following is incorrect?

For the following reaction,the equilibrium constant $K_{c}$ at $298 \ K$ is $1.6 \times 10^{17}$.
$Fe^{2+}_{(aq)} + S^{2-}_{(aq)} \rightleftharpoons FeS_{(s)}$
When equal volumes of $0.06 \ M \ Fe^{2+}_{(aq)}$ and $0.2 \ M \ S^{2-}_{(aq)}$ solutions are mixed,the equilibrium concentration of $Fe^{2+}_{(aq)}$ is found to be $Y \times 10^{-17} \ M$. The value of $Y$ is. . . . .

The equilibrium constants of the following are
$N_2 + 3H_2 \rightleftharpoons 2NH_3 \,; \quad K_1$
$N_2 + O_2 \rightleftharpoons 2NO \,; \quad K_2$
$H_2 + \frac{1}{2} O_2 \rightleftharpoons H_2O \,; \quad K_3$
The equilibrium constant $(K)$ of the reaction:
$2NH_3 + \frac{5}{2} O_2 \rightleftharpoons 2NO + 3H_2O$ is:

For the reaction $I_{2(g)} \rightleftharpoons 2I_{(g)}$,the equilibrium constant $K_c$ at $1000 \ K$ is $10^{-6}$. If $1 \ mol$ of $I_2$ is added to a $1 \ L$ container,which of the following statements is true at equilibrium?

Calculate $\Delta G^o$ (in $kcal/mole$) for the decomposition of $Cl_{2(g)} \rightleftharpoons 2Cl_{(g)}$,if chlorine molecules are $50\%$ dissociated at $1000 \ K$ at a pressure of $15 \ atm$ at equilibrium $(\ln \ 20 = 2.99)$.

$A$ gaseous reaction $A_{2(g)} \to B_{(g)} + \frac{1}{2} C_{(g)}$ shows an increase in pressure from $100 \ mm$ of $Hg$ to $120 \ mm$ of $Hg$ in $5 \ min$. What will be the rate of disappearance of $A_2$ in $mm$ of $Hg/min$?