In the reaction $CH_3COOH + C_2H_5OH \rightleftharpoons CH_3COOC_2H_5 + H_2O$,one mole of each of acetic acid and ethanol is heated in the presence of a little concentrated $H_2SO_4$. When equilibrium is reached,which of the following is true?

Given three reactions and their equilibrium constants:
$N_2 + 3H_2 \rightleftharpoons 2NH_3 ; k_1$
$N_2 + O_2 \rightleftharpoons 2NO ; k_2$
$H_2 + \frac{1}{2}O_2 \rightleftharpoons H_2O ; k_3$
The equilibrium constant for the reaction $2NH_3 + \frac{5}{2}O_2 \rightleftharpoons 2NO + 3H_2O$ in terms of $k_1, k_2,$ and $k_3$ is:

For the reaction $A + B \rightleftharpoons 2C$,the value of equilibrium constant is $100$ at $298 \ K$. If the initial concentration of all the three species is $1 \ M$ each,then the equilibrium concentration of $C$ is $X \times 10^{-1} \ M$. The value of $X$ is $.....$ (Nearest integer)

For the reaction $X_{2(g)} + Y_{2(g)} \rightleftharpoons 2XY_{(g)}$,the reaction is studied at a fixed temperature. Initially,$1 \ mol$ of $X_2$ is taken in a $1 \ L$ flask and $2 \ mol$ of $Y_2$ is taken in a $2 \ L$ flask. If the flasks are connected,what are the equilibrium concentrations of $X_2$ and $Y_2$? (Given: Equilibrium concentration of $XY = 0.6 \ mol/L$)

Two solids dissociate as follows:
$A_{(s)} \rightleftharpoons B_{(g)} + C_{(g)}$; $K_{p_1} = x \, atm^2$
$D_{(s)} \rightleftharpoons C_{(g)} + E_{(g)}$; $K_{p_2} = y \, atm^2$
The total pressure when both the solids dissociate simultaneously is:

The reaction $2 NO_{2(g)} \rightleftharpoons N_2O_{4(g)}$ is at equilibrium in a closed $15 \ L$ vessel at $300 \ K$. The total weight of the mixture of $NO_2$ and $N_2O_4$ in the vessel is $64.4 \ g$. The equilibrium constant for the reaction is $K_p = 6.67$. Assuming ideal gas behavior,the total pressure in the vessel (in $atm$) is: [Given: Gas constant $R = 0.082 \ atm \ L \ K^{-1} \ mol^{-1}$]