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 $(\ln \ 20 = 2.99)$.

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 $R = 0.082 \ atm \ L \ K^{-1} \ mol^{-1}$]

Consider the reaction $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$. The equilibrium constant of the above reaction is $K_p$. If pure ammonia is left to dissociate,the partial pressure of ammonia at equilibrium is given by (Assume that $P_{NH_3} \ll P_{total}$ at equilibrium and $P$ is the total pressure).

Nitric oxide reacts with $Br_{2}$ and gives nitrosyl bromide as per the reaction given below:
$2 NO_{(g)} + Br_{2(g)} \longleftrightarrow 2 NOBr_{(g)}$
When $0.087 \ mol$ of $NO$ and $0.0437 \ mol$ of $Br_{2}$ are mixed in a closed container at constant temperature,$0.0518 \ mol$ of $NOBr$ is obtained at equilibrium. Calculate the equilibrium amount of $NO$ and $Br_{2}$.

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?

Calculate the partial pressure of carbon monoxide from the following data:
$CaCO_{3(s)} \rightleftharpoons CaO_{(s)} + CO_{2(g)}, K_p = 8 \times 10^{-2}$
$CO_{2(g)} + C_{(s)} \rightleftharpoons 2CO_{(g)}, K_p = 2$