For the reaction,$C_{(s)} + CO_{2(g)} \rightleftharpoons 2CO_{(g)}$,the partial pressures of $CO_2$ and $CO$ are $2.0 \ atm$ and $4.0 \ atm$,respectively,at equilibrium. The $K_p$ of the reaction is

Consider the partial decomposition of $A$ as:
$2A_{(g)} \rightleftharpoons 2B_{(g)} + C_{(g)}$
At equilibrium,a $700 \ mL$ gaseous mixture contains $100 \ mL$ of gas $C$ at $10 \ atm$ and $300 \ K$. What is the value of $K_P$ for the reaction?

$2 \ mol$ of $N_2$ is mixed with $6 \ mol$ of $H_2$ in a closed vessel of $1 \ L$ capacity. If $50\%$ of $N_2$ is converted into $NH_3$ at equilibrium,the value of $K_c$ for the reaction $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$ is

Equilibrium constants $K_1$ and $K_2$ for the following equilibria are given:
$NO_{(g)} + 1/2 O_{2(g)} \rightleftharpoons NO_{2(g)}$
$2NO_{2(g)} \rightleftharpoons 2NO_{(g)} + O_{2(g)}$
What is the relationship between $K_1$ and $K_2$?

If the equilibrium constants of the following equilibria $SO_2 + \frac{1}{2} O_2 \rightleftharpoons SO_3$ and $2 SO_3 \rightleftharpoons 2 SO_2 + O_2$ are given by $K_1$ and $K_2$ respectively, which of the following relations is correct?

$A$ vessel at $1000 \ K$ contains $CO_2$ with a pressure of $0.5 \ atm$. Some of the $CO_2$ is converted into $CO$ on the addition of graphite. If the total pressure at equilibrium is $0.8 \ atm$,the value of $K_p$ is $..... \ atm$.