For the reaction $H_{2(g)} + CO_{2(g)} \rightleftharpoons CO_{(g)} + H_2O_{(g)}$. If the initial concentration of $[H_2] = [CO_2] = 1 \ M$ and $x \ mol/L$ of hydrogen is consumed at equilibrium,then the correct expression of $K_p$ is
- A$\frac{x^2}{(1 - x)^2}$
- B$\frac{(1 + x)^2}{(1 - x)^2}$
- C$\frac{x^2}{(2 + x)^2}$
- D$\frac{x^2}{1 - x^2}$
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Similar Questions
At $T(K)$,$K_{c}$ value for $AO_{2(g)} + BO_{2(g)} \rightleftharpoons AO_{3(g)} + BO_{(g)}$ is $16$. In a closed $1 \ L$ flask,one mole each of $AO_2, BO_2, AO_3$ and $BO$ are taken and heated to $T(K)$. What is the concentration (in $mol \ L^{-1}$) of $AO_3$ at equilibrium?
The equilibrium constant $(K_P)$ for the reaction $2SO_2 + O_2 \rightleftharpoons 2SO_3$ at $1000 \ K$ is $3.5$. The partial pressure of oxygen gas to give equal mole of $SO_2$ and $SO_3$ is $... \ atm$.
Medium
View SolutionIn which of the following reactions is the value of $K_p$ equal to $K_c$?
Medium
View SolutionWhat is the value of the equilibrium constant $K_p$ for the reaction ${H_2O_{(l)}} \rightleftharpoons {H_2O_{(g)}}$ at $60^{\circ}C$? (The vapor pressure of water at $60^{\circ}C$ is $0.185 \ bar$.)
Medium
View SolutionThe values of pressure equilibrium constant recorded at different temperatures for the following equilibrium reaction have been given below: $A(g) \rightleftharpoons B(g) + C(g)$.
$1/T \text{ (K}^{-1})$ $\log_{10} K_p$ $0.05$ $3.5$ $0.06$ $2.5$ $0.07$ $1.5$
The magnitude of $\frac{\Delta H^\circ}{R}$ calculated from the above data is . . . . . . . (Note: The slope $m = -\frac{\Delta H^\circ}{2.303 R}$)
| $1/T \text{ (K}^{-1})$ | $\log_{10} K_p$ |
| $0.05$ | $3.5$ |
| $0.06$ | $2.5$ |
| $0.07$ | $1.5$ |
The magnitude of $\frac{\Delta H^\circ}{R}$ calculated from the above data is . . . . . . . (Note: The slope $m = -\frac{\Delta H^\circ}{2.303 R}$)
DifficultJEE MAIN 2026
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