For the reaction $H_{2(g)} + CO_{2(g)} \rightleftharpoons CO_{(g)} + H_2O_{(g)}$,if the reaction is started with $1 \ mol$ of $H_2$ and $CO_2$ each,and $x \ mol/L$ of $H_2$ is consumed at equilibrium,then the correct expression for $K_p$ will be ........
- A$x^2 / (1-x^2)$
- B$(1+x^2) / (1-x)^2$
- C$x^2 / (1-x)^2$
- D$x^2 / (2+x)^2$
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Similar Questions
For which of the following reactions will $K_p = K_c$?
Medium
View Solution$2 \ mol$ of $PCl_5$ is heated in a closed vessel of $2 \ L$ capacity. When equilibrium is attained,$PCl_5$ is $40\%$ dissociated. The equilibrium constant $K_c$ for the reaction will be ........... $mol/L$.
Difficult
View SolutionFor the decomposition of the compound,represented as $NH_2COONH_{4(s)} \rightleftharpoons 2NH_{3(g)} + CO_{2(g)}$,the $K_p = 2.9 \times 10^{-5} \ atm^3$. If the reaction is started with $1 \ mol$ of the compound,the total pressure at equilibrium would be............ $\times 10^{-2} \ atm$.
DifficultJEE MAIN 2014
View SolutionFind the value of $\frac{P}{K_p}$ for the reaction at a certain temperature: $2NOBr_{(g)} \rightleftharpoons 2NO_{(g)} + Br_{2(g)}$,where $P$ is the total pressure of gases at equilibrium and $P_{Br_2} = \frac{P}{9}$.
Medium
View SolutionIn a $500 \,mL$ flask,the degree of dissociation of $PCl_5$ at equilibrium is $40 \%$ and the initial amount is $5 \,moles$. The value of equilibrium constant in $mol \,L^{-1}$ for the decomposition of $PCl_5$ is
DifficultAP EAMCET 2008
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