(A) The equilibrium reaction is: $2 SO_{2(g)} + O_{2(g)} \rightleftharpoons 2 SO_{3(g)}$$K_{P} = \frac{(P_{SO_3})^2}{(P_{SO_2})^2 (P_{O_2})}$Given tha

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(A) The equilibrium reaction is: $2 SO_{2(g)} + O_{2(g)} \rightleftharpoons 2 SO_{3(g)}$$K_{P} = \frac{(P_{SO_3})^2}{(P_{SO_2})^2 (P_{O_2})}$Given that at equilibrium,$P_{SO_2} = P_{SO_3}$.Substituting this into the expression: $5 = \frac{(P_{SO_2})^2}{(P_{SO_2})^2 (P_{O_2})}$$5 = \frac{1}{P_{O_2}}$$P_{O_2} = \frac{1}{5} = 0.2 \ atm$.

Class 11 Chemistry 6-1.Equilibrium (Chemical Equilibrium)Kp and Kc Relationship

Medium

The $K_{p}$ value at equilibrium of $SO_3$ formation reaction from $SO_{2(g)}$ and $O_{2(g)}$ is $5 \ atm^{-1}$. What is the equilibrium partial pressure of $O_2$ if the equilibrium pressure of $SO_2$ and $SO_3$ are equal (in $atm$)?

TS EAMCET 2022 All TS EAMCET

A
$0.2$
B
$0.4$
C
$0.3$
D
$0.1$

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6-1.Equilibrium (Chemical Equilibrium)

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Kp and Kc Relationship

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The $K_{p}$ value at equilibrium of $SO_3$ formation reaction from $SO_{2(g)}$ and $O_{2(g)}$ is $5 \ atm^{-1}$. What is the equilibrium partial pressure of $O_2$ if the equilibrium pressure of $SO_2$ and $SO_3$ are equal (in $atm$)?

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At a definite temperature and $3 \ atm$ pressure,$75\%$ of $PCl_5$ decomposes into $PCl_3$ and $Cl_2$. Find $K_p$ for the reaction: $PCl_{5(g)} \rightleftharpoons PCl_{3(g)} + Cl_{2(g)}$ (in $atm$)

In which of the following reactions is the value of $K_p$ equal to $K_c$?

In 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

For the reaction $2NOBr_{(g)} \rightleftharpoons 2NO_{(g)} + Br_{2(g)}$,if $P_{Br_2} = \frac{P}{9}$ at equilibrium and $P$ is the total pressure,find the value of $\frac{K_P}{P}$.

For the reaction: $Fe_{2}N_{(s)} + \frac{3}{2}H_{2(g)} \rightleftharpoons 2Fe_{(s)} + NH_{3(g)}$,which of the following relations is correct?

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