(B) The chemical equation is $NH_4HS_{(s)} \rightleftharpoons NH_{3_{(g)}} + H_2S_{(g)}$.Let the partial pressure of $NH_3$ be $P$ and the partial pre

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(B) The chemical equation is $NH_4HS_{(s)} \rightleftharpoons NH_{3_{(g)}} + H_2S_{(g)}$.Let the partial pressure of $NH_3$ be $P$ and the partial pressure of $H_2S$ be $P$ at equilibrium.The total pressure at equilibrium is $P_{total} = P_{NH_3} + P_{H_2S} = P + P = 2P$.Given that $P_{total} = 1.12 \ atm$,we have $2P = 1.12 \ atm$,which gives $P = 0.56 \ atm$.The equilibrium constant $K_p$ is given by $K_p = P_{NH_3} \times P_{H_2S} = P \times P = P^2$.Substituting the value of $P$,$K_p = (0.56)^2 = 0.3136 \ atm^2$.

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

Medium

For $NH_4HS_{(s)} \rightleftharpoons NH_{3_{(g)}} + H_2S_{(g)}$; the observed pressure for the reaction mixture at equilibrium is $1.12 \ atm$ at $106 \ ^oC$. The value of $K_p$ for the reaction is: (in $atm^2$)

A
$3.316$
B
$0.3136$
C
$31.36$
D
$6.68$

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6-1.Equilibrium (Chemical Equilibrium)

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Kp and Kc Relationship

For the reaction $N_2 + 3H_2 \rightleftharpoons 2NH_3$,the equilibrium constant is $K$. What will be the equilibrium constant for the reaction $NH_3 \rightleftharpoons \frac{1}{2}N_2 + \frac{3}{2}H_2$?

Medium

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For a reaction $2A_{(g)} \rightleftharpoons 2B_{(g)} + C_{(g)}$,$K_c = 3.75 \times 10^{-6}$ at $1069 \ K$. The approximate value of $K_p$ for this reaction at the same temperature is $(R = 0.082 \ L \ bar \ mol^{-1} \ K^{-1})$.

MediumTS EAMCET 2018

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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?

Medium

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For the reaction $SO_{2(g)} + \frac{1}{2} O_{2(g)} \rightleftharpoons SO_{3(g)},$ if $K_P = K_C (RT)^x$ where the symbols have usual meaning,then the value of $x$ is (assuming ideality):

MediumJEE MAIN 2014

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For the reaction $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$ at $300 \, ^\circ C$,the value of $K_c$ is $0.65$. If $R = 0.082 \, L \cdot atm \cdot K^{-1} \cdot mol^{-1}$,then the value of $K_p$ will be:

Medium

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For $NH_4HS_{(s)} \rightleftharpoons NH_{3_{(g)}} + H_2S_{(g)}$; the observed pressure for the reaction mixture at equilibrium is $1.12 \ atm$ at $106 \ ^oC$. The value of $K_p$ for the reaction is: (in $atm^2$)

Similar Questions

For the reaction $N_2 + 3H_2 \rightleftharpoons 2NH_3$,the equilibrium constant is $K$. What will be the equilibrium constant for the reaction $NH_3 \rightleftharpoons \frac{1}{2}N_2 + \frac{3}{2}H_2$?

For a reaction $2A_{(g)} \rightleftharpoons 2B_{(g)} + C_{(g)}$,$K_c = 3.75 \times 10^{-6}$ at $1069 \ K$. The approximate value of $K_p$ for this reaction at the same temperature is $(R = 0.082 \ L \ bar \ mol^{-1} \ K^{-1})$.

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?

For the reaction $SO_{2(g)} + \frac{1}{2} O_{2(g)} \rightleftharpoons SO_{3(g)},$ if $K_P = K_C (RT)^x$ where the symbols have usual meaning,then the value of $x$ is (assuming ideality):

For the reaction $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$ at $300 \, ^\circ C$,the value of $K_c$ is $0.65$. If $R = 0.082 \, L \cdot atm \cdot K^{-1} \cdot mol^{-1}$,then the value of $K_p$ will be:

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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?