Class 11Chemistry6-1.Equilibrium (Chemical Equilibrium)Mix Examples- 6-1.Equilibrium (Chemical Equilibrium)
MediumAt $783 \, K$ in the reaction,$H_{2(g)} + I_{2(g)} \rightleftharpoons 2 HI_{(g)}$,the molar concentrations $(mol \, L^{-1})$ of $H_2, I_2$ and $HI$ at some instant of time are $0.1, 0.2$ and $0.4$,respectively. If the equilibrium constant is $46$ at the same temperature,then as the reaction proceeds:
- Athe amount of $HI$ will increase
- Bthe amount of $HI$ will decrease
- Cthe amount of $H_2$ and $I_2$ will increase
- Dthe amount of $H_2$ and $I_2$ will not change
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Similar Questions
For the reaction $CH_{4(g)} + 2O_{2(g)} \rightleftharpoons CO_{2(g)} + 2H_{2}O_{(g)}$ with $\Delta H = -170.8 \ kJ \ mol^{-1}$,which of the following statements is incorrect?
Medium
View SolutionWhen $5 \ mol$ of $SO_2$ and $5 \ mol$ of $O_2$ are reacted,$60\%$ of $SO_2$ is consumed at equilibrium. If the total pressure of the equilibrium mixture is $1 \ atm$,then the partial pressure of $O_2$ will be ...... $atm$.
Medium
View Solution$A$ reaction mixture containing $H_2, N_2$ and $NH_3$ has partial pressures of $2 \ atm, 1 \ atm$ and $3 \ atm$ respectively at $725 \ K.$ If the value of $K_P$ for the reaction,$N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g)$ is $4.28 \times 10^{-5} \ atm^{-2}$ at $725 \ K,$ in which direction will the net reaction proceed?
Medium
View SolutionBromine monochloride,$BrCl$ decomposes into bromine and chlorine and reaches the equilibrium:
$2 BrCl_{(g)} \longleftrightarrow Br_{2(g)} + Cl_{2(g)}$
for which $K_c = 32$ at $500 \ K$.
If initially pure $BrCl$ is present at a concentration of $3.3 \times 10^{-3} \ mol \ L^{-1}$,what is its molar concentration in the mixture at equilibrium?
$2 BrCl_{(g)} \longleftrightarrow Br_{2(g)} + Cl_{2(g)}$
for which $K_c = 32$ at $500 \ K$.
If initially pure $BrCl$ is present at a concentration of $3.3 \times 10^{-3} \ mol \ L^{-1}$,what is its molar concentration in the mixture at equilibrium?
Medium
View SolutionFor a reaction $2 A \rightleftharpoons B + C$,$K_c$ is $2 \times 10^{-3}$. At a given time,the reaction mixture has $[A] = [B] = [C] = 3 \times 10^{-4} \ M$. Which of the following options is correct?
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