(C) The reaction is $A + 2B \rightleftharpoons 2C + D$.Initial moles: $A = 1.1, B = 2.2, C = 0, D = 0$.At equilibrium,$0.2 \ mol$ of $C$ is formed. Si

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(C) The reaction is $A + 2B \rightleftharpoons 2C + D$.Initial moles: $A = 1.1, B = 2.2, C = 0, D = 0$.At equilibrium,$0.2 \ mol$ of $C$ is formed. Since the stoichiometric coefficient of $C$ is $2$,the change in moles is:$A: 1.1 - 0.1 = 1.0 \ mol$$B: 2.2 - 0.2 = 2.0 \ mol$$C: 0 + 0.2 = 0.2 \ mol$$D: 0 + 0.1 = 0.1 \ mol$Since the volume is $1 \ L$,the concentrations are equal to the number of moles.$K_C = \frac{[C]^2 [D]}{[A] [B]^2} = \frac{(0.2)^2 \times (0.1)}{(1.0) \times (2.0)^2} = \frac{0.04 \times 0.1}{1.0 \times 4.0} = \frac{0.004}{4.0} = 0.001$.

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

Medium

$1.1 \ mol$ of $A$ and $2.2 \ mol$ of $B$ are mixed in a $1 \ L$ flask until equilibrium is reached. At equilibrium,$0.2 \ mol$ of $C$ is formed. If the equilibrium reaction is $A + 2B \rightleftharpoons 2C + D$,the value of the equilibrium constant $K_C$ is:

A
$0.002$
B
$0.004$
C
$0.001$
D
$0.003$

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6-1.Equilibrium (Chemical Equilibrium)

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Kp and Kc Relationship

What 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 $0.185 \ bar$.)

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For the reaction $Mg(HCO_3)_{2(s)} \rightleftharpoons MgCO_{3(s)} + CO_{2(g)} + H_2O_{(g)}$,the equilibrium constant $K_p = 64 \ atm^2$. Calculate the total pressure at equilibrium.

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The equilibrium constant of $NH_4COONH_2$ in a closed vessel at $400 \ K$ temperature is $600 \ bar^3$. What will be the total pressure at equilibrium (in $bar$)?
$NH_4COONH_{2(s)} \rightleftharpoons 2NH_{3(g)} + CO_{2(g)}$

Medium

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For the equilibrium $SO_2Cl_{2(g)} \rightleftharpoons SO_{2(g)} + Cl_{2(g)}$,what is the temperature at which $\frac{K_p}{K_c} = \frac{1}{3}$? (Given $R = 0.0821 \ L \ atm \ K^{-1} \ mol^{-1}$)

Medium

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At $700 \, K$,the equilibrium constant $K_p$ for the reaction $2SO_{3(g)} \rightleftharpoons 2SO_{2(g)} + O_{2(g)}$ is $1.80 \times 10^{-3}$. The numerical value in $mol \, L^{-1}$ of $K_c$ for this reaction at the same temperature will be $(R = 8.314 \, J \, K^{-1} \, mol^{-1})$.

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$1.1 \ mol$ of $A$ and $2.2 \ mol$ of $B$ are mixed in a $1 \ L$ flask until equilibrium is reached. At equilibrium,$0.2 \ mol$ of $C$ is formed. If the equilibrium reaction is $A + 2B \rightleftharpoons 2C + D$,the value of the equilibrium constant $K_C$ is:

Similar Questions

What 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 $0.185 \ bar$.)

For the reaction $Mg(HCO_3)_{2(s)} \rightleftharpoons MgCO_{3(s)} + CO_{2(g)} + H_2O_{(g)}$,the equilibrium constant $K_p = 64 \ atm^2$. Calculate the total pressure at equilibrium.

The equilibrium constant of $NH_4COONH_2$ in a closed vessel at $400 \ K$ temperature is $600 \ bar^3$. What will be the total pressure at equilibrium (in $bar$)?$NH_4COONH_{2(s)} \rightleftharpoons 2NH_{3(g)} + CO_{2(g)}$

For the equilibrium $SO_2Cl_{2(g)} \rightleftharpoons SO_{2(g)} + Cl_{2(g)}$,what is the temperature at which $\frac{K_p}{K_c} = \frac{1}{3}$? (Given $R = 0.0821 \ L \ atm \ K^{-1} \ mol^{-1}$)

At $700 \, K$,the equilibrium constant $K_p$ for the reaction $2SO_{3(g)} \rightleftharpoons 2SO_{2(g)} + O_{2(g)}$ is $1.80 \times 10^{-3}$. The numerical value in $mol \, L^{-1}$ of $K_c$ for this reaction at the same temperature will be $(R = 8.314 \, J \, K^{-1} \, mol^{-1})$.

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The equilibrium constant of $NH_4COONH_2$ in a closed vessel at $400 \ K$ temperature is $600 \ bar^3$. What will be the total pressure at equilibrium (in $bar$)?
$NH_4COONH_{2(s)} \rightleftharpoons 2NH_{3(g)} + CO_{2(g)}$