(D) The equilibrium reaction is: $CaCO_{3(s)} \rightleftharpoons CaO_{(s)} + CO_{2(g)}$.Initial moles of $CaCO_{3} = \frac{50 \ g}{100 \ g/mol} = 0.5

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(D) The equilibrium reaction is: $CaCO_{3(s)} \rightleftharpoons CaO_{(s)} + CO_{2(g)}$.Initial moles of $CaCO_{3} = \frac{50 \ g}{100 \ g/mol} = 0.5 \ mol$.For this reaction,$K_{p} = P_{CO_{2}} = 1.64 \ atm$.Using the ideal gas equation $PV = nRT$ for $CO_{2}$ gas:$1.64 \ atm \times 10 \ L = n_{CO_{2}} \times 0.082 \ L \ atm \ K^{-1} \ mol^{-1} \times 1000 \ K$.$16.4 = n_{CO_{2}} \times 82$.$n_{CO_{2}} = \frac{16.4}{82} = 0.2 \ mol$.Since $1 \ mol$ of $CaCO_{3}$ produces $1 \ mol$ of $CO_{2}$,the moles of $CaCO_{3}$ reacted $= 0.2 \ mol$.Moles of $CaCO_{3}$ remaining $= 0.5 - 0.2 = 0.3 \ mol$.Percentage of unreacted $CaCO_{3} = \frac{0.3}{0.5} \times 100 = 60 \%$.

Class 11 Chemistry 6-1.Equilibrium (Chemical Equilibrium)Mix Examples- 6-1.Equilibrium (Chemical Equilibrium)

Medium

For the equilibrium:
$CaCO_{3(s)} \rightleftharpoons CaO_{(s)} + CO_{2(g)}$; $K_{p} = 1.64 \ atm$ at $1000 \ K$.
$50 \ g$ of $CaCO_{3}$ in a $10 \ L$ closed vessel is heated to $1000 \ K$. The percentage of $CaCO_{3}$ that remains unreacted at equilibrium is:
(Given $R = 0.082 \ L \ atm \ K^{-1} \ mol^{-1}$)

KCET 2014 All KCET

A
$50$
B
$20$
C
$40$
D
$60$

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6-1.Equilibrium (Chemical Equilibrium)

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Mix Examples- 6-1.Equilibrium (Chemical Equilibrium)

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For the reaction,$N_2O_{4(g)} \rightleftharpoons 2NO_{2(g)}$,if dinitrogen tetroxide is $50\%$ dissociated at $60^\circ C$,the standard free energy change at this temperature and $1 \ atm$ pressure is:

MediumAP EAMCET 2020

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The equilibrium constants $(K_C)$ of two reactions $H_2 + I_2 \rightleftharpoons 2 HI$ and $N_2 + 3 H_2 \rightleftharpoons 2 NH_3$ are $50$ and $1000$,respectively. The equilibrium constant of the reaction $N_2 + 6 HI \rightleftharpoons 2 NH_3 + 3 I_2$ is closest to

MediumKVPY 2014

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Given three reactions and their equilibrium constants:
$N_2 + 3H_2 \rightleftharpoons 2NH_3 ; k_1$
$N_2 + O_2 \rightleftharpoons 2NO ; k_2$
$H_2 + \frac{1}{2}O_2 \rightleftharpoons H_2O ; k_3$
The equilibrium constant for the reaction $2NH_3 + \frac{5}{2}O_2 \rightleftharpoons 2NO + 3H_2O$ in terms of $k_1, k_2,$ and $k_3$ is:

Medium

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At a certain temperature,the equilibrium constant $K_c$ is $0.25$ for the reaction:
$A_{2(g)} + B_{2(g)} \rightleftharpoons C_{2(g)} + D_{2(g)}$
If we take $1 \ mol$ of each of the four gases in a $10 \ L$ container,what would be the equilibrium concentration of $A_{2(g)}$ (in $M$)?

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If the pressure in a reaction vessel for the following reaction is increased by decreasing the volume,what will happen to the concentrations of $CO$ and $CO_2$ ?
$H_2O_{(g)} + CO_{(g)} \rightleftharpoons H_{2(g)} + CO_{2(g)} + \text{Heat}$

Medium

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For the reaction,$N_2O_{4(g)} \rightleftharpoons 2NO_{2(g)}$,if dinitrogen tetroxide is $50\%$ dissociated at $60^\circ C$,the standard free energy change at this temperature and $1 \ atm$ pressure is:

The equilibrium constants $(K_C)$ of two reactions $H_2 + I_2 \rightleftharpoons 2 HI$ and $N_2 + 3 H_2 \rightleftharpoons 2 NH_3$ are $50$ and $1000$,respectively. The equilibrium constant of the reaction $N_2 + 6 HI \rightleftharpoons 2 NH_3 + 3 I_2$ is closest to

At a certain temperature,the equilibrium constant $K_c$ is $0.25$ for the reaction:$A_{2(g)} + B_{2(g)} \rightleftharpoons C_{2(g)} + D_{2(g)}$If we take $1 \ mol$ of each of the four gases in a $10 \ L$ container,what would be the equilibrium concentration of $A_{2(g)}$ (in $M$)?

If the pressure in a reaction vessel for the following reaction is increased by decreasing the volume,what will happen to the concentrations of $CO$ and $CO_2$ ?$H_2O_{(g)} + CO_{(g)} \rightleftharpoons H_{2(g)} + CO_{2(g)} + \text{Heat}$

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At a certain temperature,the equilibrium constant $K_c$ is $0.25$ for the reaction:
$A_{2(g)} + B_{2(g)} \rightleftharpoons C_{2(g)} + D_{2(g)}$
If we take $1 \ mol$ of each of the four gases in a $10 \ L$ container,what would be the equilibrium concentration of $A_{2(g)}$ (in $M$)?

If the pressure in a reaction vessel for the following reaction is increased by decreasing the volume,what will happen to the concentrations of $CO$ and $CO_2$ ?
$H_2O_{(g)} + CO_{(g)} \rightleftharpoons H_{2(g)} + CO_{2(g)} + \text{Heat}$