(C) $A. K_p > Q$: Since the reaction quotient $Q$ is less than the equilibrium constant $K_p$,the reaction proceeds in the forward direction,making it

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$A-(iv), B-(i), C-(ii), D-(iii)$

(C) $A. K_p > Q$: Since the reaction quotient $Q$ is less than the equilibrium constant $K_p$,the reaction proceeds in the forward direction,making it spontaneous. $(A-(iv))$$B. \Delta G^\circ 0$,indicating a non-spontaneous process. $(B-(i))$$C. K_p = Q$: The system is at equilibrium. $(C-(ii))$$D. T > \frac{\Delta H}{\Delta S}$: For an endothermic process $(\Delta H > 0)$,if $T > \frac{\Delta H}{\Delta S}$,then $T \Delta S > \Delta H$,resulting in $\Delta G = \Delta H - T \Delta S < 0$,which means the process is spontaneous and endothermic. $(D-(iii))$

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

Medium

Match List-$I$ (Equations) with List-$II$ (Type of processes) and select the correct option.
List-$I$ (Equations) List-$II$ (Type of processes)
$A. K_p > Q$ $(i)$ Non-spontaneous
$B. \Delta G^\circ < RT \ln Q$ $(ii)$ Equilibrium
$C. K_p = Q$ $(iii)$ Spontaneous and endothermic
$D. T > \frac{\Delta H}{\Delta S}$ $(iv)$ Spontaneous

AIPMT 2010 All AIPMT

A
$A-(i), B-(ii), C-(iii), D-(iv)$
B
$A-(iii), B-(iv), C-(ii), D-(i)$
C
$A-(iv), B-(i), C-(ii), D-(iii)$
D
$A-(ii), B-(i), C-(iv), D-(iii)$

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6-1.Equilibrium (Chemical Equilibrium)

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

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AIPMT 2010 Paper All AIPMT years →

Calculate the partial pressure of carbon monoxide from the following data:
$CaCO_{3(s)} \rightleftharpoons CaO_{(s)} + CO_{2(g)}, K_p = 8 \times 10^{-2}$
$CO_{2(g)} + C_{(s)} \rightleftharpoons 2CO_{(g)}, K_p = 2$

Difficult

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For the reaction $A + 2B \rightleftharpoons 2C + D$,the initial concentration of $A$ is $a$ and the initial concentration of $B$ is $1.5$ times that of $A$. If the concentrations of $A$ and $D$ are equal at equilibrium,what will be the concentration of $B$ at equilibrium?

Medium

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Match the items in List-$X$ with List-$Y$ and select the correct option.

List-$X$ List-$Y$

$(A)$ Active mass $(i)$ $\Delta n = 0$

$(B)$ Equilibrium constant $(ii)$ Molar concentration

$(C)$ $A + \text{Heat} \rightleftharpoons B$ $(iii)$ Van't Hoff equation

$(D)$ $2A_{(g)} + B_{(g)} \rightleftharpoons 3C_{(g)}$ $(iv)$ Favoured by increase in temperature

$(v)$ Chemical equilibrium

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 $M$)?

Difficult

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$3.00 \ mol$ of $PCl_5$ kept in $1 \ L$ closed reaction vessel was allowed to attain equilibrium at $380 \ K$. If $1.59 \ mol$ of reactant was converted into the product at equilibrium,then $K_c$ is:

Medium

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List-$I$ (Equations)	List-$II$ (Type of processes)
$A. K_p > Q$	$(i)$ Non-spontaneous
$B. \Delta G^\circ < RT \ln Q$	$(ii)$ Equilibrium
$C. K_p = Q$	$(iii)$ Spontaneous and endothermic
$D. T > \frac{\Delta H}{\Delta S}$	$(iv)$ Spontaneous

List-$X$	List-$Y$
$(A)$ Active mass	$(i)$ $\Delta n = 0$
$(B)$ Equilibrium constant	$(ii)$ Molar concentration
$(C)$ $A + \text{Heat} \rightleftharpoons B$	$(iii)$ Van't Hoff equation
$(D)$ $2A_{(g)} + B_{(g)} \rightleftharpoons 3C_{(g)}$	$(iv)$ Favoured by increase in temperature
	$(v)$ Chemical equilibrium

Similar Questions

Calculate the partial pressure of carbon monoxide from the following data:$CaCO_{3(s)} \rightleftharpoons CaO_{(s)} + CO_{2(g)}, K_p = 8 \times 10^{-2}$$CO_{2(g)} + C_{(s)} \rightleftharpoons 2CO_{(g)}, K_p = 2$

For the reaction $A + 2B \rightleftharpoons 2C + D$,the initial concentration of $A$ is $a$ and the initial concentration of $B$ is $1.5$ times that of $A$. If the concentrations of $A$ and $D$ are equal at equilibrium,what will be the concentration of $B$ at equilibrium?

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 $M$)?

$3.00 \ mol$ of $PCl_5$ kept in $1 \ L$ closed reaction vessel was allowed to attain equilibrium at $380 \ K$. If $1.59 \ mol$ of reactant was converted into the product at equilibrium,then $K_c$ is:

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Calculate the partial pressure of carbon monoxide from the following data:
$CaCO_{3(s)} \rightleftharpoons CaO_{(s)} + CO_{2(g)}, K_p = 8 \times 10^{-2}$
$CO_{2(g)} + C_{(s)} \rightleftharpoons 2CO_{(g)}, K_p = 2$

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 $M$)?