(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 →

For the reaction $2A_{(g)} + B_{(g)} \rightleftharpoons 3C_{(g)} + D_{(g)}$,two moles each of $A$ and $B$ were taken into a $1 \ L$ flask. Which of the following must always be true when the system attains equilibrium?

Medium

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For the reactions $X \rightleftharpoons 2Y$ and $Z \rightleftharpoons P + Q$,the equilibrium constants $K_p$ and $K_q$ are in the ratio $1:9$. If the degree of dissociation of $X$ and $Z$ is the same,then the ratio of their total pressures is:

Difficult

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For the ideal gas reaction,$X + Y \rightleftharpoons Z$,a mixture with $n_{X} = 1 \, mol$,$n_{Y} = 3 \, mol$ and $n_{Z} = 2 \, mol$ is at equilibrium at $300 \, K$ and $1 \, bar$. If the pressure is isothermally increased to $2 \, bar$,the number of moles of $X$ in the new equilibrium is closest to $......$

DifficultKVPY 2021

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$A$ $20 \, L$ container at $400 \, K$ contains $CO_{2(g)}$ at a pressure of $0.4 \, atm$ and an excess of $SrO$ (neglect the volume of solid $SrO$). The volume of the container is now decreased by moving the movable piston fitted in the container. The maximum volume of the container,when the pressure of $CO_2$ attains its maximum value,will be........$L$
(Given: $SrCO_{3(s)} \rightleftharpoons SrO_{(s)} + CO_{2(g)}, K_p = 1.6 \, atm$)

MediumNEET 2017

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The equilibrium constant at $298 \ K$ for a reaction $A + B \rightleftharpoons C + D$ is $100$. If the initial concentration of all the four species were $1 \ M$ each,then the equilibrium concentration of $D$ (in $mol \ L^{-1}$) will be:

DifficultKCET 2025

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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

Similar Questions

For the reaction $2A_{(g)} + B_{(g)} \rightleftharpoons 3C_{(g)} + D_{(g)}$,two moles each of $A$ and $B$ were taken into a $1 \ L$ flask. Which of the following must always be true when the system attains equilibrium?

For the reactions $X \rightleftharpoons 2Y$ and $Z \rightleftharpoons P + Q$,the equilibrium constants $K_p$ and $K_q$ are in the ratio $1:9$. If the degree of dissociation of $X$ and $Z$ is the same,then the ratio of their total pressures is:

The equilibrium constant at $298 \ K$ for a reaction $A + B \rightleftharpoons C + D$ is $100$. If the initial concentration of all the four species were $1 \ M$ each,then the equilibrium concentration of $D$ (in $mol \ L^{-1}$) will be:

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