(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 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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1 Equilibrium: Chemical Equilibrium

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

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In a closed vessel,the decomposition of solid $Mg(HCO_3)_2$ is given as follows:
$Mg(HCO_3)_{2(s)} \rightleftharpoons MgCO_{3(s)} + CO_{2(g)} + H_2O_{(g)}$
Given $K_p = 64 \ bar^2$ and the mole fraction of $CO_2$ is $0.8$,calculate the total pressure at equilibrium. (in $bar$)

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$CH_3COOH_{(l)} + C_2H_5OH_{(l)} \rightleftharpoons CH_3COOC_2H_{5_{(l)}} + H_2O_{(l)}$. In the above reaction,one mole of each of acetic acid and alcohol are heated in the presence of a little conc. $H_2SO_4$. On equilibrium being attained:

Difficult

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Three moles of $PCl_{5}$,three moles of $PCl_{3}$ and two moles of $Cl_{2}$ are taken in a closed vessel. If at equilibrium the vessel has $1.5$ moles of $PCl_{5}$,the number of moles of $PCl_{3}$ present in it is

MediumKCET 2008

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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

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The dissociation of $CO_2$ is represented as $2CO_2(g) \rightleftharpoons 2CO(g) + O_2(g)$. If $2 \ mol$ of $CO_2$ are taken initially and $40\%$ of $CO_2$ dissociates,what will be the total number of moles at equilibrium?

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

Similar Questions

In a closed vessel,the decomposition of solid $Mg(HCO_3)_2$ is given as follows:$Mg(HCO_3)_{2(s)} \rightleftharpoons MgCO_{3(s)} + CO_{2(g)} + H_2O_{(g)}$Given $K_p = 64 \ bar^2$ and the mole fraction of $CO_2$ is $0.8$,calculate the total pressure at equilibrium. (in $bar$)

$CH_3COOH_{(l)} + C_2H_5OH_{(l)} \rightleftharpoons CH_3COOC_2H_{5_{(l)}} + H_2O_{(l)}$. In the above reaction,one mole of each of acetic acid and alcohol are heated in the presence of a little conc. $H_2SO_4$. On equilibrium being attained:

Three moles of $PCl_{5}$,three moles of $PCl_{3}$ and two moles of $Cl_{2}$ are taken in a closed vessel. If at equilibrium the vessel has $1.5$ moles of $PCl_{5}$,the number of moles of $PCl_{3}$ present in it is

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?

The dissociation of $CO_2$ is represented as $2CO_2(g) \rightleftharpoons 2CO(g) + O_2(g)$. If $2 \ mol$ of $CO_2$ are taken initially and $40\%$ of $CO_2$ dissociates,what will be the total number of moles at equilibrium?

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In a closed vessel,the decomposition of solid $Mg(HCO_3)_2$ is given as follows:
$Mg(HCO_3)_{2(s)} \rightleftharpoons MgCO_{3(s)} + CO_{2(g)} + H_2O_{(g)}$
Given $K_p = 64 \ bar^2$ and the mole fraction of $CO_2$ is $0.8$,calculate the total pressure at equilibrium. (in $bar$)