List of top Chemistry Questions on Law Of Chemical Equilibrium And Equilibrium Constant asked in JEE Advanced

When potassium iodide is added to an aqueous solution of potassium ferricyanide, a reversible reaction is observed in which a complex P is formed. In a strong acidic medium, the equilibrium shifts completely towards P. Addition of zinc chloride to P in a slightly acidic medium results in a sparingly soluble complex Q.

In a one-litre flask, 6 moles of A undergoes the reaction A (g) ⇌ P (g). The progress of product formation at two temperatures (in Kelvin), T₁ and T₂, is shown in the figure: 

If T₁ = 2T₂ and (∆G₂^Θ − ∆G₁^Θ) = RT₂ ln x, then the value of x is ___ .
[∆G₁^Θ and ∆G₂^Θ are standard Gibb’s free energy change for the reaction at temperatures T₁ and T₂, respectively.]

In a one-litre flask, 6 moles of A undergoes the reaction A (g) ⇌ P (g). The progress of product formation at two temperatures (in Kelvin), T₁ and T₂, is shown in the figure: 

If T₁ = 2T₂ and (∆G₂^Θ − ∆G₁^Θ) = RT₂ ln x, then the value of x is ___ . [∆G₁^Θ and ∆G₂^Θ are standard Gibb’s free energy change for the reaction at temperatures T₁ and T₂, respectively.]

For the reaction, $X (s) \rightleftharpoons Y (s)+ Z (g)$, the plot of $\ln \frac{p_{ Z }}{p^{0}}$ versus $\frac{10^{4}}{T}$ is given below (in solid line), where $p_{ z }$ is the pressure (in bar) of the gas $Z$ at temperature $T$ and $p^0=1$ bar 

(Given, $\frac{ d (\ln K)}{ d \left(\frac{1}{T}\right)}=-\frac{\Delta H^{0}}{R}$, where the equilibrium constant, $K=\frac{p_{z}}{p^{0}}$ and the gas constant, $R=8.314 \,J \,K ^{-1} mol ^{-1}$ ) 
The value of $\Delta S^{0}$ (in $J\, K ^{-1} mol ^{-1}$ ) for the given reaction, at $1000\, K$ is ______

For the reaction, $X (s) \rightleftharpoons Y (s)+ Z (g)$, the plot of $\ln \frac{p_{ Z }}{p^{0}}$ versus $\frac{10^{4}}{T}$ is given below (in solid line), where $p_{ z }$ is the pressure (in bar) of the gas $Z$ at temperature $T$ and $p^0=1$ bar

 (Given, $\frac{ d (\ln K)}{ d \left(\frac{1}{T}\right)}=-\frac{\Delta H^{0}}{R}$, where the equilibrium constant, $K=\frac{p_{z}}{p^{0}}$ and the gas constant, $R=8314 \,J \,K ^{-1} mol ^{-1}$ ) 
The value of standard enthalpy, $\Delta H^{0}$ (in $kJ\, mol ^{-1}$ ) for the given reaction is ______

For the reaction, $X (s) \rightleftharpoons Y (s)+ Z (g)$, the plot of $\ln \frac{p_{ Z }}{p^{0}}$ versus $\frac{10^{4}}{T}$ is given below (in solid line), where $p_{ z }$ is the pressure (in bar) of the gas $Z$ at temperature $T$ and $p^0=1$ bar

 (Given, $\frac{ d (\ln K)}{ d \left(\frac{1}{T}\right)}=-\frac{\Delta H^{0}}{R}$, where the equilibrium constant, $K=\frac{p_{z}}{p^{0}}$ and the gas constant, $R=8314 \,J \,K ^{-1} mol ^{-1}$ )

Consider the reaction $A \rightleftharpoons B$ at $1000\, K$ At time '$t$', the temperature of the system was increased to $2000 \,K$ and the system was allowed to reach equilibrium. Throughout this experiment the partial pressure of $A$ was maintained at $1$ bar. Given below is the plot of the partial pressure of $B$ with time. What is the ratio of the standard Gibbs energy of the reaction at $1000\, K$ to that at $2000\, K$ ?

An acidified solution of $0.05 \,M\, Zn ^{2+}$ is saturated with $0.1 \,M \,H _{2} S$. What is the minimum molar concentration $(M)$ of $H ^{+}$required to prevent the precipitation of $ZnS$ ?
Use $K_{s p}( ZnS )=1.25 \times 10^{-22}$ and overall dissociation constant of $H _{2} S. K _{ NET }=K_{1} K_{2}=1 \times 10^{-21}$

The precipitate of C$aF_2, \, ( K_{sp} = 1.7 \times 10^{ - 10 } )$ is obtained, when equal volumes of which of the following are mixed?