Chemical Equilibrium - Physical Chemistry PYQ

Using the data provided, find the value of equilibrium constant for the following reaction at \(298 \mathrm{~K}\) and \(1 \mathrm{~atm}\) pressure.

$$\begin{aligned} \[\mathrm{NO}(g)+\frac{1}{2} \mathrm{O}_2(g) \rightleftharpoons & \mathrm{NO}_2(g) \\\] \[\Delta_f H \mathrm{Y}[\mathrm{NO}(g)] & =90.4 \mathrm{~kJ} \mathrm{~mol}^{-1} \\\] \[\Delta_f H \mathrm{Y}\left[\mathrm{NO}_2(g)\right] & =32.48 \mathrm{~kJ} \mathrm{~mol}^{-1} \\\] \[\Delta S Y a t ~298 \mathrm{~K} & =-70.8 \mathrm{~JK}^{-1} \mathrm{~mol}^{-1}\] \end{aligned}$$

$$[\operatorname{antilog}(0.50)=3162 \text { ] }$$

Standard entropies of \(X_2, Y_2\) and \(X Y_3\) are 60, 40 and \(50 \mathrm{JK}^{-1} \mathrm{~mol}^{-1}\) respectively. At what temperature, the following reaction will be at equilibrium? [given: \(\Delta H \Upsilon=-30 \mathrm{~kJ}\)]

$$\frac{1}{2} X_2+\frac{3}{2} Y_2 \rightleftharpoons X Y_3$$

Which among the following denotes the correct relationship between \(K_p\) and \(K_c\) for the reaction, \(2 A(g) \rightleftharpoons B(g)+C(g)\)

For the reaction \(\mathrm{SO}_2(g)+\frac{1}{2} \mathrm{O}_2(g) \rightleftharpoons \mathrm{SO}_3(g)\), the percentage yield of product at different pressure is shown in the figure. Then, which among the following is true?

At \(60^{\circ} \mathrm{C}\), dinitrogen tetroxide is dissociated. Find it's standard free energy change at this temperature and one atmosphere. [Given \(\log 1.33=0.1239\)]

Le-Chatelier's principle is not applicable to

The formation of ammonia from its constituent elements is an exothermic reaction. The effect of increased temperature on the reaction equilibrium is

At 500 K , for the reaction \(\mathrm{N}_2(\mathrm{~g})+3 \mathrm{H}_2(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NH}_3(\mathrm{~g})\), the \(K_p\) is \(0.036 \mathrm{~atm}^{-2}\). What is its \(K_C\) in \(\mathrm{L}^2 \mathrm{~mol}^{-1}\) ? \(\left(R=0.082 \mathrm{~L}^2\right.\) atom \(\left.\mathrm{mol}^{-1} \mathrm{~K}^{-1}\right)\).

$K_{\mathrm{c}}$ for the following reaction is 99.0

$$A_2(g) \stackrel{T(K)}{\rightleftharpoons} B_2(g)$$

In a one litre flask, 2 moles of $A_2$ was heated to $T(\mathrm{~K})$ and the above equilibrium is reached. The concentration at equilibrium of $A_2$ and $B_2$ are $C_1\left(A_2\right)$ and $C_2\left(B_2\right)$ respectively. Now, one mole of $A_2$ was added to flask and heated to $T(\mathrm{~K})$ to established the equilibrium again. The concentration of $A_2$ and $B_2$ are $C_3\left(A_2\right)$ and $C_4\left(B_2\right)$ respectively. what is the value of $C_3\left(A_2\right)$ in $\mathrm{mol} \mathrm{L}^{-1}$ ?

At $T(\mathrm{~K})$, the equilibrium constant for the reaction $\mathrm{H}_2(g)+\mathrm{Br}_2(\mathrm{~g}) \rightleftharpoons 2 \mathrm{HBr}(\mathrm{g})$

is $1.6 \times 10^5$. If 10 bar of HBr is introduced into a sealed vessel at $T(\mathrm{~K})$, the equilibrium pressure of HBr (in bar) is approximately

At equilibrium of the reaction,

$$A_2(g)+B_2(g) \rightleftharpoons 2 A B(g)$$

The concentrations of $A_2, B_2$ and $A B$ respectively are $15 \times 10^{-3} \mathrm{M}, 2.1 \times 10^{-3} \mathrm{M}$, and $1.4 \times 10^{-3} \mathrm{M}$ in a sealed vessel at 800 K . What will be $K_p$ for the decomposition of $A B$ at same temperature ?

At $293 \mathrm{~K}, \Delta_r G^{\circ}$ for the following reaction is $165.469 \mathrm{~kJ} \mathrm{~mol}^{-1}$.

$$\frac{3}{2} \mathrm{O}_2(\mathrm{~g}) \longrightarrow \mathrm{O}_3(\mathrm{~g})$$

What is the equilibrium constant for this reaction?

$$\left(R=83 \mathrm{~J} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}\right)$$

The following equilibrium is established at STP.

$$B_2(g) \rightleftharpoons 2 B(g)$$

Atoms of $B$ occupy $20 \%$ of total volume at STP. The total pressure of the system is 1 bar. What is its $K_p$ ? $($ STP volume $=22.7 \mathrm{~L})$

At 298 K , the value of $K_c$ for the following reaction is $x \mathrm{~mol} \mathrm{~L}^{-1}$.

What is the approximate $K_{\mathrm{P}}$ value for this reaction?

$$\begin{array}{r} \left(R=0.082 \mathrm{~L} \mathrm{~atm} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}\right) \\ \mathrm{A}_2 \mathrm{O}_4(\mathrm{~g}) \rightleftharpoons 2 \mathrm{AO}_2(\mathrm{~g}) \end{array}$$