Chemical Equilibrium · Chemistry · AP EAPCET

At $T(\mathrm{~K}), K_c$ value of $A \mathrm{O}_2(g)+B \mathrm{O}_2(g) \rightleftharpoons A \mathrm{O}_3(g)+B O(g)$ is 16 . In a closed 1 L flask, one mole each of $A O_2, B O_2 A \mathrm{O}_3$ and $B \mathrm{O}$ are taken and heated to $T(\mathrm{~K})$. Identify the correct statements about this equilibrium.

I. Total number of moles at equilibrium is 4 .

II. At equilibrium, the ratio of moles of $A \mathrm{O}_2$ and $A \mathrm{O}_3$ is $1: 4$.

III. Total number of moles of $A \mathrm{O}_2$ and $B \mathrm{O}_2$ at equilibrium is 0.8 .

Consider the following equilibrium reaction in gaseous state at $T(\mathrm{~K})$.

$$ A+2 B \rightleftharpoons 2 C+D $$

The initial concentration of $B$ is 1.5 times that of $A$. At equilibrium, the concentrations of $A$ and $B$ are equal. The equilibrium constant for the reaction is

For the following given equilibrium reaction $\frac{K_c}{K_p}$ is equal to 1076 at $T(\mathrm{~K})$. What is the value of $T$ (in K )?

$$ \begin{aligned} & \left(R=0.082 \mathrm{~L}-\mathrm{atm} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}\right) \\ & \mathrm{N}_2(\mathrm{~g})+3 \mathrm{H}_2(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NH}_3(\mathrm{~g}) \end{aligned} $$

At $T(\mathrm{~K})$, consider the following gaseous reaction, which is in equilibrium.

$$ \mathrm{N}_2 \mathrm{O}_5 \rightleftharpoons 2 \mathrm{NO}_2+\frac{1}{2} \mathrm{O}_2 $$

What is the fraction of $\mathrm{N}_2 \mathrm{O}_5$ decomposed at constant volume and temperature, if the initial pressure is 300 mm Hg and pressure at equilibrium is 480 mm Hg ? (Assume all gases as ideal)

At 298 K , the value of $K_p$ for $\mathrm{N}_2 \mathrm{O}_4(g) \rightleftharpoons 2 \mathrm{NO}_2(g)$ is 0.113 atm . The partial pressure of $\mathrm{N}_2 \mathrm{O}_4$ at equilibrium is 0.2 atm . What is the partial pressure (in atm) of $\mathrm{NO}_2$ equilibrium?

Consider the following gaseous equilibrium reactions (I), (II) and (III) with equilibrium constants $K_1, K_2$ and $K_3$ respectively

(I) $\frac{1}{2} \mathrm{~N}_2+\frac{3}{2} \mathrm{H}_2 \rightleftharpoons \mathrm{NH}_3$

(II) $2 \mathrm{NO} \rightleftharpoons \mathrm{N}_2+\mathrm{O}_2$

(III) $\mathrm{H}_2+\frac{1}{2} \mathrm{O}_2 \rightleftharpoons \mathrm{H}_2 \mathrm{O}$

The correct expression for the equilibrium constant for the gaseous equilibrium reaction

$$ 2 \mathrm{NH}_3+\frac{5}{2} \mathrm{O}_2 \rightleftharpoons 2 \mathrm{NO}+3 \mathrm{H}_2 \mathrm{O} \text { is } $$

At $T(\mathrm{~K})$, the following gaseous equilibrium is established.

$$ W+X \rightleftharpoons Y+Z $$

The initial concentration of $W$ is two times to the initial concentration of $X$. The system is heated to $T(\mathrm{~K})$ to establish the equilibrium. At equilibrium the concentration of $Y$ is four times to the concentration of $X$. What is the value of $K_C$ ?

At $T(\mathrm{~K}), K_C$ value for

$\mathrm{AO}_2(\mathrm{~g})+\mathrm{BO}_2(\mathrm{~g}) \rightleftharpoons \mathrm{AO}_3(\mathrm{~g})+\mathrm{BO}(\mathrm{g})$ is 16 . In a closed 1 L flask, one mole each of $A \mathrm{O}_2, B \mathrm{O}_2, A \mathrm{O}_3$ and $B \mathrm{O}$ are taken and heated to $T(\mathrm{~K})$.

What is the concentration (in $\mathrm{mol} \mathrm{L}^{-1}$ ) of $\mathrm{AO}_3$ at equilibrium?

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?

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

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 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 $T(\mathrm{~K})$, 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

$K_{\mathrm{c}}$ 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 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 $$\left.\mathrm{mol}^{-1} \mathrm{~K}^{-1}\right)$$.

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

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

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: $$\Delta H \Upsilon=-30 \mathrm{~kJ}$$]

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

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?

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