iCON Education - Chemical Equilibrium AP-EAPCET Test

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 } $

$\frac{K_3^2}{K_1 \times K_2}$

$\frac{K_3^3}{K_1^2 \times K_2}$

$\frac{K_3^2}{K_1^2 \times K_2}$

$\frac{K_3}{K_1^{\frac{1}{2}} \times K_2^2}$

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 $300 \mathrm{~K}, K_C$ for the reaction. $ A_2 B_2(g) \rightleftharpoons A_2(g)+B_2(g) $ is $100 \mathrm{~mol} \mathrm{~L}^{-1}$, What is its $K_p$ (in atm ) at the same temperature ? $\left(R=0.082 \mathrm{~L} \mathrm{~atm} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}\right)$

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 ?

15 moles of $\mathrm{H}_2$ and 5.2 moles of $\mathrm{I}_2$ are mixed and allowed to attain equilibrium at 773 K . At equilibrium, the number of moles of HI is found to be 10 . The equilibrium constant for the dissociation of HI is

$K_C$ for the reaction,
$A_2(g) \stackrel{T(\mathrm{~K})}{\rightleftharpoons} B_2(\mathrm{~g})$
is 39.0. In a closed one litre flask, one mole of $A_2(g)$ was heated to $T(\mathrm{~K})$. What are the concentrations of $A_2(g)$ and $B_2(g)$ (in mol L ${ }^{-1}$ ) respectively at equilibrium?

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

$K_C$ for the reaction, $A_2(g) \stackrel{T(\mathrm{~K})}{\rightleftharpoons} B_2(g)$ is 99.0 . In a 1 L closed flask two moles of $B_2(g)$ is heated to $T(\mathrm{~K})$. What is the concentration of $B_2(g)\left(\right.$ in $\left.\mathrm{mol} \mathrm{L}^{-1}\right)$ at equilibrium?

$K_{\mathrm{c}}$ 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 $T(\mathrm{~K}), K_c$ for the reaction $A_2(g) \rightleftharpoons B_2(g)$ is 99.0 . Two moles of $A_2(s)$ was heated to $T(\mathrm{~K})$ in a 1 L . closed flask to reach the above equilibrium. What are the concentrations (in mol $\mathrm{L}^{-1}$ ) of $A_2(g)$ and $B_2(g)$ respectively at equilibrium?

At $27^{\circ} \mathrm{C}$, the degree of dissociation of weak acid ( $\mathrm{H} A$ ) in its 0.5 M aqueous solution is $1 \%$. Its $K_e$, value is approximately

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

$2.1 \times 10^{-4}$

$2.1 \times 10^{-5}$

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

the rate of the forward reaction becomes zero.

no effect of temperature.

forward reaction is favoured

backward reaction is favoured

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

$-650 \mathrm{~J} \mathrm{~mol}^{-1}$

$-830 \mathrm{~J} \mathrm{~mol}^{-1}$

$-790 \mathrm{~J~mol}^{-1}$

$-875 \mathrm{~J} \mathrm{~mol}^{-1}$

Le-Chatelier's principle is not applicable to

$\mathrm{H}_2(g)+\mathrm{I}_2(g) \rightleftharpoons 2 \mathrm{HI}(g)$

$\mathrm{Fe}(\mathrm{s})+\mathrm{S}(\mathrm{s}) \rightleftharpoons \mathrm{FeS}(\mathrm{s})$

$\mathrm{N}_2(g)+3 \mathrm{H}_2(g) \rightleftharpoons 2 \mathrm{NH}_3(g)$

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

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

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

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

$3.162 \times 10^{-4}$

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?

AP EAPCET 2021 - 19th August Morning Shift Chemistry - Chemical Equilibrium Question 28 English

Pressure has no effect

$p_1=p_2=p_3 \neq 0$

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

$K_c=\left(K_p\right)^2$