Embibe Experts Solutions for Chapter: Equilibrium, Exercise 1: JEE Main - 1 February 2023 Shift 2

Water decomposes at $2300 \mathrm{K}$

${\mathrm{H}}_2\mathrm{O}\left(\mathrm{g}\right)\to {\mathrm{H}}_2\left(\mathrm{g}\right)+\frac{1}{2}{\mathrm{O}}_2\left(\mathrm{g}\right)$

The percent of water decomposing at $2300 \mathrm{K}$ and 1 bar is _____ (Nearest integer). Equilibrium constant for the reaction is $2\times {10}^{-3}$ at $2300 \mathrm{K}$

At $298 \mathrm{K}$

${\mathrm{N}}_2\left(\mathrm{g}\right)+3{\mathrm{H}}_2\left(\mathrm{g}\right)\rightleftharpoons 2{\mathrm{NH}}_3\left(\mathrm{g}\right),{\mathrm{K}}_1=4\times {10}^5$

${\mathrm{N}}_2\left(\mathrm{g}\right)+{\mathrm{O}}_2\left(\mathrm{g}\right)\rightleftharpoons 2\mathrm{NO}\left(\mathrm{g}\right),{\mathrm{K}}_2=1.6\times {10}^{12}$

${\mathrm{H}}_2\left(\mathrm{g}\right)+\frac{1}{2}{\mathrm{O}}_2\left(\mathrm{g}\right)\rightleftharpoons {\mathrm{H}}_2\mathrm{O}\left(\mathrm{g}\right),{\mathrm{K}}_3=1.0\times {10}^{-13}$

Based on above equilibria, the equilibrium constant of the reaction,

$2{\mathrm{NH}}_3\left(\mathrm{g}\right)+\frac{5}{2}{\mathrm{O}}_2( \mathrm{g})\rightleftharpoons 2\mathrm{NO}\left(\mathrm{g}\right)+3{\mathrm{H}}_2\mathrm{O}\left(\mathrm{g}\right)$
is _____ $\times {10}^{-33}$ (Nearest integer)

$600\mathrm{mL}$ of $0.01\mathrm{M} \mathrm{HCl}$ is mixed with $400\mathrm{mL}$ of $0.01\mathrm{M} {\mathrm{H}}_2{\mathrm{SO}}_4$. The $\mathrm{pH}$ of the mixture is _____$\times {10}^{-2}$. (Nearest integer)

[Given $\log 2=0.30, \log 3=0.48, \log 5=0.69, \log 7=0.84, \log 11=1.04$]

Consider the following equation:

$2{\mathrm{SO}}_2\left(\mathrm{g}\right)+{\mathrm{O}}_2\left(\mathrm{g}\right)\rightleftharpoons 2{\mathrm{SO}}_3\left(\mathrm{g}\right),\mathrm{\Delta H}=-190 \mathrm{kJ}$.

The number of factors which will increase the yield of ${\mathrm{SO}}_3$ at equilibrium from the following is _____ .

A. Increasing temperature
B. Increasing pressure
C. Adding more ${\mathrm{SO}}_2$
D. Adding more ${\mathrm{O}}_2$
E. Addition of catalyst

For reaction: ${\mathrm{SO}}_2( \mathrm{g})+\frac{1}{2}{\mathrm{O}}_2( \mathrm{g})\rightleftharpoons {\mathrm{SO}}_3( \mathrm{g})$ ${\mathrm{K}}_{\mathrm{P}}=2\times {10}^{12}$ at $27°\mathrm{C}$ and $1 \mathrm{atm}$ pressure. The ${\mathrm{K}}_{\mathrm{c}}$ for the same reaction is $\mathrm{x}\times {10}^{13}.$ (Nearest integer)
(Given $\mathrm{R}=0.082 \mathrm{L} \mathrm{atm} {\mathrm{K}}^{-1} {\mathrm{mol}}^{-1}$ )

At $298 \mathrm{K}$, the solubility of silver chloride in water is $1.434\times {10}^{-3} \mathrm{g} {\mathrm{L}}^{-1}$. The value of $-{\mathrm{logK}}_{\mathrm{sp}}$ for silver chloride is
(Given mass of Ag is $107.9 \mathrm{g} {\mathrm{mol}}^{-1}$, and mass of $\mathrm{Cl}$ is $35.5 \mathrm{g} {\mathrm{mol}}^{-1}$ )

(i) $\mathrm{X}\left(\mathrm{g}\right)\rightleftharpoons \mathrm{Y}\left(\mathrm{g}\right)+\mathrm{Z}\left(\mathrm{g}\right) {\mathrm{K}}_{\mathrm{p}1}=3$

(ii) $\mathrm{A}\left(\mathrm{g}\right)\rightleftharpoons 2 \mathrm{B}( \mathrm{g}) {\mathrm{K}}_{\mathrm{p}2}=1$

If the degree of dissociation and initial concentration of both the reactants $\mathrm{X}( \mathrm{g})$ and $\mathrm{A}\left(\mathrm{g}\right)$ are equal, then the ratio of the total pressure at equilibrium $\left(\frac{p_1}{p_2}\right)$ is equal to $\mathrm{x}: 1$. The value of $\mathrm{x}$ is (Nearest integer)

The effect of addition of helium gas to the following reaction in equilibrium state at constant volume, is :
${\mathrm{PCI}}_5( \mathrm{g})\rightleftharpoons {\mathrm{PCl}}_3( \mathrm{g})+{\mathrm{Cl}}_2( \mathrm{g})$