Embibe Experts Solutions for Chapter: Equilibrium, Exercise 1: CG PET 2019

For the reaction

$2 {{\mathrm{NO}}_2}_{\left(\mathrm{g}\right)} \rightleftharpoons 2{\mathrm{NO}}_{\left(\mathrm{g}\right)} + {\mathrm{O}}_{2\left(\mathrm{g}\right)}$

${\mathrm{K}}_{\mathrm{c}}=1.8\times {10}^{-6} \mathrm{mol} {\mathrm{L}}^{-1}$ at $184 °\mathrm{C}$

$\mathrm{R} = 0.0831 \mathrm{L} \mathrm{bar} {\mathrm{K}}^{-1} {\mathrm{mol}}^{-1}$

The relationship between ${\mathrm{K}}_{\mathrm{p}}$ and ${\mathrm{K}}_{\mathrm{c}}$ at $184 °\mathrm{C}$ is

The decomposition of dinitrogen tetroxide at$300 \mathrm{K}$ and $1.0$ atm pressure is $20\%$. At equilibrium, the partial pressure (in atm) of a nitrogen peroxide is
 

In a $100 \mathrm{mL}$ of buffer solution of acetic acid and sodium acetate, both are $0.1 \mathrm{mol}$. In this buffer, $10 \mathrm{mL}$ of $0.01 \mathrm{mole}$ of $\mathrm{HCl}$ is added. The $\mathrm{pH}$ of the buffer

What is the solubility of silver bromide in one litre of$0.4$ molar ${\mathrm{NH}}_3$ solution $\left({\mathrm{K}}_{\mathrm{f}}\right({\left[\mathrm{Ag}{\left({\mathrm{NH}}_3\right)}_2\right]}^{+})=1.0\times {10}^8 )$?

Given that ${\mathrm{K}}_{\mathrm{sp}}\left(\mathrm{AgBr}\right)=3.3\times {10}^{-13}$

A metal halide has molar concentration of $0.000011 \mathrm{mol}/\mathrm{L}$ in saturated state. If its ${\mathrm{K}}_{\mathrm{sp}}=39.5\times {10}^{-20}$, then the halide is

If solubility of $\mathrm{M}{\left(\mathrm{OH}\right)}_3$ is $\mathrm{S}$, its solubility product will be: