Embibe Experts Solutions for Chapter: Equilibrium, Exercise 2: EXERCISE-2

The equation, $\mathrm{a}=\frac{\mathrm{D}-\mathrm{d}}{(\mathrm{n}-1)\mathrm{d}}$ is correctly matched for :

The percentage of ammonia obtainable, if equilibrium were to be established during the Haber process, is plotted against the operating pressure for two temperatures $400°\mathrm{C}$ and $500°\mathrm{C}.$ Which of the following correctly represents the two graphs ?

For the synthesis of ${\mathrm{NH}}_3$ from the Haber process starting with stoichiometric amount of ${\mathrm{N}}_2$ and ${\mathrm{H}}_2,$ the attainment of equilibrium is predicted by which curve :-

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

The rate constant for the forward reaction $\mathrm{A}\left(\mathrm{g}\right)\rightleftharpoons 2 \mathrm{B}\left(\mathrm{g}\right)$ is $1.5\times {10}^{-3}{ \mathrm{s}}^{-1}$ at $100 \mathrm{K}.$ If ${10}^{-5}$ moles of $\mathrm{A}$ and $100$ moles of $\mathrm{B}$ are present in a $10$ litre vessel at equilibrium then rate constant for the backward reaction at this temperature is :-

For the reacton $\mathrm{A}+2\mathrm{B}\rightleftharpoons \mathrm{C}+\mathrm{D},$ the equilibrium constant ${\mathrm{K}}_{\mathrm{C}}={10}^9.$ If the initial moles of $\mathrm{A}, \mathrm{B}, \mathrm{C}$ and $\mathrm{D}$ are $0.5, 1, 3.5$ and $0.5$ moles respectively in a one litre vessel, what is the equilibrium conc. of $\mathrm{B}$ at equilibrium :-

Which of the following statements(s) is/are incorrect:

Statement $\left(\mathrm{a}\right)$ $:$ $16 \mathrm{gm}$ of ${\mathrm{O}}_2$ contains ${\mathrm{N}}_{\mathrm{A}}$ oxygen atoms

Statement $\left(\mathrm{b}\right)$ $:$ For an aqueous solution to be netral it must have $\mathrm{pH}=7$

Statement $\left(\mathrm{c}\right) :$ For the reactions

$\frac{1}{2}{ \mathrm{N}}_2+\frac{1}{2}{\mathrm{O}}_2\rightleftharpoons \mathrm{NO}$      equilibrium constant is ${\mathrm{K}}_1$

and $2\mathrm{NO}\rightleftharpoons {\mathrm{N}}_2+{\mathrm{O}}_2$  equilibrium constant is ${\mathrm{K}}_2$

then ${\mathrm{K}}_2·{\mathrm{K}}_1=1$

Statement $\left(\mathrm{d}\right) :$ Whenever $\alpha$-particles emits $\mathrm{n}/\mathrm{p}$ ratio slightyl increase

Give the correct order of initials $\mathrm{T}$ (true) of $\mathrm{F}$ (false) for following statements.

$\left(\mathrm{i}\right)$ On decreasing pressure to the equilibrium ${\mathrm{H}}_2\mathrm{O}\left(\mathrm{s}\right)\rightleftharpoons {\mathrm{H}}_2\mathrm{O}\left(\ell \right),$ more ice will be formed

$\left(\mathrm{ii}\right)$ At equilibrium, if ${\mathrm{K}}_0=1,$ then $\mathrm{\Delta G}°<1$

$\left(\mathrm{iii}\right)$ For the reaction $2{\mathrm{SO}}_2\left(\mathrm{g}\right)+{\mathrm{O}}_2\left(\mathrm{g}\right)\rightleftharpoons 2{\mathrm{SO}}_3\left(\mathrm{g}\right), {\mathrm{K}}_{\mathrm{p}}$ is less than ${\mathrm{K}}_{\mathrm{c}}$

$\left(\mathrm{iv}\right)$ Data for the given reaction ${\mathrm{N}}_2{\mathrm{O}}_4\left(\mathrm{g}\right)\to 2{\mathrm{NO}}_2\left(\mathrm{g}\right); \mathrm{\Delta H}=5.4 \mathrm{kJ}, {\mathrm{E}}_{\mathrm{a}}$ (forward) $=57.2 \mathrm{kJ}$

Then activation energy for the reverse reaction is $3.2 \mathrm{kJ}$

For a reversible reaction ${\mathrm{N}}_2+3{\mathrm{H}}_2\rightleftharpoons 2{\mathrm{NH}}_3$ at equilibrium if some moles of ${\mathrm{H}}_2$ are replaced by same number of moles of ${\mathrm{T}}_2( \mathrm{T}$ is Tritium, isotope of $\mathrm{H}$$\&$ assume isotopes do not have different chemical properties) without affecting other parameters.