Physical Chemistry PYQ — Page 62

If$100\mathrm{mole}$ of ${H}_{2}{O}_{2}$ decompose at $1\mathrm{bar}$ and $300K$, the work is done ($\mathrm{kJ}$) by one mole of ${O}_{2}(g)$ as it expands against $1\mathrm{bar}$ pressure is: $2{H}_{2}{O}_{2}(l)\rightleftharpoons 2{H}_{2}O(l)+{O}_{2}(g)$ $(R=8.3 J {K}^{-1} {\mathrm{mol}}^{-1})$

The rate law for the reaction below is given by the expression $k[A][B]$ $A+B\rightarrow Product$ If the concentration of $B$ is increased from $0.1\mathrm{to}0.3\mathrm{mol}$, keeping the value of $A$ at $0.1\mathrm{mol}$, the rate constant will be:

Galvanization is applying a coating of:

The heats of combustion of carbon and carbon monoxide are $-393.5 and-283.5 kJ mo{l}^{-1},$ respectively. The heat of formation $(\mathrm{in}\mathrm{kJ})$ of carbon monoxide per mole is:

Aqueous solution of which of the following salts will not contain ions with the electronic configuration $1{s}^{2}2{s}^{2}2{p}^{6}3{s}^{2}3{p}^{6}$ ?

The reaction of ozone with oxygen atoms in the presence of chlorine atoms can occur by a two step process shown below: ${O}_{3}(g)+{\mathrm{Cl}}^{•}\rightarrow {O}_{2}(g)+{\mathrm{ClO}}^{•}(g)$ ...(i) ${k}_{i}=5.2\times {10}^{9} L mo{l}^{-1} {s}^{-1}$ ${\mathrm{ClO}}^{•}(g)+{O}^{•}(g)\rightarrow {O}_{2}(g)+{\mathrm{Cl}}^{•}(g)$ ...(ii) ${k}_{ii}=2.6\times {10}^{10} L mo{l}^{-1} {s}^{-1}$ The closest rate constant for the overall reaction ${O}_{3}(g)+{O}^{•}(g)\rightarrow 2{O}_{2}(g)$ is:

The solubility of ${N}_{2}$ in water at $\text{300} \text{K}$ and $\text{500} \text{torr}$ partial pressure is $0.01g{L}^{-1}.$ The solubility (in ${ \text{g L}}^{ -\text{1}}$ ) at $\text{750} \text{torr}$ partial pressure is:

Identify the correct statement:

An aqueous solution of a salt $M{X}_{2}$ at certain temperature has a Van't Hoff factor of $2$. What is the degree of dissociation for this solution of the salt?

The equilibrium constant at $298K$ for a reaction $A+B\rightleftharpoons C+D$ is $100$. If the initial concentration of all the four species were$1M$ each, then the equilibrium concentration of $D$ (in mol ${L}^{-1}$) will be:

The amount of arsenic pentasulphide that can be obtained when $35.5g$ arsenic acid is treated with excess ${H}_{2}S$ in the presence of conc. $\mathrm{HCl}$ (assuming $100%$ conversion) is

A solid $\mathrm{XY}$kept in an evacuated sealed container undergoes decomposition to form a mixture of gases $X\mathrm{and}Y$ at temperature $T$. The equilibrium pressure is $10\mathrm{bar}$ in this vessel. ${K}_{p}$ for this reaction is?

A solution at ${\text{20}}^{\text{o}}\text{C}$ is composed of 1.5 mol of benzene and 3.5 mol of toluene. If the vapour pressure of pure benzene and pure toluene at this temperature are 74.7 torr and 22.3 torr respectively, then the total vapour pressure of the solution and the benzene mole fraction in equilibrium with it will be, respectively:

A variable, the opposite external potential $({E}_{\mathrm{ext}})$ is applied to the cell $Zn | Z{n}^{2+} (1M)\parallel C{u}^{2+} (1 M)| Cu$, of potential $1.1V$. When ${E}_{ext}<1.1 V$ and ${E}_{ext}>1.1 V$, respectively electrons flow from

Which of the following is the energy of a possible excited state of hydrogen?

The standard Gibbs energy change at 300 K for the reaction $2A\rightleftharpoons B+C$ is 2494.2 J. At a given time, the composition of the reaction mixture is $[A]=\frac{1}{2}, [B]=2$ and $[C]=\frac{1}{2}$ . The reaction proceeds in the: $[R=8.314 J/K-mol , e=2.718]$ {Given antilog (-0.44)=0.36}

For the equilibrium, $A(g)\rightleftharpoons B(g), \Delta H\mathrm{is}-40\mathrm{kJ}/\mathrm{mol}$ . If the ratio of the activation energies of the forward $({E}_{f})$ and reverse $({E}_{b})$ reactions is $\frac{2}{3}$ then:

Higher order (>3) reactions are rare due to:

The heat of atomization of methane and ethane are $360\mathrm{kJ}{\mathrm{mol}}^{-1}$ and $620\mathrm{kJ}{\mathrm{mol}}^{-1}$, respectively. The longest wavelength of light capable of breaking the $C-C$ bond is (Avogadro's number$=6.023\times {10}^{23}, h=6.62\times {10}^{-34} J s$)

$A+2B\rightarrow C$ , the rate equation for the reaction is given as Rate $=k[A][B]$ If the concentration of A is kept the same but that of B is doubled what will happen to the rate itself?

At temperature $T$, the average kinetic energy of any particle is $\frac{3}{2}\mathrm{kT}$. The de Broglie wavelength follows the order:

An element $X$ shows $+3$, oxidation state in its compounds. Out of the four compounds given below, choose the incorrect formula for the element $X$.

Two Faraday of electricity is passed through a solution of $CuS{O}_{4}$ . The mass of copper deposited at the cathode is: (Atomic mass of Cu = 63.5 amu)

In the following reaction: $A+2B+3C\rightleftharpoons A{B}_{2}{C}_{3}$ $6.0g$ of $A$, $6.0\times {10}^{23}$ atoms of $B$ and $0.036\mathrm{mol}$ of $C$ reacted and formed $4.8g$ of compound $A{B}_{2}{C}_{3}$. If the atomic mass of $A$ and $C$ are $60$ and $80\mathrm{amu}$, respectively. What is the atomic mass of $B$ in $\mathrm{amu}$? (Avogadro number$=6\times {10}^{23}$)