Physical Chemistry PYQ — Page 62

Identify the correct statement:

$18g$ glucose $({C}_{6}{H}_{12}{O}_{6})$ is added to $178.2g$ water. The vapour pressure of water (in torr) for this aqueous solution is:

Galvanization is applying a coating of:

For the reaction, $A(g)+B(g)\rightarrow C(g)+D(g), \Delta {H}^{o}$ and $\Delta {S}^{o}$ are, respectively, $-29.8 kJ mo{l}^{-1}$ and $-0.100 kJ {K}^{-1} mo{l}^{-1}$ at 298 K. The equilibrium constant for the reaction at 298 k is:

Decomposition of ${H}_{2}{O}_{2}$ follows a first order reaction. In fifty minutes the concentration of ${\text{H}}_{2} {\text{O}}_{2}$ decreases from $0.5$ to $0.125 M$ in one such decomposition. When the concentration of ${H}_{2}{O}_{2}$ reaches $0.05 M$ , the rate of formation of ${O}_{2}$ will be:

At $300K$ and $1\mathrm{atm}$, $15\mathrm{mL}$ of a gaseous hydrocarbon requires $375\mathrm{mL}$ air containing $20%{O}_{2}$ by volume, for complete combustion. After combustion, the gases occupy $345\mathrm{mL}$. Assuming that the water formed is in liquid form and the volumes were measured at the same temperature and pressure, the formula of the hydrocarbon is: (Assume complete combustion of reactant)

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

An organic compound contains $C,H$ and $S$. The minimum molecular weight of the compound containing $8%$ Sulphur is

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?

A stream of electrons from a heat filament was passed between two charge plates kept at a potential difference $V\mathrm{esu}$. If $e$ and $m$ are charge and mass of an electron, respectively, then the value of $\frac{h}{\lambda }$ (where $\lambda$ is wavelength associated with the electron wave) is given by:

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 reaction at 1 bar is non-spontaneous at low temperature but becomes spontaneous at high temperature. Identify the correct statement about the reaction among the following:

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

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)

The vapour pressure of acetone at ${20}^{o}C$ is $185\mathrm{torr}$. When $1.2g$ of a non-volatile substance was dissolved in $100g$ of acetone at ${20}^{o}C$ , its vapour pressure was $183\mathrm{torr}$. The molar mass $(g mo{l}^{-1})$ of the substance is:

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}

The reaction $2{N}_{2}{O}_{5}(g)\rightarrow 4N{O}_{2}(g)+{O}_{2}(g)$ follows first order kinetics. The pressure of a vessel containing only ${N}_{2}{O}_{5}$ was found to increase from 50 mm Hg to 87.5 mm Hg in 30 min. The pressure exerted by the gases after 60 min. Will be (Assume temperature remains constant) :

$A+2B\rightarrow C$ , 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?

The molecular formula of a commercial resin used for exchanging ions in water softening is ${C}_{8}{H}_{7}S{O}_{3}Na$ $(\mathrm{molecular}\mathrm{weight}=206)$. What would be the maximum uptake of $C{a}^{2+}$ ions by the resin if expressed in $\mathrm{mol}$ per $\mathrm{gm}$?

The increase of pressure on $ice \rightleftharpoons water$ system at constant temperature will lead 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$=6.023\times {10}^{23}, h=6.62\times {10}^{-34} J s$)

The following reaction is performed at $298K$. $2NO(g)+{O}_{2}(g)\rightleftharpoons 2N{O}_{2}(g)$ The standard free energy of the formation of $NO(g)$ is $86.6\mathrm{kJ}{\mathrm{mol}}^{-1}$ at $298K$. What is the standard free energy of the formation of $N{O}_{2}(g)$ at $298K$? $({K}_{P}=1.6\times {10}^{12})$

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$=6\times {10}^{23}$)

If the principal quantum number $\text{n}=6,$ the correct sequence of filling of electrons will be: