Physical Chemistry PYQ — Page 57

The given plots represent the variation of the concentration of a reactant $R$ with time for two different reactions $(i)\mathrm{and}(\mathrm{ii})$. The respective orders of the reaction are (i)  (ii) 

Consider the reaction $\mathrm{N}_{2}(\mathrm{~g})+3 \mathrm{H}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NH}_{3}(\mathrm{~g})$ The equilibrium constant of the above reaction is $\mathrm{K}_{\mathrm{P}}$. If pure ammonia is left to dissociate, the partial pressure of ammonia at equilibrium is given by (Assume that $\mathrm{P}_{\mathrm{NH}_{3}}< < \mathrm{P}_{\text {total }}$ at equilibrium)

An example of a disproportionation reaction is

Calculate the standard cell potential (in V) of the cell in which the following reaction takes place: ${Fe}^{2+} (aq)+A{g}^{+}(aq)\rightarrow F{e}^{3+}(aq)+Ag(s)$ Given that ${E}_{{\mathrm{Ag}}^{+}/Ag}^{o}=x V$ ${E}_{{Fe}^{2+}/Fe}^{o}=y V$ ${E}_{{Fe}^{3+}/Fe}^{o}=z V$

For a reaction scheme $A\overset{{ k}_{1} }{\rightarrow }B\overset{{ k}_{2} }{\rightarrow }C,$ if the net rate of formation of B is set to be zero then the concentration of B is given by:

What is the molar solubility of $AI{(OH)}_{3}$ in $0.2$ $M NaOH$ solution? Given that, solubility product of $\mathrm{Al}{(OH)}_{3}=2.4\times {10}^{-24}$ :

The standard electrode potential ${E}^{o}$ and its temperature coefficient $(\frac{\mathrm{dE}}{\mathrm{dT}})$ for a cell are $2V$ and $-5{\times 10}^{-4} V{K}^{-1}$ at $300 K$, respectively. The reaction is $\mathrm{Zn}(s)+{\mathrm{Cu}}^{2+}(\mathrm{aq})\rightarrow {\mathrm{Zn}}^{2+}(\mathrm{aq})+\mathrm{Cu}(s)$. The standard reaction enthalpy $({\Delta }_{r}{H}^{-})$ at $300K$ in $mo{l}^{-1}$ is $[$Use $R=8J{K}^{-1}{\mathrm{mol}}^{-1}$ and $F=96,500C{\mathrm{mol}}^{-1}]$

At room temperature, a dilute solution of urea is prepared by dissolving $0.60 g$ of urea in $360 g$ of water. If the vapour pressure of pure water at this temperature is $35 mm Hg$ , lowering of vapour pressure will be: (molar mass of urea $=60 g mo{l}^{-1}$ )

A mixture of $100 m\mathrm{mol}$ of $\mathrm{Ca}{(\mathrm{OH})}_{2}$ and $2g$ of sodium sulphate was dissolved in water and the volume was made up to $100 \mathrm{mL}.$ What is the mass of calcium sulphate formed and the concentration of ${\mathrm{OH}}^{-}$ in resulting solution, respectively? (Molar mass of $\mathrm{Ca}{(\mathrm{OH})}_{2}, {\mathrm{Na}}_{2}{\mathrm{SO}}_{4}$ and ${\mathrm{CaSO}}_{4}$ are $74, 143$ and $136g {\mathrm{mol}}^{-1},$ respectively; ${K}_{\mathrm{sp}}$ of $\mathrm{Ca}{(\mathrm{OH})}_{2}\mathrm{is} 5.5\times {10}^{-6}$)

Liquids $A$ and $B$ form an ideal solution in the entire composition range. At $350K,$ the vapour pressure of pure A and pure B are $7\times {10}^{3}\mathrm{Pa}$ and $12\times {10}^{3}\mathrm{Pa}$ , respectively. The composition of the vapour in equilibrium with a solution containing 40 mole percent of A at this temperature is:

The amphoteric hydroxide is:

Among the following, the set of parameters that represents path functions, is: i) $q+w$ ii) $q$ iii) $w$ iv) $H-TS$

The quantum number of four electrons are given below: $I. n=4, l=2, {m}_{l}=–2, {m}_{s}=–1/2$ $II. n=3, l=2, {m}_{l}=1, {m}_{s}=+1/2$ $III. n=4, l=1, {m}_{l}=0, {m}_{s}=+1/2$ $IV. n=3, l=1, {m}_{l}=1, {m}_{s}=–1/2$ The correct order of their increasing energies will be:

A solution containing $62 g$ ethylene glycol in $250 g$ water is cooled to $-{10}^{o}C$ . If ${K}_{f}$ for water is $1.86 K \mathrm{kg} {\mathrm{mol}}^{-1}$ , the amount of water (in $g$ ) separated as ice is:

Given: $(i)$ $\text{C}(\mathrm{graphite})+{O}_{2}(g)\rightarrow {\mathrm{CO}}_{2}(g);$ ${\Delta rH}^{\Theta }=x \mathrm{kJ} {\mathrm{mol}}^{-1}$ $(\mathrm{ii})$ $C(\mathrm{graphite})+\frac{1}{2}{O}_{2}(g)\rightarrow \mathrm{CO}(g);$ ${\Delta rH}^{\Theta }=y \mathrm{kJ} {\mathrm{mol}}^{-1}$ $(\mathrm{iii}) \mathrm{CO}(g)+\frac{1}{2}{O}_{2}(g)\rightarrow {\mathrm{CO}}_{2}(g);$ ${\Delta rH}^{\Theta }=z \mathrm{kJ} {\mathrm{mol}}^{-1}$ Based on the above thermochemical equations, find out which one of the following algebraic relationships is correct?

$25 \mathrm{~mL}$ of the given $\mathrm{HCl}$ solution requires $30 \mathrm{~mL}$ of $0.1 \mathrm{M}$ sodium carbonate solution. What is the volume of this $\mathrm{HCl}$ solution required to titrate $30 \mathrm{~mL}$ of $0.2 \mathrm{M}$ aqueous $\mathrm{NaOH}$ solution?

Which of the graphs shown below does not represent the relationship between incident light and the electron ejected from metal surface?

Two blocks of the same metal having same mass and at temperature $\mathrm{T}_{1},$ and $\mathrm{T}_{2}$, respectively, are brought in contact with each other and allowed to attain thermal equilibrium at constant pressure. The change in entropy, $\Delta \mathrm{S}$, for this process is :

Consider the statements $S1$ and $S2$ : $S1$ : Conductivity always increases with decreases in the concentration of electrolyte. $S2$ : Molar conductivity always increases with decreases in the concentration of electrolyte. The correct option among the following

Liquid $M$ and liquid $N$ form an ideal solution. The vapour pressures of pure liquids $M$ and $N$ are $450$ and $700 mmHg,$ respectively, at the same temperature. Then correct statements is: ( ${x}_{M}=Mole fraction of {'M}^{'} in solution;$ ${x}_{N}=Mole fraction of {'N}^{'}in solution;$ ${y}_{M}=Mole fraction of {'M}^{'} in vapour phase;$ ${y}_{N}=Mole fraction of {'N}^{'} in vapour phase;$ )

The graph between ${|\psi |}^{2}$ and $r$ (radical distance) is shown below. This represents: 

For an elementary chemical reaction, ${A}_{2}⇄_{{k}_{-1}}^{{k}_{1}}2A$ , the expression for $\frac{d[A]}{\mathrm{dt}}$ is:

During compression of a spring the work done is $10 kJ$ and $2 kJ$ escaped to the surroundings as heat. The change in internal energy, $\Delta U(in kJ)$ is:

The minimum amount of ${O}_{2}(g)$ consumed per gram of reactant is for the reaction: (Given atomic mass: $Fe=56, O=16, Mg=24, P=31, C=12,H=1$ )