JEE Main 2018 — Physical Chemistry

An alkali is titrated against acid with methyl orange as an indicator, which of the following is a correct combination?

An aqueous solution contains an unknown concentration of ${\mathrm{Ba}}^{2+}$. When $50\mathrm{mL}\mathrm{of}a1M$ solution of ${\mathrm{Na}}_{2}{\mathrm{SO}}_{4}$ is added, ${\mathrm{BaSO}}_{4}$ just begins to precipitate. The final volume is $500\mathrm{mL}$. The solubility product of ${\mathrm{BaSO}}_{4}$ is $1\times {10}^{-10}$. What is the original concentration of ${\mathrm{Ba}}^{2+}$?

An aqueous solution contains $0.10M {H}_{2}S$ and $0.20M\mathrm{HCl}$. If the equilibrium constant for the formation of ${\mathrm{HS}}^{-}$ from ${H}_{2}S$ is $1.0\times {10}^{-7}$ and that of ${S}^{2-}$ from ${\mathrm{HS}}^{-}$ ions is $1.2\times {10}^{-13}$, then, the concentration of ${S}^{2-}$ ions in the aqueous solution is:

An ideal gas undergoes a cyclic process as shown in the figure  $\Delta {U}_{\mathrm{BC}}=-5{\mathrm{KJmol}}^{-1},{q}_{\mathrm{AB}}=2{\mathrm{KJmol}}^{-1}$ ${W}_{\mathrm{AB}}=-5{\mathrm{KJmol}}^{-1},{W}_{\mathrm{CA}}=3{\mathrm{KJmol}}^{-1}$ Heat absorbed by the system during process $\mathrm{CA}$is

An ideal gas undergoes a cyclic process as shown in Figure.  $\begin{aligned} &\Delta \mathrm{U}_{\mathrm{BC}}=-5 \mathrm{~kJ} \mathrm{~mol}^{-1}, \mathrm{q}_{\mathrm{AB}}=2 \mathrm{~kJ} \mathrm{~mol}^{-1} \\ &\mathrm{~W}_{\mathrm{AB}}=-5 \mathrm{~kJ} \mathrm{~mol}^{-1}, \mathrm{~W}_{\mathrm{CA}}=3 \mathrm{~kJ} \mathrm{~mol}^{-1} \end{aligned}$ Heat absorbed by the system during process CA is:

An unknown chlorohydrocarbon has 3.55 % of chlorine. If each molecule of the hydrocarbon has one chlorine atom only; chlorine atoms present in 1 g of chlorohydrocarbon are :(Atomic wt. of $\mathrm{Cl}=35.5 u;$ Avogadro constant $=6.023\times {10}^{23} {\mathrm{mol}}^{–1}$)

At 320 K, a gas ${A}_{2}$ is 20 % dissociated to $A(g)$ . The standard Gibbs free energy change at $320 K and 1 atm in J mo{l}^{–1}$ is approximately: $(R = 8.314 {\mathrm{JK}}^{–1} {\mathrm{mol}}^{–1} ;\mathrm{ln}2 = 0.693 ;\mathrm{ln}3 = 1.098)$

At a certain temperature in a 5L vessel, 2 moles of carbon monoxide and 3 moles of chlorine were allowed to reach equilibrium according to the reaction, $\mathrm{CO}+\mathrm{Cl}_2 \rightleftharpoons \mathrm{COCl}_2$. At equilibrium, if one mole of $\mathrm{CO}$ is present then equilibrium constant $\left(K_{\mathrm{c}}\right)$ for the reaction is:

$\Delta_{\mathrm{f}} \mathrm{G}^{\circ}$ at $500 \mathrm{~K}$ for substance ' $\mathrm{S}$ ' in liquid state and gaseous state are $+100.7 \mathrm{kcal} \mathrm{mol}^{-1}$ and $+103$ $\mathrm{kcal} \mathrm{mol}^{-1}$, respectively. Vapour pressure of liquid ' $\mathrm{S}$ ' at $500 \mathrm{~K}$ is approximately equal to: $$ \left(\mathrm{R}=2 \mathrm{cal} \mathrm{K}^{-1} \mathrm{~mol}^{-1}\right) \text {. } $$

At ${518}^{o}C,$ the rate of decomposition of a sample of gaseous acetaldehyde, initially at a pressure of $363 \mathrm{Torr}$ was $1.00 \mathrm{Torr} {s}^{-1}$ when $5%$ had reacted and $0.50 \mathrm{Torr} {s}^{-1}$ when 33% had reacted. The order of the reaction is:

$\mathrm{N}_2 \mathrm{O}_5$ decomposes to $\mathrm{NO}_2$ and $\mathrm{O}_2$ and follows first order kinetics. After $50$ minutes, the pressure inside the vessel increases from $50 \mathrm{~mm} \mathrm{~Hg}$ to $87.5 \mathrm{~mm} \mathrm{~Hg}$. The pressure of the gaseous mixture after $100$ minutes at constant temperature will be ______.

${N}_{2}{O}_{5}$ decomposes to ${\mathrm{NO}}_{2}$ and ${O}_{2}$ follows the first order kinetics. After $50$ minutes, the pressure inside the vessel increases from $50\mathrm{mm}\mathrm{Hg}$ to $87.5\mathrm{mm}\mathrm{Hg}$. The pressure of the gaseous mixture after $100$ minutes at constant temperature will be:

Ejection of the photoelectron from metal in the photoelectric effect experiment can be stopped by applying $0.5 \mathrm{~V}$ when the radiation of $250 \mathrm{~nm}$ is used. The work function of the metal is :

Ejection of the photoelectron from metal in the photoelectric effect experiment can be stopped by applying $0.5V$, when the radiation of $250\mathrm{nm}$ is used. The work function of the metal is

Following four solutions are prepared by mixing different volumes of $\mathrm{NaOH}$ and $\mathrm{HCl}$ of different concentrations, $\mathrm{pH}$ of which one of them will be equal to 1 ?

For a first order reaction, $\mathrm{A} \rightarrow \mathrm{P}, \mathrm{t}_{1 / 2}$ (half-life) is 10 days. The time required for $\frac{1}{4}^{\text {th }}$ conversion of $\mathrm{A}$ (in days) is: $(\ln 2=0.693, \ln 3=1.1)$.

For per gram of reactant, the maximum quantity of $\mathrm{N}_2$ gas is produced in which of the following thermal decomposition reactions? (Given: Atomic wt. : $\mathrm{Cr}=52 \mathrm{u}, \mathrm{Ba}=137 \mathrm{u}$ ).

For standardizing $\mathrm{NaOH}$ solution, which of the following is used as a primary standard?

For which of the following processes, $\Delta S$ is negative?

For which of the following reactions, $\Delta \mathrm{H}$ is equal to $\Delta \mathrm{U}$ ?

For which of the following reactions, $\Delta H$ is equal to $\Delta U$?

For$1\mathrm{molal}$aqueous solution of the following compounds, which one will show the highest freezing point?

Given (i) $2 \mathrm{Fe}_2 \mathrm{O}_3(\mathrm{~s}) \rightarrow 4 \mathrm{Fe}(\mathrm{s})+3 \mathrm{O}_2(\mathrm{~g})$; $$ \Delta_{\mathrm{r}} \mathrm{G}^{\circ}=+1487.0 \mathrm{~kJ} \mathrm{~mol}^{-1} $$ (ii) $2 \mathrm{CO}(\mathrm{g})+\mathrm{O}_2(\mathrm{~g}) \rightarrow 2 \mathrm{CO}_2(\mathrm{~g})$; $$ \Delta_{\mathrm{r}} \mathrm{G}^{\circ}=-514.4 \mathrm{~kJ} \mathrm{~mol}^{-1} $$ Free energy change, $\Delta_{\mathrm{r}} \mathrm{G}^{\circ}$ for the reaction $2 \mathrm{Fe}_2 \mathrm{O}_3(\mathrm{~s})+6 \mathrm{CO}(\mathrm{g}) \rightarrow 4 \mathrm{Fe}(\mathrm{s})+6 \mathrm{CO}_2(\mathrm{~g})$ will be:

How long (approximate) should water be electrolysed by passing through $100$$\mathrm{amperes}$current so that the oxygen released can completely burn $27.66g$ of diborane? (Atomic weight of $B=10.8u$)

If 50 % of a reaction occurs in 100 second and 75 % of the reaction occurs in 200 second, the order of this reaction is:

In which of the following reactions, an increase in the volume of the container will favour the formation of products?

In which of the following reactions, an increase in the volume of the container will favour the formation of products?

The combustion of benzene $(l)$ gives ${\mathrm{CO}}_{2}(g)$ and ${H}_{2}O(l).$ Given that heat of combustion of benzene at constant volume is $-3263.9 \mathrm{kJ} {\mathrm{mol}}^{-1}$ at $25^{\circ}C;$ the heat of combustion $(\mathrm{in} \mathrm{kJ} {\mathrm{mol}}^{-1})$ of benzene at constant pressure will be $(R=8.314 {\mathrm{JK}}^{-1} {\mathrm{mol}}^{-1})$

The de-Broglie's wavelength of electron present in first Bohr orbit of ' $\mathrm{H}$ ' atom is:

The gas phase reaction $2{\mathrm{NO}}_{2}(g) \rightarrow {N}_{2}{O}_{4} (g)$ is an exothermic reaction. The decomposition of ${N}_{2}{O}_{4}$ , in equilibrium mixture of ${\mathrm{NO}}_{2} (g) \mathrm{and} {N}_{2}{O}_{4} (g)$ can be increased by:

The mass of a non-volatile, non-electrolyte solute (molar mass $= 50 g {\mathrm{mol}}^{-1}$) needed to be dissolved in 114 g octane to reduce its vapour pressure by 75 %, is:

The minimum volume of water required to dissolve 0.1 g lead (II) chloride to get a saturated solution ( ${K}_{sp}$ of ${PbCl}_{2}=3.2\times {10}^{-8}$ ;atomic mass of $Pb=207 u$ ) is:

The minimum volume of water required to dissolve $0.1 \mathrm{~g}$ lead (II) chloride to get a saturated solution $\left(K_{\mathrm{SP}}\right.$ of $\mathrm{PbCl}_2=3.2 \times 10^{-8}$; atomic mass of $\mathrm{Pb}=207 \mathrm{~u})$ is :

The ratio of mass percent of $C\mathrm{and}H$ of an organic compound $({C}_{X}{H}_{Y}{O}_{Z})$ is $6:1.$ If one molecule of the above compound $({C}_{X}{H}_{Y}{O}_{Z})$ contains half as much oxygen as required to burn one molecule of compound ${C}_{X}{H}_{Y}$ completely to ${\mathrm{CO}}_{2}$ and ${H}_{2}O.$ The empirical formula of the compound ${C}_{X}{H}_{Y}{O}_{Z}$ is

Two 5 molal solutions are prepared by dissolving a non-electrolyte, non-volatile solute separately in the solvents $\mathrm{X}$ and $\mathrm{Y}$. The molecular weights of the solvents are $\mathrm{M}_{\mathrm{X}}$ and $\mathrm{M}_{\mathrm{Y}}$, respectively where $\mathrm{M}_X=\frac{3}{4} \mathrm{M}_{\mathrm{Y}}$. The relative lowering of vapour pressure of the solution in $\mathrm{X}$ is " $\mathrm{m}$ " times that of the solution in Y. Given that the number of moles of solute is very small in comparison to that of solvent, the value of "m" is:

When 9.65 ampere current was passed for 1.0 hour into nitrobenzene in acidic medium, the amount of p-aminophenol produced is:

When an electric current is passed through acidified water, 112 mL of hydrogen gas at N.T.P was collected at the cathode in 965 seconds. The current passed, in ampere, is:

When an electric current is passes through acidified water, $112 \mathrm{~mL}$ of hydrogen gas at N.T.P. was collected at the cathode in $965$ seconds. The current passed, in ampere, is :

Which of the following are Lewis acids?

Which of the following is a Lewis acid?

Which of the following is a Lewis acid?

Which of the following lines correctly show the temperature dependence of equilibrium constant $K,$ for an exothermic reaction? 

Which of the following salts is the most basic in aqueous solution?

Which of the following statements is false?