JEE Main 2007 — Physical Chemistry

Consider the reaction, $2 \mathrm{A}+\mathrm{B} \rightarrow$ Products When concentration of $\mathrm{B}$ alone was doubled, the half-life did not change. When the concentration of $\mathrm{A}$ alone was doubled, the rate increased by two times. The unit of rate constant for this reaction is

Identify the correct statement regarding a spontaneous process

In a sautrated solution of the sparingly soluble strong electrolyte $\mathrm{AgIO}_3$ (Molecular mass $=283$) the equilibrium which sets in is $\mathrm{AgIO}_{3(\mathrm{s})} \rightleftharpoons \mathrm{Ag}_{(\mathrm{aq})}^{+}+\mathrm{IO}_{3(\mathrm{aq})}^{-}$ If the solubility product constant $\mathrm{K}_{\mathrm{sp}}$ of $\mathrm{AgIO}_3$ at a given temperature is $1.0 \times 10^{-8}$, what is the mass of $\mathrm{AgIO}_3$ contained in $100 \mathrm{~ml}$ of its saturated solution?

In conversion of lime-stone to lime, $\mathrm{CaCO}_3(\mathrm{~s}) \longrightarrow \mathrm{CaO}(\mathrm{s})+\mathrm{CO}_2(\mathrm{~g})$ the vales of $\Delta \mathrm{H}^{\circ}$ and $\Delta \mathrm{S}^{\circ}$ are $+179.1 \mathrm{~kJ} \mathrm{~mol}^{-1}$ and $160.2 \mathrm{~J} / \mathrm{K}$ respectively at $298 \mathrm{~K}$ and $1\mathrm{~bar}$. Assuming that $\Delta \mathrm{H}^{\circ}$ do not change with temperature, temperature above which conversion of limestone to lime will be spontaneous is

Regular use of which of the following fertilizer increases the acidity of soil?

The cell, $\mathrm{Zn}\left|\mathrm{Zn}^{2+}(1 \mathrm{M}) \| \mathrm{Cu}^{2+}(1 \mathrm{M})\right| \mathrm{Cu}\left(\mathrm{E}_{\text {cell }}^0=1.10 \mathrm{~V}\right)$, was allowed to be completely discharged at $\mathrm{298~K}$. The relative concentration of $\mathrm{Zn}^{2+}$ to $\mathrm{Cu}^{2+}\left[\frac{\left[\mathrm{Zn}^{2+}\right]}{\left[\mathrm{Cu}^{2+}\right]}\right]$ is

The density (in $\mathrm{g} \mathrm{~mL}^{-1}$ ) of a $3.60 \mathrm{~M}$ sulphuric acid solution that is $29 \% ~\mathrm{H}_2 \mathrm{SO}_4$ (Molar mass $=98 \mathrm{~g}$ $\mathrm{mol}^{-1}$ ) by mass will be

The energies of activation for forward and reverse reactions for $A_2+B_2 \rightleftharpoons 2 A B$ are $180 \mathrm{~kJ} \mathrm{~mol}^{-1}$ and $200 \mathrm{~kJ} \mathrm{~mol}^{-1}$ respectively. The presence of catalyst lowers the activation energy of both (forward and reverse) reactions by $100 \mathrm{~kJ} \mathrm{~mol}^{-1}$. The enthalpy change of the reaction $\left(\mathrm{A}_2+\mathrm{B}_2 \longrightarrow 2 \mathrm{AB}\right)$ in the presence of catalyst will be (in $\mathrm{kJ} \mathrm{~mol}^{-1}$ )

The equivalent conductances of two strong electrolytes at infinite dilution in $\mathrm{H}_2 \mathrm{O}$ (where ions move freely through a solution) at $25^{\circ} \mathrm{C}$ are given below: $\wedge^{\circ} \mathrm{CH}_3 \mathrm{COONa}=91.0 \mathrm{~S} \mathrm{~cm}^2$ /equiv $\wedge_{\mathrm{HCl}}^{\circ}=426.2 \mathrm{~S} \mathrm{~cm^2}$ / equiv What additional information/quantity one needs to calculate $\wedge^{\circ}$ of an aqueous solution of acetic acid?

The first and second dissociation constants of an acid $\mathrm{H}_2 \mathrm{A}$ are $1.0 \times 10^{-5}$ and $5.0 \times 10^{-10}$ respectively. The overall dissociation constant of the acid will be

The $\mathrm{pKa}$ of a weak acid $(\mathrm{HA})$ is $4.5$. The $\mathrm{pOH}$ of an aqueous buffered solution of $\mathrm{HA}$ in which $50 \%$ of the acid is ionized is

Which of the following sets of quantum numbers represents the highest energy of an atom?