Physical Chemistry PYQ — Page 16

Which one of the following molecular hydrides acts as a Lewis acid ?

An increase in equivalent conductance of a strong electrolyte with dilution is mainly due to

Three moles of an ideal gas expanded spontaneously into vacuum. The work done will be

If $\mathrm{pH}$ of a saturated solution of $\mathrm{Ba}(\mathrm{OH})_2$ is 12 , the value of its $K_{s p}$ is

Standard entropies of $\mathrm{X}_2, \mathrm{Y}_2$ and $\mathrm{XY}_3$ are 60,40 and $50 \mathrm{~J} \mathrm{~K} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}$ respectively. For the reaction $\frac{1}{2} \mathrm{X}_2+\frac{3}{2} \mathrm{Y}_2 \rightleftharpoons \mathrm{XY}_3 ; \Delta \mathrm{H}=-30 \mathrm{~kJ}$, to be at equilibrium, the temperature should be

The correct order of the decreasing ionic radii among the following isoelectronic species is

$25.3 \mathrm{~g}$ of sodium carbonate, $\mathrm{Na}_2 \mathrm{CO}_3$ is dissolved in enough water to make $250 \mathrm{~mL}$ of solution. If sodium carbonate dissociates completely, molar concentration of sodium ion, $\mathrm{Na}^{+}$and carbonate ion, $\mathrm{CO}_3^{2-}$ are respectively (Molar mass of $\mathrm{Na}_2 \mathrm{CO}_3=106 \mathrm{~g} \mathrm{~mol}^{-1}$ )

In a buffer solution containing equal concentration of $\mathrm{B}^{-}$and $\mathrm{HB}$, the $\mathrm{K}_{\mathrm{b}}$ for $\mathrm{B}^{-}$is $10^{-10}$. The $\mathrm{pH}$ of buffer solution is

Match List I (equations) with List II (types of process) and select the correct OPTION.  

Which one of the following ions has electronic configuration $[\mathrm{Ar}] 3 \mathrm{~d}^6$ ? (At. no: $\mathrm{Mn}=25, \mathrm{Fe}=26, \mathrm{Co}=27, \mathrm{Ni}=28$ )

The reaction, \(2 \mathrm{~A}_{(\mathrm{g})}+\mathrm{B}_{(\mathrm{g})} \leftrightharpoons 3 \mathrm{C}_{(\mathrm{g})}+\mathrm{D}_{(\mathrm{g})}\) is begun with the concentrations of \(A\) and \(B\) both at an initial value of 1.00 M When equilibrium is reached, the concentration of \(D\) is measured and found to be 0.25 M. The value for the equilibrium constant for this reaction is given by the expression

The number of atoms in 0.1 mole of a triatomic gas is $\left(\mathrm{N}_{\mathrm{A}}=6.02 \times 10^{23} \mathrm{~mol}^{-1}\right)$

What is $\left[\mathrm{H}^{+}\right]$in $\mathrm{mol} / \mathrm{L}$ of a solution that is $0.20 \mathrm{M}$ in $\mathrm{CH}_3 \mathrm{COONa}$ and $0.10 \mathrm{M}$ in $\mathrm{CH}_3 \mathrm{COOH}$ ? $\left(\mathrm{K}_{\mathrm{a}}\right.$ for $\mathrm{CH}_3 \mathrm{COOH}=1.8 \times 10^{-5}$ )

In which of the following equilibrium $\mathrm{K}_C$ and $\mathrm{K}_{\mathrm{P}}$ are not equal ?

For the reaction \(\mathrm{N}_2 \mathrm{O}_5(\mathrm{g}) \rightarrow 2 \mathrm{NO}_2(\mathrm{g})+(1 / 2) \mathrm{O}_2(\mathrm{g})\) the value of rate of disappearance of \(\mathrm{N}_2 \mathrm{O}_5\) is given as \(6.25 \times 10^{-3} \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~s}^{-1}\). The rate of formation of \(\mathrm{NO}_2\) and \(\mathrm{O}_2\) is given respectively as

A $0.66 \mathrm{~kg}$ ball is moving with a speed of $100 \mathrm{~m} / \mathrm{s}$. The associated wavelength will be (h $\left.=6.6 \times 10^{-34} \mathrm{Js}\right)$

In producing chlorine by electrolysis $100 \mathrm{~kW}$ power at $125 \mathrm{~V}$ is being consumed. How much chlorine per minute is liberated (ECE of chlorine is $0.367 \times 10^{-6} \mathrm{kgC}^{-1}$ )

For the reduction of silver ions with copper metal, the standard cell potential was found to be $+0.46 \mathrm{~V}$ at $25^{\circ} \mathrm{C}$. The value of standard Gibbs energy, $\Delta \mathrm{G}^{\circ}$ will be $\left(\mathrm{F}=96500 \mathrm{C} \mathrm{mol}^{-1}\right)$

An aqueous solution is 1.00 molal in KI. Which change will cause the vapour pressure of the solution to increase ?

For an endothermic reaction, energy of activation is $E_a$ and enthalpy of reaction is $\Delta H$ (both of these in $\mathrm{kJ} / \mathrm{mol}$ ). Minimum value of $E_a$ will be

Consider the following relations for emf of a electrochemical cell (A) Emf of cell = (oxidation potential of anode) - (reduction potential of cathode) (B) Emf of cell = (oxidation potential of anode) + (reduction potential of cathode) (C) Emf of cell = (reduction potential of anode) + (reduction potential of cathode) (D) Emf of cell = (oxidation potential of anode)-(Oxidation potential of cathode) Which of the above relations are correct?

During the kinetic study of the reaction, $2 \mathrm{~A}+\mathrm{B} \rightarrow \mathrm{C}+\mathrm{D}$, following results were obtained \(\begin{array}{|c|c|c|c|} \hline \text { Run } & [A] / \mathrm{mol~} \mathrm{L}^{-1} & [B] / \mathrm{mol~} \mathrm{L}^{-1} & \begin{array}{cc} \text{Initial rate of} \\ \text{formation of} \\ D / \mathrm{mol~} \mathrm{L}^{-1} \mathrm{~min}^{-1} \end{array} \\ \hline \text { I } & 0.1 & 0.1 & 6.0 \times 10^{-3} \\ \hline \text { II } & 0.3 & 0.2 & 7.2 \times 10^{-2} \\ \hline \text { III } & 0.3 & 0.4 & 2.88 \times 10^{-1} \\ \hline \text { IV } & 0.4 & 0.1 & 2.40 \times 10^{-2} \\ \hline \end{array}\) Based on the above data which one of the following is correct?

Which of the following expressions correctly represents the equivalent conductance at infinite dilution of $\mathrm{Al}_2\left(\mathrm{SO}_4\right)_3$. Given that $\Lambda_{\mathrm{Al}^{3+}}^{\circ}$ and $\Lambda_{\mathrm{SO}_4^{2-}}^{\circ}$ are the equivalent conductances at infinite dilution of the respective ions?

What is the $\left[\mathrm{OH}^{-}\right]$in the final solution prepared by mixing $20.0 \mathrm{~mL}$ of $0.050 \mathrm{M} \mathrm{HCl}$ with $30.0 \mathrm{~mL}$ of $0.10 \mathrm{M} \mathrm{Ba}(\mathrm{OH})_2$ ?