Question Bank Directory

The correct value of cell potential in volts for the reaction that occurs when the following two half cells are connected, is: $Fe^{2+}(aq) + 2e^- \rightarrow Fe(s) \ ; \ E^{\circ} = -0.44\text{ V}$ $Cr_2O_7^{2-}(aq) + 14H^+ + 6e^- \rightarrow 2Cr^{3+} + 7H_2O \ ; \ E^{\circ} = +1.33\text{ V}$

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

Which of the following can be used as the halide component for Friedel-Crafts reaction?

A 20 litre container at 400 K contains $CO_2(g)$ at pressure 0.4 atm and an excess of SrO (neglect the volume of solid SrO). The volume of the container is now decreased by moving the movable piston fitted in the container. The maximum volume of the container, when the pressure of $CO_2$ attains its maximum value, will be (Given that: $SrCO_3(s) \rightleftharpoons SrO(s) + CO_2(g)$, ($K_p = 1.6\text{ atm}$))

The specific palindromic sequence which is recognized by EcoRI is

If the equilibrium constant for $N_2(g) + O_2(g) \rightleftharpoons 2NO(g)$ is $K$, the equilibrium constant for $\frac{1}{2}N_2(g) + \frac{1}{2}O_2(g) \rightleftharpoons NO(g)$ will be?

The ionization constant of ammonium hydroxide is $1.77 \times 10^{-5}$ at $298 \text{ K}$. Hydrolysis constant of ammonium chloride is:

MY and $NY_3$, two nearly insoluble salts, have the same $K_{sp}$ values of $6.2 \times 10^{-13}$ at room temperature. Which statement would be true in regard to MY and $NY_3$?

The solubility product of $\text{BaSO}_4$ in water is $1.5 \times 10^{-9}$. The molar solubility of $\text{BaSO}_4$ in $0.1\text{ M}$ solution of $\text{Ba(NO}_3\text{)}_2$ is:

Predict the order of reactivity of the following four isomers towards $\text{S}_\text{N}2$ reaction. (I) $\text{CH}_3\text{CH}_2\text{CH}_2\text{CH}_2\text{Cl}$ (II) $\text{CH}_3\text{CH}_2\text{CH}(\text{Cl})\text{CH}_3$ (III) $(\text{CH}_3)_2\text{CHCH}_2\text{Cl}$ (IV) $(\text{CH}_3)_3\text{CCl}$

The conductivity of centimolar solution of KCl at $25^{\circ}\text{C}$ is $0.0210\text{ ohm}^{–1}\text{ cm}^{–1}$ and the resistance of the cell containing the solution at $25^{\circ}\text{C}$ is $60\text{ ohm}$. The value of the cell constant is:

Given the following two reactions: $A + B \rightleftharpoons C + D$, with equilibrium constant $K_1$ $E + F \rightleftharpoons G + H$, with equilibrium constant $K_2$ What is the equilibrium constant for the reaction $C + D + E + F \rightleftharpoons A + B + G + H$?

For the equilibrium $2\text{NOCl}(g) \rightleftharpoons 2\text{NO}(g) + \text{Cl}_2(g)$ the value of the equilibrium constant is $3.0 \times 10^{-6}$ at $1000\text{ K}$. Find $K_p$ for the reaction at this temperature (Given $R = 8.314\text{ J K}^{-1}\text{mol}^{-1}$):

The hydrogen ion concentration of a $10^{-8}\text{ M}$ HCl aqueous solution at 298 K ($K_w = 10^{-14}$) is:

A buffer solution is prepared in which the concentration of $NH_3$ is 0.30 M and the concentration of $NH_4^+$ is 0.20 M. If the equilibrium constant, $K_b$ for $NH_3$ equals $1.8 \times 10^{-5}$, then what is the pH of this solution? ($\log 1.8 = 0.25$; $\log 0.67 = -0.176$)

A satellite is orbiting just above the surface of the earth with period $T$. If $d$ is the density of the earth and $G$ is the universal constant of gravitation, the quantity $\frac{3\pi}{Gd}$ represents

The solubility of $BaSO_4$ in water is $2.42 \times 10^{-3} \text{ g L}^{-1}$ at $298 \text{ K}$. The value of the solubility product will be: (Molar mass of $BaSO_4 = 233 \text{ g mol}^{-1}$)

HCl with an alkene X reacts in accordance with Markovnikov’s rule to give 1-Chloro-1-methylcyclohexane. The structure of alkene (X) is:

Under isothermal condition, a gas at 300 K expands from 0.1 L to 0.25 L against a constant external pressure of 2 bar. The work done by the gas is (Given that 1 L bar = 100 J)

For a given exothermic reaction, $K_p$ and $K_p'$ are the equilibrium constants at temperatures $T_1$ and $T_2$ respectively. Assuming that the heat of reaction is constant in the temperature range between $T_1$ and $T_2$, it is readily observed that: (Assume $T_2 > T_1$)