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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? ($\log 1.8 = 0.25$; $\log 0.67 = -0.176$)

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 $T_2 > T_1$)

Which of the following is an amphoteric hydroxide?

Which one of the following orders correctly represents the increasing acid strengths of the given acids?

In the following reaction, What will be the major product?

$\text{CCl}_2\text{F}_2$ is one of the most common haloalkanes used in industries. The reaction through which it is manufactured from tetrachloromethane is called:

The equilibrium concentration of the species in the reaction $\text{A} + \text{B} \rightleftharpoons \text{C} + \text{D}$ are $2$, $3$, $10$ and $6\text{ mol L}^{-1}$, respectively at $300\text{ K}$. $\Delta G^\circ$ for the reaction is: ($R = 2\text{ cal/mol K}$)

$K_p$ for the following reaction is $3.0$ at $1000\text{ K}$. $\text{CO}_2(g) + \text{C}(s) \rightleftharpoons 2\text{CO}(g)$ The value of $K_c$ for the reaction at the same temperature is: (Given: $R = 0.083\text{ L bar K}^{-1} \text{mol}^{-1}$)

The dissociation constants for acetic acid and HCN at $25^\circ \text{C}$ are $1.5 \times 10^{-5}$ and $4.5 \times 10^{-10}$, respectively. The equilibrium constant for the equilibrium, $CN^- + CH_3COOH \rightleftharpoons HCN + CH_3COO^-$ would be:

Which of the following is the most preferred method for preparing pure alkyl chlorides from alcohols?

Identify the statement that is incorrect regarding chirality:

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

$\text{C}_6\text{H}_5\text{CH}_2\text{Br} \xrightarrow[2.\text{ H}_3\text{O}^+]{1.\text{ Mg, Ether}} \text{X}$ The product 'X' in the above reaction is: