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Zinc can be coated on iron to produce galvanised iron but the reverse is not possible. It is because

The pressure of $\text{H}_2$ required to make the potential of $\text{H}_2$-electrode zero in pure water at $298 \text{ K}$ is

The molar conductance of $\text{NaCl}$, $\text{HCl}$, and $\text{CH}_3\text{COONa}$ at infinite dilution are $126.45$, $426.16$, and $91.0\text{ S cm}^2\text{ mol}^{-1}$ respectively. The molar conductance of $\text{CH}_3\text{COOH}$ at infinite dilution will be:

Conjugate acid of $\text{NH}_2^-$ is:

A reaction among the following can generate isonitriles as a major product. (A) $\text{R-X} + \text{HCN} \rightarrow$ (B) $\text{R-X} + \text{AgCN} \rightarrow$ (C) $\text{R-X} + \text{KCN} \rightarrow$ (D) $\text{R-X} + \text{NaCN} \xrightarrow{\text{C}_2\text{H}_5\text{OH}/\text{H}_2\text{O}}$ Choose the most appropriate answer from the options given below:

For the reaction, $CH_4(g) + 2O_2(g) \rightleftharpoons CO_2(g) + 2H_2O(l)$, $\Delta_r H = -170 \text{ kJ mol}^{-1}$. Which of the following statements is not true?

Given the following cell reaction: $2\text{Fe}^{3+}\text{(aq)} + 2\text{I}^-\text{(aq)} \rightarrow 2\text{Fe}^{2+}\text{(aq)} + \text{I}_2\text{(aq)}$ $E^\circ_{\text{cell}} = 0.24 \text{ V}$ at $298 \text{ K}$. The standard Gibbs energy $\Delta_r G^\circ$ of the cell reaction is: [Given: $F = 96500 \text{ C mol}^{-1}$]

Limiting molar conductivities, for the given solutions, are: $\lambda^0_m(\text{H}_2\text{SO}_4) = x \text{ S cm}^2 \text{ mol}^{-1}$ $\lambda^0_m(\text{K}_2\text{SO}_4) = y \text{ S cm}^2 \text{ mol}^{-1}$ $\lambda^0_m(\text{CH}_3\text{COOK}) = z \text{ S cm}^2 \text{ mol}^{-1}$ From the data given above, it can be concluded that $\lambda^0_m$ in $(\text{S cm}^2 \text{ mol}^{-1})$ for $\text{CH}_3\text{COOH}$ will be:

For the disproportionation of copper: $2Cu^+ \rightarrow Cu^{2+} + Cu$, $E^{\circ}$ is: (Given $E^{\circ}$ for $Cu^{2+}/Cu$ is $0.34\text{ V}$ and $E^{\circ}$ for $Cu^{2+}/Cu^+$ is $0.15\text{ V}$)

The molar conductance of an electrolyte increases with dilution according to the equation: $\Lambda_m = \Lambda^{\circ}_m - A\sqrt{c}$ Consider the following four statements: A: This equation applies to both strong and weak electrolytes. B: The value of the constant $A$ depends upon the nature of the solvent. C: The value of constant $A$ is the same for both $\text{BaCl}_2$ and $\text{MgSO}_4$. D: The value of constant $A$ is the same for both $\text{BaCl}_2$ and $\text{Mg(OH)}_2$. Which of the above statements are correct?

Polyblend, a fine powder of recycled modified plastic, has proved to be a good material for

For a cell reaction involving a two-electron change, the standard Emf of the cell is found to be $0.295\text{ V}$ at $25^{\circ}\text{C}$. The equilibrium constant of the reaction at $25^{\circ}\text{C}$ will be:

Standard electrode potential of three metals X, Y and Z are $-1.2 \text{ V}$, $+0.5 \text{ V}$ and $-3.0 \text{ V}$ respectively. The reducing power of these metals will be:

Which of the following cannot act both as a Bronsted acid and as a Bronsted base?

The EMF of a Daniel cell at $298\text{ K}$ is $E_1$: $Zn|ZnSO_4(0.01\text{ M}) || CuSO_4(1.0\text{ M})|Cu$. When the concentration of $ZnSO_4$ is $1.0\text{ M}$ and that of $CuSO_4$ is $0.01\text{ M}$, the EMF is changed to $E_2$. The correct relationship between $E_1$ and $E_2$ is:

Limiting molar conductivity of $\text{NH}_4\text{OH}$ (i.e., $\Lambda^\circ_m(\text{NH}_4\text{OH})$) is equal to:

The correct relation between dissociation constants of a di-basic acid is:

Limiting molar conductivity of $\text{NH}_4\text{OH}$ (i.e. $\Lambda^\circ_m(\text{NH}_4\text{OH})$) is equal to:

Given below are half-cell reactions: $MnO_4^- + 8H^+ + 5e^- \rightarrow Mn^{2+} + 4H_2O \ ; \ E^\circ_{Mn^{2+}/MnO_4^-} = -1.510\text{ V}$ $\frac{1}{2}O_2 + 2H^+ + 2e^- \rightarrow H_2O \ ; \ E^\circ_{O_2/H_2O} = +1.223\text{ V}$ Will the permanganate ion, $MnO_4^-$, liberate $O_2$ from water in the presence of an acid?

A hypothetical electrochemical cell is shown below: $\text{A} | \text{A}^+(x\text{ M}) || \text{B}^+(y\text{ M}) | \text{B}$ The EMF measured is $+0.20 \text{ V}$. The cell reaction is: