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

Find the emf of the cell in which the following reaction takes place at $298\text{ K}$: $Ni(s) + 2Ag^+(0.001\text{ M}) \rightarrow Ni^{2+}(0.001\text{ M}) + 2Ag(s)$ (Given that $E^{\circ}_{cell} = 1.05\text{ V}; \frac{2.303RT}{F} = 0.059$)

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

Identify the statement that is incorrect regarding chirality:

In the electrochemical cell: $\text{Zn}|\text{ZnSO}_4(0.01 \text{ M}) || \text{CuSO}_4(1.0 \text{ M})|\text{Cu}$, the emf of this Daniel cell is $E_1$. When the concentration of $\text{ZnSO}_4$ is changed to $1.0 \text{ M}$ and that of $\text{CuSO}_4$ is changed to $0.01 \text{ M}$, the emf changes to $E_2$. The relationship between $E_1$ and $E_2$ is : (Given, $\frac{RT}{F} = 0.059$)

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?

In producing chlorine through electrolysis, 100 W power at 125 V is being consumed. The liberation of chlorine per min is: (ECE of chlorine is $0.367 \times 10^{-6} \text{ kg/C}$)

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 $0.15\text{ V}$)

Which of the following molecules acts as a Lewis acid?

Which of the following fluoro-compounds is most likely to behave as a Lewis base?

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?

The fertilizer which makes the soil acidic is:

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

$\Lambda^o_m$ for $\text{NaCl}$, $\text{HCl}$ and $\text{CH}_3\text{COONa}$ are $126.4$, $425.9$, and $91.05\text{ S cm}^2\text{ mol}^{-1}$ respectively. If the conductivity of $0.001028\text{ mol L}^{-1}$ acetic acid solution is $4.95 \times 10^{-5}\text{ S cm}^{-1}$, the degree of dissociation of the acetic acid solution is:

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: