Calculate emf of the half cell given below :
$$ \begin{aligned} & \mathrm{Pt}(\mathrm{~s})\left|\mathrm{H}_2(\mathrm{~g}, 2 \mathrm{~atm})\right| \mathrm{HCl}(\mathrm{aq}, 0.02 \mathrm{M}) \\ & \mathrm{E}_{\mathrm{H}_2 / \mathrm{H}^{+}}^{\circ}=0 \mathrm{~V} \end{aligned} $$
(Given: $\frac{2.303 R T}{F}=0.059, \log 2=0.3010$ )
From the following select the one which is not an example of corrosion.
The standard cell potential of the following cell $$\mathrm{Zn}\left|\mathrm{Zn}^{2+}(\mathrm{aq})\right| \mathrm{Fe}^{2+}(\mathrm{aq}) \mid \mathrm{Fe}$$ is $$0.32 \mathrm{~V}$$. Calculate the standard Gibbs energy change for the reaction:
$$\mathrm{Zn}(\mathrm{s})+\mathrm{Fe}^{2+}(\mathrm{aq}) \rightarrow \mathrm{Zn}^{2+}(\mathrm{aq})+\mathrm{Fe}(\mathrm{s})$$
(Given : $$1 \mathrm{~F}=96487 \mathrm{C}$$)
Match List I with List II.
| List I (Conversion) |
List II (Number of Faraday required) |
||
|---|---|---|---|
| A. | 1 mole of H$$_2$$O to O$$_2$$ | I. | 3F |
| B. | 1 mol of MnO$$_4^-$$ to Mn$$^{2+}$$ | II. | 2F |
| C. | 1.5 mol of Ca from molten CaCl$$_2$$ | III. | 1F |
| D. | 1 mol of FeO to Fe$$_2$$O$$_3$$ | IV. | 5F |
Choose the correct answer from the options given below :
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