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NEET CHEMISTRYMedium

Given below are two statements: Statement I: 2 F2\text{ F} electricity is required for the oxidation of 1 mole H2O1\text{ mole H}_2\text{O} to O2\text{O}_2. Statement II: To get 40.0 g40.0\text{ g} of Aluminium from molten Al2O3\text{Al}_2\text{O}_3 required electricity is 4.44 F4.44\text{ F}. In the light of the above statements, choose the correct answer from the options given below:

A

Both Statement I and Statement II are true

B

Both Statement I and Statement II are false

C

Statement I is true but Statement II is false

D

Statement I is false but Statement II is true

Step-by-Step Solution

Statement I: The oxidation of water is represented by the equation: H2O→12O2+2H++2e−\text{H}_2\text{O} \rightarrow \frac{1}{2}\text{O}_2 + 2\text{H}^+ + 2\text{e}^- For 1 mole1\text{ mole} of H2O\text{H}_2\text{O}, 2 moles2\text{ moles} of electrons are involved. Thus, 2 F2\text{ F} of electricity is required. So, Statement I is true.

Statement II: The reduction of Aluminium from molten Al2O3\text{Al}_2\text{O}_3 is: Al3++3e−→Al\text{Al}^{3+} + 3\text{e}^- \rightarrow \text{Al} 3 F3\text{ F} of electricity is required to produce 1 mole1\text{ mole} (27 g27\text{ g}) of Al\text{Al}. To produce 40.0 g40.0\text{ g} of Al\text{Al}, the required electricity =3 F27 g×40.0 g=4.44 F= \frac{3\text{ F}}{27\text{ g}} \times 40.0\text{ g} = 4.44\text{ F}. So, Statement II is also true.

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