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Chapter 7: Problem 24

In a Daniel cell, if \(A\left(E_{0}=-0.76 v\right)\) and \(B(=-2.36 v)\) half- cells are taken then (a) \(\mathrm{B}\) acts as an anode (b) \(\mathrm{A}\) acts as an anode (c) \(\mathrm{B}\) acts as a cathode (d) cannot be predicted

Short Answer

Expert verified
Answer: (a) B acts as an anode.

Step by step solution

01

Identify the half-cell with the higher and lower reduction potential.

We are given: A: \(E_{0}=-0.76 V\) B: \(E_{0}=-2.36 V\) Comparing these values, \(E_{0}\) of A is higher than that of B: \(-0.76 V > -2.36 V\)
02

Determine the anode and cathode

As the higher reduction potential half-cell acts as the cathode, and the lower reduction potential half-cell acts as the anode, we can conclude that: A acts as the cathode (because it has a higher reduction potential). B acts as the anode (because it has a lower reduction potential).
03

Choose the appropriate answer option

Based on the conclusions in Step 2, we can now determine the correct answer option: (a) B acts as an anode, which matches our conclusion that B is the anode. Therefore, the correct answer is option (a).

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Most popular questions from this chapter

The amounts of metals deposited when \(965 \mathrm{C}\) of electricity is passed through \(\mathrm{NaCl}\) and \(\mathrm{AgNO}_{3}\) solutions are ___ and ___ respectively. (a) \(23 \mathrm{~g}, 108 \mathrm{~g}\) (b) \(11.5 \mathrm{~g}, 54 \mathrm{~g}\) (c) \(0.23 \mathrm{~g}, 1.08 \mathrm{~g}\) (d) \(2.3 \mathrm{~g}, 10.8 \mathrm{~g}\)

Identify the set of metals which require same amount of charge for the deposition of one mole of metals: (a) \(\mathrm{Na}, \mathrm{Ag}, \mathrm{Al}\) (b) \(\mathrm{Zn}, \mathrm{Cu}, \mathrm{Ag}\) (c) \(\mathrm{Al}, \mathrm{Cu}, \mathrm{Zn}\) (d) \(\mathrm{Mg}, \mathrm{Zn}, \mathrm{Cd}\)

State whether the following statements are true or false. The salt bridge permits movement of charge and mixing of the solution.

Assertion (A): Passage of 48,250 coulombs of electricity through cupric sulphate and ferrous sulphate solutions result in the deposition \(0.5\) moles each of iron and copper at the respective cathodes. Reason (R): Number of equivalents of a metal deposited at cathode is equal to the number of faradays of electricity passed through the electrolyte. (a) Both "A" and "R" are true and "R" is the correct explanation of "A". (b) Both "A" and "R" are true and "R" is not the correct explanation of "A". (c) "A" is correct and "R" is wrong. (d) "A" is wrong and "R" is correct.

Pairs of electrodes and their corresponding standard electrode potentials are given. Arrange the cells constructed by these electrodes in increasing order of emf values. (1) Electrode \(\rightarrow \mathrm{A}, \mathrm{E}^{\circ}=-2.92 \mathrm{~V}\) and Electrode \(\rightarrow\) \(\mathrm{B}, \mathrm{E}^{\circ}=-2.71 \mathrm{~V}\) (2) Electrode \(\rightarrow \mathrm{C}, \mathrm{E}^{\circ}=-0.760 \mathrm{~V}\) and Electrode \(\rightarrow\) \(\mathrm{D}, \mathrm{E}^{\circ}=-0.44 \mathrm{~V}\) (3) Electrode \(\rightarrow \mathrm{B}, \mathrm{E}^{\circ}=-2.71 \mathrm{~V}\) and Electrode \(\rightarrow\) \(\mathrm{D}, \mathrm{E}^{\circ}=-0.44 \mathrm{~V}\) (4) Electrode \(\rightarrow \mathrm{A}, \mathrm{E}^{\circ}=-2.92 \mathrm{~V}\) and Electrode \(\rightarrow\) \(\mathrm{C}, \mathrm{E}^{\circ}=-0.76 \mathrm{~V}\) (a) 2143 (b) 1243 (c) 2413 (d) 2431
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