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Chapter 7: Problem 26

Equimolar solutions of zinc sulphate and ferric sulphate are subjected to electrolysis. What is the ratio of Faradays of electricity required for deposition of one mole each of zinc and iron? (a) \(1: 2\) (b) \(2: 3\) (c) \(1: 3\) (d) \(3: 2\)

Short Answer

Expert verified
Answer: The ratio of Faradays of electricity required for deposition of one mole each of zinc and iron is 2:3.

Step by step solution

01

Write down the reduction half-reactions for zinc and iron

In order to determine the total charge required for deposition of each metal, we need to write the half-reactions for each metal ion reduction. We have: Zinc reduction: Zn\(^{2+}\) + 2e\(^-\) → Zn (s) Ferric reduction: Fe\(^{3+}\) + 3e\(^- \)→ Fe (s)
02

Calculate the moles of electrons required for deposition of one mole of each metal

In the zinc reduction half-reaction, 2 moles of electrons are required to deposit 1 mole of zinc. In the ferric reduction half-reaction, 3 moles of electrons are required to deposit 1 mole of iron.
03

Determine the ratio of Faradays of electricity required for deposition of one mole each of zinc and iron

According to Faraday's Law, the amount of charge (in Faradays) needed to deposit one mole of a substance is equal to the moles of electrons required for deposition. Since zinc requires 2 moles of electrons and iron requires 3 moles of electrons, the ratio of Faradays of electricity required for deposition of one mole each of zinc and iron is: Ratio = moles of electrons for zinc : moles of electrons for iron = 2 : 3 Thus, the correct answer is (b) \(2: 3\).

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Most popular questions from this chapter

The metal deposited first at the cathode when a solution containing \(\mathrm{Fe}^{+2}, \mathrm{Cu}^{+2}\) is electrolyzed is (a) \(\mathrm{Fe}\) (b) \(\mathrm{Cu}\) (c) \(\mathrm{Fe}^{+3}\) (d) both 1 and 2

Identify the false statement among the following: (a) Oxidation takes place at positive electrode in electrolytic cell, whereas reduction at negative electrode in voltaic cell. (b) Deposition of metals takes place in both electrolytic and galvanic cells. (c) Direction of flow of current is from cathode to anode in electrolytic cell. (d) Both (a) and (b)

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Match the entries given in column \(A\) with the appropriate ones in column B. $$ \begin{array}{ll} \text { Column A } & \text { Column B } \\ \begin{array}{ll} \text { A. Concentrated } \mathrm{HCl} \\ \text { solution } \end{array} & \text { () } \text { a. } \mathrm{Na} \text { and } \mathrm{O}_{2} \\ \text { B. Fused alumina } & () \quad \text { b. } \mathrm{Na} \text { and } \mathrm{Cl}_{2} \\ \text { C. Aqueous sodium } & \text { () } \text { c. } \mathrm{H}_{2} \text { and } \mathrm{Cl}_{2} \\ \text { hydroxide } & \\ \text { D. Molten sodium } & \text { () } \text { d. } \mathrm{H}_{2} \text { and } \mathrm{O}_{2} \\ \text { chloride } & \\ \text { E. Fused } \mathrm{NaOH} & \text { () } \text { e. } \mathrm{Al} \text { and } \mathrm{O}_{2} \end{array} $$

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) \(\mathrm{Mg}, \mathrm{Zn}, \mathrm{Cd}\)
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