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Chapter 21: Q21.105P (page 976)

How many seconds does it take to deposit 65.5g ofZn on a steel gate when21.0A is passed through a ZnSO4solution?

Short Answer

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Step 1: Definition

Step by step solution

01

Calculating the time

A current of 21.0A(A=C/s)is passed through a ZnSO4solution.

We need to find the time (in seconds) it takes to deposit 65.5gof Zn.

ZnSO4鈫�Zn2++SO42-

The half-reaction for Zn2+reduction is

Zn2++2e-鈫�Zn

- Here we can see that for every mole of Zndeposited, we need 2moles of electrons.

The number of moles of Zndeposited is (the molar mass of Znis 65.38g/mol)

MolesZndeposited=65.5g65.38=1.002molZn

Hence, the number of moles of electrons is

Molese-=1.002molZn脳2mole-1molZn=2.004mole-

02

Calculating deposit time

- Faraday constant: charge of a mole of electrons F=96485C/mol-

Now, we will calculate the charge, using the Faraday constant

Charge = Moles e-脳F

=2.004mol-脳96485Cmol-=193355.94C

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Most popular questions from this chapter

When zinc is refined by electrolysis, the desired half reaction at the cathode is:

Zn2 +(aq) + 2e-鈫�Zn(s)

A competing reaction, which lowers the yield, is the formation of hydrogen gas:

2H+(aq) + 2e-鈫�H2(g)

If 91.50%of the current flowing results in zinc being deposited, while8.50% produces hydrogen gas, how many litres ofH2 , measured at STP, form per kilogram of zinc?

Water is used to balance O atoms in the half-reaction method. Why can鈥檛O2-ions be used instead?

Which statements are true? Correct any that are false.

(a) In a voltaic cell, the anode is negative relative to the cathode.

(b) Oxidation occurs at the anode of a voltaic or electrolytic cell.

(c) Electrons flow into the cathode of an electrolytic cell.

(d) In a voltaic cell, the surroundings do work on the system.

(e) A metal that plates out of an electrolytic cell appears on the cathode.

(f) The cell electrolyte provides a solution of mobile electrons.

Bubbles of H2 form when metal D is placed in hot . No reaction occurs when D is placed in a solution of a salt of metal E, but D is discoloured and coated immediately when placed in a solution of a salt of metal F. What happens if E is placed in a solution of a salt of metal ? Rank metals, E, and F in order of increasing reducing strength.

Why are E half-cell values for the oxidation and reduction of water different from E掳 half-cell values for the same processes? In an aqueous electrolytic cell, nitrate ions never react at the anode, but nitrite ions do. Explain.
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