Answered: A tub of water containing Cu²⁺(aq) is…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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A tub of water containing Cu²⁺(aq) is subjected to a current of 0.3 amperes for 30 minutes. How many grams of Cu(s) can be produced.

A) 0.18g

B) 0.354g

C) 1.52g

D) 2.13g

Expert Solution

Introduction:

Faraday's law of electrolysis states that the mass of metal produced or deposited at electrode is directly proportional to the charge. Charge is calculated by multiplying current with time. Molar mass and Faraday's constant have fixed value. The formula for calculating the mass of metal is as follows;

$w = \frac{I \times t \times M}{Z \times F}$

Where;

w = mass of metal in grams

I = current in amperes

t = time in seconds

M = molar mass of metal in g/mol

Z = number of electrons (charge on metal ion)

F = Faraday's constant (96500 C/mol)

Given data:

I = 0.3 A

$\begin{array}{rcl} t & = & 30 minutes \\ = & 30 \times 60 \\ = & 1800 seconds \end{array}$

M = 63.546 g/mol

Z = 2

F = 96500 C/mol

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