EBK GENERAL CHEMISTRY: THE ESSENTIAL CO
EBK GENERAL CHEMISTRY: THE ESSENTIAL CO
7th Edition
ISBN: 8220106637203
Author: Chang
Publisher: YUZU
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Chapter 19, Problem 19.54QP

(a)

Interpretation Introduction

Interpretation:

Need to calculate the amount of copper deposited and current needed to electrolyze the cell containing CuCl2 connected in series with the cell containing AgNO3.

Concept introduction:

In the given case two electrolytic cell containing AgNO3 and CuCl2 were connected in series, so the quantity of electricity flowing through both of the cell will be same

Half-cell reaction for cell-1 was given below.

Cathode (reduction) Ag+(aq)+ e-Ag(s)

The amount of the silver deposited was given, from which the amount of electricity flows though both of the cell can be calculated in steps. Number of moles of silver deposited was calculated first.  Since one mole of electron is needed to reduce one mole of Ag+. Therefore number of moles of electron is equal to number of moles of sliver. The coulombs of electron passing can be calculated by the equation given below.

Numberofmolesofsilver=weight(g)Atomicmass(gmole-1)

Numberofmoles of electrons = Number of moles of SilverthenCharges=Numberofmoles of electrons×Faradayconstant (96500C/mole e-)

Half-cell reaction for cell-2 was given below.

Cathode (reduction) Cu2+(aq)+2e-Cu(s)

Since they are connected in series, same amount of charges will be passing through both the cell. From the calculated charges the number of moles of electrons utilized can be calculated.

Numberofmoles of electrons (n)=Charges×Faradayconstant (96500C/mole e-)

From the cell reaction it was known that two mole of electron will be needed to produce one mole of copper,

So 

numberofmolesofcopper=nmoleofe×1moleCu2moleeWeightofCopper=numberofmolesofcopper × atomic mass

Since time was given the amperes of current flowing through the circuit can be calculated by the equation given below

Current (A) =charges (C)time(s)

To find: The amount of copper deposited and current consumed in a CuCl2 cell connected in series with the cell containing AgNO3.

(b)

Interpretation Introduction

Interpretation:

Need to calculate the amount of copper deposited and current needed to electrolyze the cell containing CuCl2 connected in series with the cell containing AgNO3

Concept introduction:

In the given case two electrolytic cell containing AgNO3 and CuCl2 were connected in series, so the quantity of electricity flowing through both of the cell will be same

Half-cell reaction for cell-1 was given below.

Cathode (reduction) Ag+(aq)+ e-Ag(s)

The amount of the silver deposited was given, from which the amount of electricity flows though both of the cell can be calculated in steps. Number of moles of silver deposited was calculated first.  Since one mole of electron is needed to reduce one mole of Ag+. Therefore number of moles of electron is equal to number of moles of sliver. The coulombs of electron passing can be calculated by the equation given below.

Numberofmolesofsilver=weight(g)Atomicmass(gmole-1)

Numberofmoles of electrons = Number of moles of SilverthenCharges=Numberofmoles of electrons×Faradayconstant (96500C/mole e-)

Half-cell reaction for cell-2 was given below.

Cathode (reduction) Cu2+(aq)+2e-Cu(s)

Since they are connected in series, same amount of charges will be passing through both the cell. From the calculated charges the number of moles of electrons utilized can be calculated.

Numberofmoles of electrons (n)=Charges×Faradayconstant (96500C/mole e-)

From the cell reaction it was known that two mole of electron will be needed to produce one mole of copper,

So

numberofmolesofcopper=nmoleofe×1moleCu2moleeWeightofCopper=numberofmolesofcopper × atomic mass

Since time was given the amperes of current flowing through the circuit can be calculated by the equation given below

Current (A) =charges (C)time(s)

To find: The amount of copper deposited and current consumed in a CuCl2 cell connected in series with the cell containing AgNO3.

Blurred answer

Chapter 19 Solutions

EBK GENERAL CHEMISTRY: THE ESSENTIAL CO

Ch. 19.5 - Prob. 2PECh. 19.5 - Prob. 1RCCh. 19.7 - Prob. 1RCCh. 19.8 - Prob. 1RCCh. 19.8 - An aqueous solution of Mg(NO3)2 is electrolyzed....Ch. 19.8 - Prob. 2RCCh. 19.8 - Prob. 2PECh. 19.8 - Prob. 3RCCh. 19 - Prob. 19.1QPCh. 19 - Prob. 19.2QPCh. 19 - Prob. 19.3QPCh. 19 - Prob. 19.4QPCh. 19 - Prob. 19.5QPCh. 19 - Prob. 19.6QPCh. 19 - 19.7 What is the difference between the...Ch. 19 - Prob. 19.8QPCh. 19 - Prob. 19.9QPCh. 19 - Prob. 19.10QPCh. 19 - Prob. 19.11QPCh. 19 - Prob. 19.12QPCh. 19 - Prob. 19.13QPCh. 19 - 19.14 Which of the following reagents can oxidize...Ch. 19 - 19.15 Consider the following half-reactions: (aq)...Ch. 19 - 19.16 Predict whether the following reactions...Ch. 19 - Prob. 19.17QPCh. 19 - Prob. 19.18QPCh. 19 - Prob. 19.19QPCh. 19 - Prob. 19.20QPCh. 19 - Prob. 19.21QPCh. 19 - Prob. 19.22QPCh. 19 - Prob. 19.23QPCh. 19 - Prob. 19.24QPCh. 19 - Prob. 19.25QPCh. 19 - Prob. 19.26QPCh. 19 - Prob. 19.27QPCh. 19 - Prob. 19.28QPCh. 19 - Prob. 19.29QPCh. 19 - Prob. 19.30QPCh. 19 - Prob. 19.31QPCh. 19 - Prob. 19.33QPCh. 19 - Prob. 19.34QPCh. 19 - 19.35 Explain the differences between a primary...Ch. 19 - Prob. 19.36QPCh. 19 - Prob. 19.37QPCh. 19 - Prob. 19.38QPCh. 19 - Prob. 19.39QPCh. 19 - Prob. 19.40QPCh. 19 - Prob. 19.41QPCh. 19 - Prob. 19.42QPCh. 19 - 19.43 What is the difference between a galvanic...Ch. 19 - Prob. 19.44QPCh. 19 - Prob. 19.45QPCh. 19 - Prob. 19.46QPCh. 19 - Prob. 19.47QPCh. 19 - Prob. 19.48QPCh. 19 - Prob. 19.49QPCh. 19 - Prob. 19.50QPCh. 19 - 19.51 Calculate the amounts of Cu and Br2 produced...Ch. 19 - Prob. 19.52QPCh. 19 - Prob. 19.53QPCh. 19 - Prob. 19.54QPCh. 19 - 19.55 What is the hourly production rate of...Ch. 19 - Prob. 19.56QPCh. 19 - Prob. 19.57QPCh. 19 - Prob. 19.58QPCh. 19 - Prob. 19.59QPCh. 19 - Prob. 19.60QPCh. 19 - Prob. 19.61QPCh. 19 - Prob. 19.62QPCh. 19 - Prob. 19.63QPCh. 19 - Prob. 19.64QPCh. 19 - Prob. 19.65QPCh. 19 - 19.66 A sample of iron ore weighing 0.2792 g was...Ch. 19 - Prob. 19.67QPCh. 19 - Prob. 19.68QPCh. 19 - Prob. 19.69QPCh. 19 - Prob. 19.70QPCh. 19 - Prob. 19.71QPCh. 19 - Prob. 19.72QPCh. 19 - Prob. 19.73QPCh. 19 - Prob. 19.74QPCh. 19 - Prob. 19.75QPCh. 19 - Prob. 19.76QPCh. 19 - Prob. 19.77QPCh. 19 - Prob. 19.78QPCh. 19 - Prob. 19.79QPCh. 19 - Prob. 19.80QPCh. 19 - Prob. 19.81QPCh. 19 - Prob. 19.82QPCh. 19 - Prob. 19.83QPCh. 19 - Prob. 19.84QPCh. 19 - Prob. 19.86QPCh. 19 - Prob. 19.87QPCh. 19 - Prob. 19.88QPCh. 19 - Prob. 19.89QPCh. 19 - Prob. 19.90QPCh. 19 - Prob. 19.91QPCh. 19 - Prob. 19.92QPCh. 19 - Prob. 19.93QPCh. 19 - Prob. 19.94QPCh. 19 - Prob. 19.95QPCh. 19 - Prob. 19.96QPCh. 19 - Prob. 19.97QPCh. 19 - Prob. 19.98QPCh. 19 - Prob. 19.99QPCh. 19 - Prob. 19.100QPCh. 19 - Prob. 19.101QPCh. 19 - 19.102 The magnitudes (but not the signs) of the...Ch. 19 - Prob. 19.103QPCh. 19 - Prob. 19.104QPCh. 19 - Prob. 19.105QPCh. 19 - Prob. 19.106QPCh. 19 - Prob. 19.107QPCh. 19 - Prob. 19.108QPCh. 19 - Prob. 19.109QPCh. 19 - Prob. 19.110QPCh. 19 - 19.111 A spoon was silver-plated electro lyrically...Ch. 19 - Prob. 19.112QPCh. 19 - Prob. 19.113QPCh. 19 - Prob. 19.114QPCh. 19 - Prob. 19.115QPCh. 19 - Prob. 19.116QPCh. 19 - Prob. 19.117QPCh. 19 - Prob. 19.118QPCh. 19 - Prob. 19.119QPCh. 19 - Prob. 19.120QPCh. 19 - Prob. 19.121SPCh. 19 - Prob. 19.122SPCh. 19 - Prob. 19.123SPCh. 19 - Prob. 19.124SPCh. 19 - Prob. 19.125SPCh. 19 - Prob. 19.126SPCh. 19 - Prob. 19.128SPCh. 19 - Prob. 19.129SPCh. 19 - Prob. 19.130SP
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