Chemistry for Engineering Students
Chemistry for Engineering Students
4th Edition
ISBN: 9781337398909
Author: Lawrence S. Brown, Tom Holme
Publisher: Cengage Learning
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Chapter 13, Problem 13.43PAE

Calculate the equilibrium constant for the redox reactions that could occur in the following situations and use that value to explain whether or not any reaction will be observed.

(a) A piece of iron is placed in a 1.0 M solution of NiCl2(aq).

(b) A copper wire is placed in a 1.0 M solution of Pb(NO3)2(aq).

(a)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation: The equilibrium constant for the redox reaction should be determined along with by using the value of equilibrium constant identifies whether the reaction occurs or not.

A piece of iron is placed in a 1.0 M solution of NiCl2 (aq).

Concept introduction: The equilibrium constant (Kc) for a reaction is the ratio of the product of the concentration of the products raised to the power of their stoichiometric coefficients to the product of the concentration of the reactants raised to their power of the stoichiometric coefficients. The redox reaction included with electron transfer process. All chemical reactions included with redox reactions. Both oxidation and reduction occurs in redox reactions.

Answer to Problem 13.43PAE

Solution:

Kc=0.4407 and reaction will occur.

Explanation of Solution

An iron piece is placed in 1.0 m NiCl2(aq)

Fe(s) + NiCl(aq)FeCl2(aq) + Ni(s)

Anode:

Fe(s)Fe2++2e

Cathode:

Ni2+(aq)+2eNi(s)

E0Fe+2/Fe = -0.44 VE0Ni+2/Ni = -0.25 V

Formula used:

Ecell0=0.059nlogKc

where,

Ecell0= reduction potential

n =number of electrons

Kc= equilibrium constant

Calculation: Cathode and anode is identified from above equation

E0cell=E0cathodeE0anode= -0.25-(-0.44)= -0.25+0.44= 0.19 V

Ecell0=0.059nlogKc0.19=0.0592logKclogKc=2×0.190.059=6.4407Kc=antilog(6.4407)Kc=0.4407

The value of equilibrium constant is positive which implies product is more and reaction will occur.

Thus, reaction will occur.

(b)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation: The equilibrium constant for the redox reaction should be determined along with by using the value of equilibrium constant identifies whether the reaction occurs or not.

A copper wire is placed in a 1.0 M solution of Pb(NO3)2(aq).

Concept introduction: The equilibrium constant (Kc) for a reaction is the ratio of the product of the concentration of the products raised to the power of their stoichiometric coefficients to the product of the concentration of the reactants raised to their power of the stoichiometric coefficients. The redox reaction included with electron transfer process. All chemical reactions included with redox reactions. Both oxidation and reduction occurs in redox reactions.

Answer to Problem 13.43PAE

Solution:

Kc=1.175×10-16 and reaction will not occur.

Explanation of Solution

Cu(s)+Pb(NO3)2Cu2++Pb(s)

Anode:

Cu(s)Cu2+(aq)+2e

Cathode:

Pb2+(aq)+2ePb(s)

E0Cu+2/Cu = 0.34 VE0Pb+2/Pb = -0.13 V

Formula used:

Ecell0=0.059nlogKc

where,

Ecell0= reduction potential

n =number of electrons

Kc= equilibrium constant

Calculation: Cathode and anode is identified from the above equation.

E0cell=E0cathodeE0anode= -0.13 - 0.34= -0.47 V

Ecell0=0.059nlogKc0.47=0.0592logKclogKc=2×0.470.059=15.93Kc=antilog(15.93)Kc=1.175×1016

In this case, the value of equilibrium constant is so small and reactants predominates over products.

Thus, reaction will not occur.

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Chapter 13 Solutions

Chemistry for Engineering Students

Ch. 13 - Prob. 13.1PAECh. 13 - Prob. 13.2PAECh. 13 - Prob. 13.3PAECh. 13 - Prob. 13.4PAECh. 13 - For the following oxidationreduction reactions,...Ch. 13 - Which half-reaction takes place at the anode of an...Ch. 13 - If a salt bridge contains KNO3 as its electrolyte,...Ch. 13 - If a salt bridge contains KNO3 as its electrolyte,...Ch. 13 - The following oxidationreduction reactions are...Ch. 13 - Write a balanced chemical equation for the overall...Ch. 13 - For the reactions in parts (a) and (b) in the...Ch. 13 - Explain why the terms cell potential and...Ch. 13 - How does galvanic corrosion differ from uniform...Ch. 13 - Prob. 13.14PAECh. 13 - A student who has mercury amalgam fillings in some...Ch. 13 - Based on the cell potential measured for the cells...Ch. 13 - Prob. 13.17PAECh. 13 - Four voltaic cells are set up. In each, one...Ch. 13 - In tables of standard reduction potentials that...Ch. 13 - In the table of standard reduction potentials,...Ch. 13 - Using values from the table of standard reduction...Ch. 13 - Using values from the table of standard reduction...Ch. 13 - One half-cell in a voltaic cell is constructed...Ch. 13 - Four metals, A, B, C, and D, exhibit the following...Ch. 13 - Use the Nernst equation to calculate the cell...Ch. 13 - One half-cell in a voltaic cell is constructed...Ch. 13 - We noted that a tin-plated steel can corrodes more...Ch. 13 - The following half-cells are available: Ag(s);...Ch. 13 - Prob. 13.29PAECh. 13 - Prob. 13.30PAECh. 13 - In May 2000, a concrete pedestrian walkway...Ch. 13 - Prob. 13.32PAECh. 13 - Calculate the standard free energy change for the...Ch. 13 - Suppose that you cannot find a table of standard...Ch. 13 - Prob. 13.35PAECh. 13 - Which of the following reactions is (are)...Ch. 13 - Consult a table of standard reduction potentials...Ch. 13 - The equilibrium constant for a reaction is 31015...Ch. 13 - Some calculators cannot display results of an...Ch. 13 - Calculate the equilibrium constant for the...Ch. 13 - Use the standard reduction potentials for the...Ch. 13 - Hydrogen peroxide is often stored in the...Ch. 13 - Calculate the equilibrium constant for the redox...Ch. 13 - An engineer is assigned to design an...Ch. 13 - A magnesium bar with a mass of 6.0 kg is attached...Ch. 13 - Prob. 13.46PAECh. 13 - Prob. 13.47PAECh. 13 - Prob. 13.48PAECh. 13 - Prob. 13.49PAECh. 13 - If you put a 9-volt battery in a smoke detector in...Ch. 13 - If alkaline batteries were not alkaline but rather...Ch. 13 - What would happen to the voltage of an alkaline...Ch. 13 - What product forms from the lead components of a...Ch. 13 - Prob. 13.54PAECh. 13 - Prob. 13.55PAECh. 13 - Assume the specifications of a Ni-Cd voltaic cell...Ch. 13 - Prob. 13.57PAECh. 13 - What is the difference between active and passive...Ch. 13 - Prob. 13.59PAECh. 13 - Prob. 13.60PAECh. 13 - In an electroplating operation, the cell potential...Ch. 13 - Prob. 13.62PAECh. 13 - Prob. 13.63PAECh. 13 - Prob. 13.64PAECh. 13 - Use the Internet to find electroplating companies...Ch. 13 - Prob. 13.66PAECh. 13 - If a current of 15 A is run through an...Ch. 13 - Suppose somebody in a laboratory doesn't quite...Ch. 13 - If a barrel plating run uses 200.0 A for exactly 6...Ch. 13 - An electrical engineer is analyzing an...Ch. 13 - In a copper plating experiment in which copper...Ch. 13 - A metallurgist wants to gold-plate a thin sheet...Ch. 13 - Tin-plated steel is used for "tin" cans. Suppose...Ch. 13 - An electrolysis cell for aluminum production...Ch. 13 - If a plating line that deposits nickel (from NiCl2...Ch. 13 - Prob. 13.76PAECh. 13 - Prob. 13.77PAECh. 13 - A small part with a surface area of 2.62 cm2 is...Ch. 13 - An engineer is designing a mirror for an optical...Ch. 13 - Prob. 13.80PAECh. 13 - Prob. 13.81PAECh. 13 - What characteristic of lithium ions makes it...Ch. 13 - Looking at Figure 13.23, describe how the...Ch. 13 - Prob. 13.84PAECh. 13 - What is the role of a salt bridge in the...Ch. 13 - Prob. 13.86PAECh. 13 - If the SHE was assigned a value of 3.00 V rather...Ch. 13 - Prob. 13.88PAECh. 13 - Prob. 13.89PAECh. 13 - A chemical engineering student is studying the...Ch. 13 - Prob. 13.91PAECh. 13 - If a logarithmic scale had not been used for the...Ch. 13 - Battery manufacturers often assess batteries in...Ch. 13 - Prob. 13.94PAECh. 13 - Prob. 13.95PAECh. 13 - Prob. 13.96PAECh. 13 - As the voltaic cell shown here runs, the blue...Ch. 13 - Prob. 13.98PAECh. 13 - For a voltage-sensitive application, you are...Ch. 13 - Prob. 13.100PAECh. 13 - Prob. 13.101PAECh. 13 - Prob. 13.102PAECh. 13 - Prob. 13.103PAECh. 13 - 13.104 (a) What happens when a current is passed...Ch. 13 - A current is passed through a solution of...Ch. 13 - 13.106 Hydrazine, N2H4 , has been proposed as the...Ch. 13 - Prob. 13.107PAE
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