In order to charge a lead storage battery (Section 19.10) 500.0 g of PbSO 4 (s) must be converted into PbO 2 (s) and Pb(s). (a) Does the reaction represent an electrolytic or galvanic cell?

Hello everyone in this problem being told that the H G to c l t s l is converted into HD liquid and cl two gas and an experiment we're being asked here is the overall reaction, a galvanic cell or an electrolytic cell. So here let's first recognize what our half reactions are starting with our cathode side. So for the cathode we have our H G two cl two, which is a solid, we're gonna go and add two electrons to this, which yields then the two moles of H G As well as two moles of RCL -. The state of reduction potential here is equal to 0. volts. So these equations as well as the standard reduction potential values are just the values that I have. But of course you can either find this on your own, given to you by professor or even found online. Alright, so continue on then from an outside that we have here, this is equal to two moles of my cl minus which is acquis This yields our one mole of cl two in its gaseous state as well as two electrons. The standard reduction potential for this half reaction is 1. volts. Alright, so from my S. O. They're creating for this is equal to the reduction potential of my cathode minus. The reduction potential of my a node. Of course we do have these values. Let's go ahead and plug that in. So for my cathode side that is 0.28V. And then for my an outside that is 1.36V. Once I put this value into my calculator received, that my sl value is equal to negative 1.08V. Since our sl value is less than zero. So a negative value, of course, this means that we have and electronic, or each electrolytic cell, and this right here is going to be my final answer for this problem.

Ch.19 - Electrochemistry

All textbooks

McMurry 8th Edition

Ch.19 - Electrochemistry

Problem 146a

Previous problem

Next problem

Chapter 19, Problem 146a

In order to charge a lead storage battery (Section 19.10) 500.0 g of PbSO₄(s) must be converted into PbO₂(s) and Pb(s). (a) Does the reaction represent an electrolytic or galvanic cell?

Verified step by step guidance

insert step 1> Identify the type of cell by understanding the process involved. In an electrolytic cell, electrical energy is used to drive a non-spontaneous chemical reaction, whereas in a galvanic cell, a spontaneous chemical reaction generates electrical energy.

insert step 2> Recognize that charging a battery involves reversing the discharge reaction, which is typically non-spontaneous and requires an external power source.

insert step 3> Recall that in a lead storage battery, during discharge, PbO_2 and Pb react with H_2SO_4 to form PbSO_4 and water. Charging the battery involves converting PbSO_4 back into PbO_2 and Pb.

insert step 4> Since the conversion of PbSO_4 to PbO_2 and Pb requires an input of electrical energy, this process is characteristic of an electrolytic cell.

insert step 5> Conclude that the reaction represents an electrolytic cell because it involves the input of electrical energy to drive the non-spontaneous conversion of PbSO_4 into PbO_2 and Pb.

Verified Solution

Video duration:

This video solution was recommended by our tutors as helpful for the problem above.

Was this helpful?

Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Electrolytic vs. Galvanic Cells

Electrolytic cells use electrical energy to drive a non-spontaneous chemical reaction, while galvanic cells generate electrical energy from spontaneous reactions. In electrolytic cells, an external power source is required to facilitate the reaction, whereas galvanic cells produce voltage as a result of the chemical reaction occurring spontaneously.

Lead Storage Battery Chemistry

A lead storage battery operates through the reversible reactions of lead dioxide (PbO2), lead (Pb), and lead sulfate (PbSO4). During discharge, PbSO4 is formed, and during charging, PbSO4 is converted back to PbO2 and Pb, illustrating the principles of redox reactions and energy storage in electrochemical systems.

Redox Reactions

Redox reactions involve the transfer of electrons between two species, resulting in oxidation (loss of electrons) and reduction (gain of electrons). In the context of the lead storage battery, lead sulfate is reduced to lead and oxidized to lead dioxide, highlighting the importance of electron flow in energy conversion processes.

Recommended video:

Guided course

03:12

Identifying Redox Reactions

Previous problem

Next problem

Related Practice

Textbook Question

What constant current (in amperes) is required to produce aluminum by the Hall–Héroult process at a rate of 40.0 kg/h?

424

views

Textbook Question

Electrolysis of a metal nitrate solution M(NO3)2(aq) for 325 min with a constant current of 20.0 A gives 111 g of the metal. Identify the metal ion M2+.

835

views

Textbook Question

Aluminum, titanium, and several other metals can be col-ored by an electrochemical process called anodizing. Anodizing oxidizes a metal anode to yield a porous metal oxide coating that can incorporate dye molecules to give brilliant colors. In the oxidation of aluminum, for instance, the electrode reactions are The thickness of the aluminum oxide coating that forms on the anode can be controlled by varying the current flow during the electrolysis. How many minutes are required to produce a 0.0100-mm thick coating of Al2O3 (density 3.97 g/cm^3) on a square piece of aluminum metal 10.0 cm on an edge if the current passed through the piece is 0.600 A?

768

views

Textbook Question

In order to charge a lead storage battery (Section 19.10) 500.0 g of PbSO₄(s) must be converted into PbO₂(s) and Pb(s). (b) How many coulombs of electrical charge are needed?

191

views

Textbook Question

In order to charge a lead storage battery (Section 19.10) 500.0 g of PbSO₄(s) must be converted into PbO₂(s) and Pb(s). (c) If a current of 500 A is used, how long will it take?

Textbook Question

When the nickel–zinc battery, used in digital cameras, is recharged, the following cell reaction occurs: (a) How many grams of zinc are formed when 3.35 x 10^-2 g of Ni(OH)₂ are consumed?

281

views

In order to charge a lead storage battery (Section 19.10) 500.0 g of PbSO4(s) must be converted into PbO2(s) and Pb(s). (a) Does the reaction represent an electrolytic or galvanic cell?

Verified Solution

Key Concepts

Electrolytic vs. Galvanic Cells

Lead Storage Battery Chemistry

Redox Reactions

In order to charge a lead storage battery (Section 19.10) 500.0 g of PbSO₄(s) must be converted into PbO₂(s) and Pb(s). (a) Does the reaction represent an electrolytic or galvanic cell?