Which is a type of secondary battery that can store a large amounts of charge andproduces large currents?Leclanché cellO Nickel cadmium batteryLithium ion batteryO Alkaline batteryLead-acid battery

In this question, we have to find out the correct answer of given problem by the help of the…

Which is a type of secondary battery that can store a large amounts of charge and produces large currents? O Leclanché cell O Nickel cadmium battery O Lithium ion battery O Alkaline battery Lead-acid battery

Which is a type of secondary battery that can store a large amounts of charge and produces large currents? O Leclanché cell O Nickel cadmium battery O Lithium ion battery O Alkaline battery Lead-acid battery

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 91QAP

See similar textbooks

Related questions

Q: Which of the following statements about a concentration cell is false? O a. The concentration…

A: Concentration cells are those cells in which , electro Motive Force is generated by difference in…

Q: 2 When the copper electrode is replaced by the standard hydrogen electrode in the previous cell, the…

A: If Cu electrode is replaced by a standard hydrogen electrode then the cell reaction will be as…

Q: 10. In an electrolytic cell A. the anode is positively-charged B. the cathode is positively charged…

A: In an electrolytic cell, the process of electrolysis takes place. It is the process in which…

Q: enumerate 10 importance of fuel cells

A: The answer is attached below-

Q: Consider a voltaic cell constructed using the following two reductions: Fe+3 +3e- -->Fe…

A: When there if flow of electrons from one half cell to the another due to which some potential…

Q: A secondary cell (battery) can operate either as a galvanic or an electrolytic cell. True or False…

Q: Identify what is reduced and what is oxidized in the zinc-carbondry-cell battery. What features make…

A: The oxidation number represents the number of electrons gain or loses by an element to become…

Q: In which of the following pairs of metals forming electrochemical cells will the anode undergo the…

A: Standard electrode potential is defined as the electrode potential of metal electrode as determined…

Q: What is the purpose of the salt bridge in a voltaic cell? O To increase solubility of the…

A: The purpose of the salt bridge in a voltaic cell has to be given.

Q: Both a D-sized and an AAA-sized alkaline battery have an output of 1.5 V. What property of the cell…

A: Given Battery output voltage = 1.5 V

Q: Mg(s) | Mg²*(0.025 M) || Mg²*(1.5 M) | Mg(s) Use the Nernst equation to calculate the emf of this…

A: The given cell is a concentration cell. The electrodes are same in both the half cells only the…

Q: In a Lithium Ion battery, what plays the role of the “salt bridge” in the battery?

A: The salt bridge is a device which connects the two half cells of a Galvanic Cell. Lithium Ion…

Q: When a voltaic cell reaches equilibrium: a) E= 0 b) Ecell = 0 c) Ecell = K d) E = K

A: The relationship between the potential of an electrochemical cell and change in gibbs energy is…

Q: Consider the cell described below. Al | Al3+ (1.00 M) || Pb2+ (1.00 M) | Pb Calculate the cell…

Q: 1. The top commercial applications of Voltaic/galvanic electrochemical cells are batteries: There…

Q: Which of the following items is not the electrode in voltammetry A. Reference electrode B. Auxiliary…

Q: 18.39 Consider the following galvanic cells: 1. Cu(s)|Cu²*(1 M) || Fe³*(1 M), Fe²*(1 M)|Pt(s)

A: The balanced chemical reaction is the one that contains equal number of atoms on both sides of the…

Q: For a voltaic cell, which will cause the greatest increase in cell potential? Select one: A.…

A: From Nernst equation, we know that. Ecell=E0 cell-0.059/n log oxidation/reduction At…

Q: Which type of battery is rechargeable? A) alkaline battery C) dry cell B) button battery D) lead…

A: We know that , Primary batteries are non-rechargeable batteries. Example: dry cell, button battery,…

Q: of the following cell diagrams represents a galvanic cell? (ɛ° red(Cd E(s) | Cd2*(aq) || H*(aq)|…

A: 1) Given , Current (i) = 18.0 A Time(t) = 4.40 × 3600 = 15840 s Charge (Q) = it = 15840 ×18 =…

Q: describe the electrochemistry involved in each battery.(a) Leclanche dry cell (b) button battery (c)…

A: Since you have posted multiple sub parts, the answer for first three sub-parts are given below.…

Q: Construct a complete galvanic cell/voltanic cell set up. Label it and show the flow of electrons and…

Q: Consider the voltaic cell: Sr(s)|Sr²+ (1.0 M)||H* (1.0 M)|H₂ (1 atm)|Pt(s) Which of the following…

A: Electrochemistry is branch of chemistry in which we deal with oxidation and reduction reactions…

Q: Which of the following cells is most likely to be an example of a galvanic cell? (A Zn(s) | Zn,+ ||…

Q: Diagram this cell and answer these questions: a) Direction of electron flow b) Half reactions c)…

A: Since you have posted multiple questions according to guidelines I am solving first three.If you…

Q: 11.If ΔG° is positive (+) for a reaction, then 12. Which of the following terms can be used to…

A: Welcome to bartleby ! As per company norms we cannot answer more than one question .But I have…

Q: What do we call the electrode that can be oxidized or reduced in half reaction? [A] Inert electrode…

Q: making a specific galvanic cell, explain how one decides on the electrodes and the solutions to use…

A: To find out the potential developed in between a metal that is immersed in the solution, an…

Q: What is the emf of a galvanic cell consisting of a Cd²+/Cd half-cell and a Pt/H/H₂ half-cell at the…

Q: Can you make an electrochemical cell by placing a silver electrode in 1.00 L of 4 g AgI (Ksp =…

A: In the given cell redox reaction happens in which chemical energy is converted into electrical…

Q: Consider an electrochemical cell operating under standard conditions and at 25 °C. One half cell is…

Q: A battery that cannot be recharged is classified as a _____ A) primary battery B) secondary…

A: A battery that cannot be recharged is classified as a

Q: Write the cell reaction of a lead storage battery when it is discharged. How does the density of the…

A: The cell reaction is as follows,

Q: Given the cell notation: Fe/Fe²*(0.100M)/Cd²*(0.001)/Cd a. Write the cell reaction b. Calculate…

Q: 12. Which of the following terms can be used to describe an electrochemical cell in which a…

A: 12) Answer :- Option 2 is correct. A galvanic cell (Energy released by spontaneous redox reaction is…

Q: In the following cell, write the half reaction that takes place at the anode and the half reaction…

A: Welcome to bartleby ! We have to tell anode and cathode reaction .

Q: In Zn-Cu galvanic cell, the amount of electrical energy produced is A. 2.12 x 105 J B. -6.18 x 103…

Q: Which of the following are true when a battery dies? Select an answer and submit. For keyboard…

A: A battery cell dies when the (b) cell potential is zero.

Q: Consider the galvanic cell: Pt(s) | H2(1 atm)|H*(1 M) || CI'(1 M) | Hg2Cl2(s)|Hg(l) Which of the…

A: Nernst equation: The Nernst equation relates to the reduction potential of an electrochemical…

Q: Given the reaction for the nickel cadmium battery, which species is oxidized during the discharge of…

A: Given :- 2NiO(OH)(s) + Cd(s) + 2H2O(l) → 2Ni(OH)2(s) + Cd(OH)2(s) To identify :- oxidized species…

Q: Question attached

A: Electrode potentials for the copper and aluminum are; ECu2+|Cuo=0.337 VEAl3+|Alo=-1.662 V So, from…

Q: Which of the following statements associated with the pH meter is incorrect? (A) The pH meter should…

A: A question based on electrolysis that is to be accomplished.

Q: If a voltaic cell is created between a Sr2+/Sr electrode and a In3+/ln electrode, what species is…

A: We know, Higher the standard Electrode potential higher will be the ability to behave as oxidizing…

Q: Which of the following voltaic cells is incorrectly labeled? O a. Leclanche dry cell / primary O b.…

A: A voltaic cell is an electro-chemical cell that uses a chemical reaction to produce electrical…

Q: Consider the voltaic cell: Mg Mg2+ (1.0 M)||H* (1.0 M)|H₂ (1 atm)|Pt(s) Which of the following…

A: Answer : increase the pressure of H2 at 2.0 atm Explanation :

Q: Which is a type of secondary battery that can store large amounts of charge and produce large…

A: Batteries are generally of two types, primary and secondary. Primary batteries are those in which…

Q: Which of these is NOT a component of a three-electrode cell? constant electrode O working electrode…

A: In the given question, we need to tell about the components of a three electrode cell. So among the…

Q: The mostly familiar known .37 standard cell is Fuel cell .A B. Le Clanche C. Electrolytic cell

A: There are two types of electrochemical cells in electrochemistry known as voltaic or galvanic and…

Q: of the following batteries does not use zinc as the anode? Lithium-ion Battery LeClanche…

A: Lithium ion batteries consists of four main components - Anode , cathode , electrolyte & a…

Q: Which is a type of secondary battery that can store a large amounts of charge and produces large…

A: Here we have to predict the secondary cell that can store large amount charge and produce large…

Question

Which is a type of secondary battery that can store a large amounts of charge and
produces large currents?
Leclanché cell
O Nickel cadmium battery
Lithium ion battery
O Alkaline battery
Lead-acid battery

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

SEE SOLUTION Check out a sample Q&A here

Step 1 Brief introduction about question.

VIEW

Step 2 Correct answer of given question.

VIEW

Step by step

Solved in 2 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

Consider the cell Pt|H2|H+H+|H2|Pt In the anode half-cell, hydrogen gas at 1.0 atm is bubbled over a platinum electrode dipping into a solution that has a pH of 7.0. The other half-cell is identical to the first except that the solution around the platinum electrode has a pH of 0.0. What is the cell voltage?
Consider a battery made from one half-cell that consists of a capper electrode in 1 M CuSO4 solution and another half—cell that consists of a lead electrode in 1 M Pb(NO3)2 solution. (a) What are the reactions at the anode, cathode, and the overall reaction? (b) What is the standard cell potential for the battery? (c) Most devices designed to use dry-cell batteries can operate between 1.0 and 1.5 V. Could this tell he used to make a battery that could replace a dry-cell battery? Why or why not. (d) Suppose sulfuric acid is added to the half—cell with the lead electrode and some PbSO4(s) forms. Would the cell potential increase, decrease, or remain the same?
Four voltaic cells are set up. In each, one half-cell contains a standard hydrogen electrode. The second half-cell is one of the following: (i) Cr3+(aq, 1.0 M)|Cr(s) (ii) Fea+(aq, 1.0M)|Fe(s) (iii) Cu2+(aq, 1.0M)|Cu(s) (iv) Mg2+(aq, 1.0M)|Mg(s) (a) In which of the voltaic cells does the hydrogen electrode serve as the cathode? (b) Which voltaic cell produces the highest potential? Which produces the lowest potential?
You have 1.0 M solutions of Al(NO3)3 and AgNO3 along with Al and Ag electrodes to construct a voltaic cell. The salt bridge contains a saturated solution of KCl. Complete the picture associated with this problem by a writing the symbols of the elements and ions in the appropriate areas (both solutions and electrodes). b identifying the anode and cathode. c indicating the direction of electron flow through the external circuit. d indicating the cell potential (assume standard conditions, with no current flowing). e writing the appropriate half-reaction under each of the containers. f indicating the direction of ion flow in the salt bridge. g identifying the species undergoing oxidation and reduction. h writing the balanced overall reaction for the cell.