The cell reaction for a certain alkaline battery is:\[ \text{Zn(s)} + 2\text{MnO}_2\text{(s)} + \text{H}_2\text{O(l)} \rightarrow \text{Zn(OH)}_2\text{(s)} + \text{Mn}_2\text{O}_3\text{(s)} \]Which of the following statements concerning this cell is/are correct?1. MnO\(_2\)(s) is oxidized to Mn\(_2\)O\(_3\)(s) during cell discharge.2. Water is consumed during the discharge of this cell.3. Zn(OH)\(_2\)(s) forms at the anode during discharge of this cell.Options:- ○ 2 only- ○ 1, 2 and 3- ○ 3 only- ○ 1 only- ○ 2 and 3

Answered: Image /qna-images/answer/6db559f6-9f10-4e73-a516-c3be1d9b7674.jpg

Answered: The cell reaction for a certain…

Science

Chemistry

The cell reaction for a certain alkaline battery is Zn(s) + 2MNO2(s) + H2O(1) → Zn(OH)2(s) + Mn2O3(s)

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...

See similar textbooks

Similar questions

Calculate the cell voltage under these conditions. Round your answer to 3 significant digits.
Alkaline Batteries (AA/AAA) Cathode: 2 Mno2 (s) + H2O (I) + 2 e→ Mn,O3 (s) + 2 OH: (aq) +3 · Anode: Zn (s) + 2 OH (aq) → ZnO (s) + H2O (I) + 2 e- · Anode: Zn; Cathode: MnO2 (s) What is the overall balanced equation for the redox reaction occurring in an alkaline (AA/AAA) battery?
A galvanic (voltaic) cell consists of an electrode composed of manganese in a 1.01.0 M manganese(II) ion solution and a second electrode composed of lead in a 1.01.0 M lead(II) ion solution, connected by a salt bridge. Calculate the standard potential for this cell at 25 ∘C25⁢ ∘C. Use this list of standard reduction potentials.
A voltaic electrochemical cell is constructed using the following reaction. The half-cell components are separated by a salt bridge. 21 (aq) + Cl2(g) → 2(s) + 2CI(aq) Write the reactions that take place at the anode and at the cathode, the direction in which the electrons migrate in the external circuit, and the direction the anions in the salt bridge migrate. Use smallest possible integer coefficients. If a box is not needed, leave it blank. Enter the reaction that takes place at the anode. Include state symbols: Enter the reaction that takes place at the cathode. Include state symbols: In the external circuit, electrons migrate v the Cl2 electrode v the I electrode. Anions migrate v the salt bridge v the Cl2 compartment.
A voltaic electrochemical cell is constructed using the following reaction. The half-cell components are separated by a salt bridge. Br2(1) + Mn(s) 2Br"(aq) + Mn2+(aq) Write the reactions that take place at the anode and at the cathode, the direction in which the electrons migrate in the external circuit, and the direction the anions in the salt bridge migrate. Use smallest possible integer coefficients. If a box is not needed, leave it blank. Enter the reaction that takes place at the anode. Include state symbols: Enter the reaction that takes place at the cathode. Include state symbols: In the external circuit, electrons migrate the Mn electrode the Br2 electrode. Anions migrate the salt bridge the Br2 compartment.
A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: Cu²* (ag)+ Zn (s) –→ Cu (s) + Zn²* (ag) 2+ 2+ Suppose the cell is prepared with 7.28 M Cu²" in one half-cell and 7.67 M Zn²™ in the other. Calculate the cell voltage under these conditions. Round your answer to 3 significant digits. x10 믐
What is the balanced overall reaction of the following cell? Ag(s)|Ag+(aq)||Mg2+(aq)|Mg(s) Group of answer choices: 2 Ag(s) + Mg2+(aq) → 2 Ag+(aq) + Mg(s) Ag(s) + Mg 2+(aq) → Ag+(aq) + Mg(s) 2 Ag+(aq) + Mg(s) → 2 Ag(s) + Mg2+(aq) Ag+(aq) + Mg(s) → Ag(s) + Mg2+(aq)
A chemist designs a galvanic cell that uses these two half-reactions: 3+ 2+ Fe (aq)+e → Fe (aq) Cro (aq) + 4H₂O(1)+3e¯ Cr(OH)3(s)+5 OH(aq) Answer the following questions about this cell. Write a balanced equation for the half-reaction that happens at the cathode. Write a balanced equation for the half-reaction that happens at the anode. Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is half-reaction spontaneous as written. 0 standard reduction potential Ed=+0.771 V 'red E 'red = -0.13 V ロ→ロ × x10 5
A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 3Cu* (aq)+ 2Al (s) → 3Cu (s) + 2A1³* (aq) 2+ in one half-cell and 1.05 M Al' in the other. .3+ Suppose the cell is prepared with 5.97 M Cu Calculate the cell voltage under these conditions. Round your answer to 3 significant digits.
A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2+ 2103 (aq) +12H* (aq) + 5Co (s) → 1₂ (s) + 6H₂O (1) +5Co²+ (aq) 2+ Suppose the cell is prepared with 5.23 M IO3 and 2.31 M H in one half-cell and 6.84 M Co in the other. Calculate the cell voltage under these conditions. Round your answer to 3 significant digits.
a galvanic cell consists of a zinc electrode immersed in 0.1 M ZnSO4 solution and another zinc electrode immersed in ZnS saturated solution water. Sketch the galvanic cell, show the anode and cathode. Write the reactions occurring at the anode and cathode , as well as the general reaction of the galvanic element.Calculate the fem of this reaction.
A voltaic cell is based on a nitrate/NO half-cell and a NiCl2/Ni half-cell. (Heads up, the chloride ions in this reaction are bystander ions.) Eo for NO-3 (aq) → NO(g) = +0.96 Eo for NiCl2 (aq) → Ni(s) = –0.28 What is the cell potential of the reaction when pH = 2.7, [NO3-] = 1.5 M, PNO = 0.010 atm and [Ni2+] = 0.21 M