If an alkaline battery produces a cell potential of 1.50 V, what is the value of AGcell? The half-reactions in alkaline batteries are: ZnO(s) + H,0(1) + 2e → Zn(s) + 2OH¯(aq) 2MnO, (s) +H,0(1) + 2e¯ ► Mn,0, (s) - + 20H¯(aq) 1st attempt i See Periodic Tal AGcell = kJ

If an alkaline battery produces a cell potential of 1.50 V, what is the value of AGcell? The half-reactions in alkaline batteries are: ZnO(s) + H,0(1) + 2e → Zn(s) + 2OH¯(aq) 2MnO, (s) +H,0(1) + 2e¯ ► Mn,0, (s) - + 20H¯(aq) 1st attempt i See Periodic Tal AGcell = kJ

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

Related questions

Q: The standard cell potential, begin mathsize 12px style E subscript c e l l end subscript superscript…

A: The standard cell potential, begin mathsize 12px style E subscript c e l l end subscript superscript…

Q: Four voltaic cells are set up. In each, one half-cell contains a standard hydrogen electrode (SHE).…

Q: Answer all parts below, which are related to each other. The following electrochemical cell has a…

A: Given: The following electrochemical cell has a cell voltage of 0.033 V at 25 oC and 1.00 atmosphere…

Q: Combine the half-reactions shown into three different spontaneous redox reactions, calculating…

A: The objective of the question is to combine the given half-reactions into three different…

Q: Answer the questions below considering the cell below at 25°C: Pt(s) | Sn(NO3)2 (aq) (b= 0.001…

A: In an electrochemical cell at anode oxidation and at cathode reduction takes place.

Q: What is the calculated value of the cell potential at 298K for an electrochemical cell with the…

Q: When the Hg2+ concentration is 8.62×104 M, the observed cell potential at 298K for an…

Q: A Cu"(aq, 0.15MyCu(s) half cell is connected to a H"Hzlg. 1.00atm) half cell in which the hydrogen…

A: Since Cu+(aq) has higher reduction potential, Cu+(aq) undergoes reduction to Cu(s), and H2(g)…

Q: For the KI solution, The following oxidation and reduction half-reactions are possible for the…

Q: An electrochemical cell is based on the following two half-reactions: oxidation: Sn (s) →Sn²+ (aq,…

A: Given: oxidation : Sn (s) → Sn2+(aq) + 2e- Eo = -0.14 V reduction: ClO2 (s) + e- →ClO2-(aq)…

Q: O ADVANCED MATERIAL Designing a galvanic cell from two half-reactions A chemist designs a galvanic…

A: Here we are required to find the cell potential of the given electrochemical reaction.

Q: E e' G B H Choose the label which best describes the following: C Solution containing Fe2+ and Fe 3+…

A: An electrochemical device that transforms chemical process free energy into electrical energy is…

Q: 5) In an electrochemical cell, Cu(s) is placed in the anode half-cell while Ag(s) in the cathode…

Q: 3. Calculate the standard cell potential AND determine whether the following reactions are at…

A: We will determine whether the reaction is spontaneous or not by calculating Eocell.

Q: What is the Ecell for the non-standard state, but 25 C, voltaic cell shown below? Zn(s) | Zn2*(0.015…

A: Given that: E°Zn2+/Zn = -0.76V E°Fe3+/Fe2+ = 0.77V

Q: When the Cu²+ concentration is 1.18 M, the observed cell potential at 298K for an electrochemical…

Q: Determine the equilibrium constant for the following reaction in the specified cell. The reaction is…

A: The reaction occurs at anode is: A(s)→A+aq+e-......(1) The reaction occurs at cathode is:…

Q: What is the calculated value of the cell potential at 298K for an electrochemical cell with the…

A: The given cell reaction is as follows --- 3 Ag+ (aq) + Al (s) → 3 Ag (s) +…

Q: What is the cell potential for the reaction at 89 °C when [Fe2+] = 2.80 M and [Mg2+] = 0.110 M.…

Q: You decide to make a battery with the following elements. Cu²+(aq) + Pb(s) → Cu(s) + Pb²+(aq) What…

A: The given reaction is a redox reaction, which can be split into two half-reactions. The…

Q: 2+ - What is E' for the following balanced reaction? Zn(s) + Pb*(aq) → Zn (aq) + Pb(s). 2+…

Q: What is the calculated value of the cell potential at 298K for an electrochemical cell with the…

A: The given chemical reaction:Determine the cell potential.Cell potential, also known as…

Q: 3. A proper cell notation for a galvanic cell featuring a tin electrode and an iron electrode would…

A: The objective of this question is to write a proper cell notation for a galvanic cell featuring a…

Q: Balance each of the following unbalanced equations, then calculate the standard potential, Eº, and…

A: A Galvanic cell is made up of an anode and a cathode. Reduction reaction occurs at cathode whereas…

Q: 13.25 Use the Nernst equation to calculate the cell potentials of the following cells at 298 K. (a)…

Q: The following voltaic cell is built: Ag (s) | Ag + (sat Ag2Cr04) || Ag + (0.125 M) | Ag (s) a) What…

A: Given The following voltaic cell is - Ag (s) Ag+ (sat Ag2CrO4) ∥ Ag+ (0.125 M) Ag (s) At cathode -…

Q: The balanced chemical equation for the over-all reaction represented as AI | AI+3 || Cu+2 | Cu

A: Balanced chemical equation for the over-all reaction represented as AI | AI+3 || Cu+2 | Cu

Q: the standard cell potential (E°cell) of the reaction below is +0.126V what is the value of ▲G° for…

Q: For a voltaic cell based on the reaction below, which statement is correct?…

Q: The value of Kgp for AgBr is 5.4 x 10 13. For the Ag/AgBr electrode, AgBr(s) + e = Ag(s) + Br (aq)…

Q: What is the cell potential (in V) for the reaction below with the given concentrations at 33.0 oC?…

A: Given concentrations:[H+] = 0.152 M[NO3- ] = 0.470 M[Fe3+ ] = 0.885 M[NO] = 0.623 MFirst, let's…

Q: When the Pb²+ concentration is 1.49×104 M, the observed cell potential at 298K for an…

A: Given,The cell reactions:(i) cell potential = 0.501 V[ Pb2+ ] = 1.49 x 10-4 M

Q: When the Hg2+ concentration is 4.78x10^-4 M, the observed cell potential at 298K for an…

A: We will calculate the E0cell of the reaction using reaction potentials of different electrodes.…

Q: title = q8a2 You construct a voltaic cell with Al(s |AI*(aq) || I2(s)| l"(ag) What will be the cell…

A: Oxidation half reaction: 2Al3+ + 6e ⇌ 2Al Reduction half reaction: 3I2 + 6e ⇌6I- So, the overall…

Q: What is the calculated value of the cell potential at 298K for an electrochemical cell with the…

A: NOTE: please note Reduction potential value has not been provided in the Question. so, I have…

Q: Which of the following reactions occur spontaneously as written, with the production of a measurable…

A: Answer: According to the given reactivity series, element that is present above is more reactive…

Q: A electrolytic cell operating under standard conditions (1.0 M lon concentrations) utilizes the…

A: The cell reaction given is, =>

Q: What is the calculated value of the cell potential at 298K for an electrochemical cell with the…

A: The reaction given is Cl2 (g) + Fe (s) --------> 2 Cl- (aq) + Fe2+ (aq) In the above reaction we…

Q: Question: A galvanic cell consists of Zn²" (aq, 0.45M) | Zn (s) and the standard hydrogen 17…

A: Galvanic cell with following electrode reactions: Zn2+(aq, 0.45 M)/Zn(s) with standard electrode…

Q: What is the calculated value of the cell potential at 298K for an electrochemical cell with the…

Q: Sketch the galvanic cell represented by the following line notation: Ag (s), AgCI(s) | KCI (aq, 0.1…

A: It is given that the cell is represented by the notation Ag (s), AgCl(s) | KCI (aq, 0.1 M)||FeCl2…

Q: A student wishes to determine the chloride ion concentration in a water sample at 25 °C using a…

A: Reaction :- 2Ag(s) + 2Cl-(aq) + Cu+2(aq) ------> 2AgCl + Cu(s)

Q: the following reaction? Cu(s)+Zn2+(aq)(1.0M)⇌Cu2+(aq)(1.0M)+Zn(s) EoCu2+/Cu = +0.34 V EoZn2+/Zn =…

A: In this question, we want to determine the standard cell potential of this give Equilibrium cell…

Q: Consider the following half-reactions: Half-reaction E° (V) Hg2+(aq) + 2e Cu2+(aq) + 2e™ Hg(1)…

A: Since you have posted a question with multiple sub-parts, we will solve the first three subparts for…

Concept explainers

Electrolysis

Electrolysis is defined as the process of breaking down ionic compounds into their constituent elements by passing a direct electric current through the compound in a fluid state. The cathode reduces cations, while the anode oxidizes anions. An electrolyte, electrodes, and some form of external power source are the main components required for conducting electrolysis. A partition, such as an ion-exchange membrane or a salt bridge, may also be used, but this is optional. These are primarily used to prevent the products from diffusing near the opposing electrode.

Question

If an alkaline battery produces a cell potential of 1.50 V, what is the value of AGcell? The half-reactions in alkaline batteries are:
ZnO(s) + H,0(1) + 2e¯
→ Zn(s) + 20H¯(aq)
2MnO, (s) +H,0(1) +2e¯
Mn,0, (s) +20H (ag)
1st attempt
l See Periodic Table
AGcell =
kJ

Expert Solution

This question has been solved!

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

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

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

Can you please answer these two sub problems and show all of the steps to the solution
-4 > © Macmillan Learning A redox reaction used in an electrochemical cell has a negative standard free energy change, AGrxn. Which statement about the redox reaction is true? Ecell is positive; K >1 Ecell is negative; K > 1 Ecell is negative; K <1 Ecell is positive; K < 1 Q a M 09.
4
4- help pls
What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the H, pressure is 3.37×10-3 atm, the H* concentration is 1.04M, and the Mg2+ concentration is 7.01×10-4M ? 2H (аq) + Mg(s)—— Н2(g) + - Mg2*(aq) Answer: The cell reaction as written above is spontaneous for the concentrations give v true false Submit Answer Retry Entire Group 9 more group attempts remaining
What is the correct shorthand notation for the cell on the previous slide? Oxidation: Ag(s) Ag*(aq) + e- Reduction: Mno,(s) + 4 H*(ag) + 2 e - Mn2+(aq) + 2 H,0() A. Ag(s) | Ag*(aq) || H*(aq), Mn²*(aq), H20() | MnOg(s) В. Ag*(aq) | Ag(e) || Mn02(a) | Mn²*(aq), H20(). H*(aq) C. Mno2(3) | H*(aq), Mn²*(aq), H20() || Ag*(aq) | Ag(3) D. Mn2*(aq). H20(). H*(@q) | MnO2(s) || Ag(3) | Ag*(aq)
Item 1 < 1 of 25 Constants | Periodic Table Part A The standard cell potential (E') of the reaction below is -0.55 V. The value of A G for the reaction is J/mol. I2 (5) + 2Br (aq) → 21 (aq) + Brz (1) O 1.1- 105 O 0.54 O 0.55 O 5.5 - 106 O none of the above Submit Request Answer
eq Preq 1req F2 # 3 LU E D What is the calculated value of the cell potential at 298 K for an electrochemical cell with the following reaction, when the Pb²+ concentration is 8.54 x 10-4 M and the Mg2+ concentration is 1.23 M ? Ecell F3 The cell reaction as written above is Submit Answer $ SA 4 2+ Pb²+ (aq) + Mg(s) → Pb(s) + Mg²+ (aq) R F V V F4 % References] Use the References to access important values if needed for this question. стор T Retry Entire Group G DII Cengage Learning Cengage Technical Support F5 OL Y H F6 9 more group attempts remaining & 7 U ✓for the concentrations given. F7 J OO PrtScn BN M F8 K Home F9 L End F10 Previous PgUp F11 Next Save and Exit 4x10 PgDn 8:28 PM 12/2/2022 F12 1 Ins {
When the Ag* concentration is 1.33 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is 3.279V. What is the Mg?+ concentration? 2Ag*(aq) + Mg(s)- →2Ag(s) + Mg²*(aq) Answer: M
+ Cell Potential and Equilibrium The equilibrium constant, K, for a redox reaction is related to the standard potential, E, by the equation In K FE RT where 72 is the number of moles of electrons transferred, F (the Faraday constant) is equal to 96,500 C/(mol e-). R (the gas constant) is equal to 8.314 J/(mol K), and T is the Kelvin temperature. Standard reduction potentials ▾ Part A Use the table Express your answer numerically. ▸ View Available Hint(s) K= ΥΠΙ ΑΣΦ 9 Reduction half-reaction Ag+ (aq) +eAg(s) Cu²+ (aq) +201 >Cu(s) Sn+ (aq) + 4e →→Sn(s) 2H+ (aq) +2e →H₂(g) Ni2+ (aq) + 2e →Ni(s) Fe²+ (aq) + 2e →Fe(s) Zn²+ (aq) +2e →Zn(s) Al³+ (aq) + 3e →Al(s) Mg²+ (aq) + 2e →Mg(s) standard reduction potentials given above to calculate the equilibrium constant at standard temperature (25 °C) for the following reaction: Fe(s) + Ni²+ (aq) →>Fe²+ (aq) + Ni(s) ? E (V) 0.80 0.34 0.15 0 0.26 -0.45 0.76 -1.66 2.37 29 o Review | Constants | Period
Please help with multiple choice question
▾ Part A For the reaction 2Co³+ (aq) + 2Cl(aq)-2Co2+ (aq) + Cl₂(g). E = 0.483 V what is the cell potential at 25°C if the concentrations are [Co³+] = 0.495 M. [Co²+] = 0.295 M, and [CI] = 0.272 M, and the pressure of Cl₂ is Pc, = 8.50 atm ? Express your answer with the appropriate units. View Available Hint(s) E= Submit 0 HA Value Units GAEC LIST onstans Periodic Table ?