A voltaic cell is constructed using the half-reactions below:MnO2 (s) + 4H* (aq) + 2eMn2*(aq) + 2H2O(1)E° = +1.23 V-->TIO2*(aq) + 2H* (aq) + 4e -->Ti(s) + H20(1)E° = -0.88 Va. Write the equation for the reaction that produces a positive standard potential andthen calculate that potential (show half cell reactions and over-all reaction).b. Show the cell notation or cell symbol.c. State whether each of the changes listed in parts i -iii will affect the cell potentialcalculated for the assembled cell. For each change, state whether the potential willincrease, decrease, or remain the same. Outline your reasoning or show your calculationsin each case.i. The [Mn2+] is halved.ii. The size of the Ti(s) electrode is doubled.iii. The pH of both compartments is increased by the same amount.

The reaction cell which is going to produce a positive electrode potential should be the one which…

Answered: A voltaic cell is constructed using the…

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...

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You are asked to build an electrolytic cell using the following two half-reactions:Cu2+(aq) + 2e- -----> Cu(s) E°red = 0.342 VNi2+(aq) + 2e- -----> Ni(s) E°red = -0.257 V What is the minimum voltage required to make this reaction happen?
Given: Half cell reaction E (V) Ag+(aq) + e- ---> Ag(s) 0.80 Cu+2(aq) + 2 e- ---> Cu(s) 0.34 Zn+2(aq) + 2 e- ---> Zn(s) -0.76 Ni+2(aq) + 2 e- ---> Ni(s) -0.23 (a) Pick up two of the above listed half-cells to build a voltaic cell that would have a maximum overall cell potential. Write the overall reaction equation. (b) Draw a detailed cell diagram and indicate which electrode is anode and which is cathode, and indicate the (-) electrode and the (+) electrode.
An electrochemical cell is based on these two half - reactions Ox : Pb(s) -> Pb ^ 2 (aq, 0.20 mol L^ -1 )+2 e^ -; E anode ^ 0 =-0.13(V) Red: MnO4 ^ - (aq,1.55 mol L^ -1 )+4 H^ + (aq,2.0 mol L^ -1 )+3 e^ - MnO^2(s) + 2H_{2}*O(l) E 1.68 (V) Compute the cell potential at 25 ∘C.
You are asked to build an electrolytic cell using the following two half-reactions:Cu2+(aq)+2e−----->Cu(s) E°red = 0.342 VNi2+(aq)+2e−-------->Ni(s) E°red = -0257V What is the minimum voltage required to make this reaction happen? V
You are asked to build an electrolytic cell using the following two half-reactions:Cu2+(aq)+2e−Cu(s) E°red = 0.342 VNi2+(aq)+2e−Ni(s) E°red=-0.257v What is the minimum voltage required to make this reaction happen?
A voltaic cell prepared using aluminum and nickel has the following cell notation. Al(s) | AI3+(aq) || Ni2*(aq) | Ni(s) Which of the following reactions occurs at the cathode? Al(s) Al3*(ag) + 3e- O Ni2*(aq) + 2e- Ni(s) Al3+(aq) + 3e Al(s) > Ni(s) Ni2*(aq) + 2e
Consider a voltaic cell with the cell notation shown below. Which of the following statements is INCORRECT? C(s) | V³+ (aq) (1 M), VO²+ (aq) (1 M), H* (aq) (1 M) || Cr₂O7²- (aq) (4 M), Cr³+ (aq) (0.5 M), H* (aq) (1 M) | C(s) Given: VO²+ (aq) + 2 H+ *(aq) + e² = √³+ (aq) + H₂O(1) E° = +0.34 V Cr₂O7²- (aq) + 14 H* (aq) + 6 e¯ 2 Cr³+ (aq) + 7 H₂0 (1) E° = +1.33 V T = 298.15 K; R = 8.3145 J/mol-K; F = 96485 J/V-mol e The maximum work that can be generated by the cell is - 520 kJ. O Six moles of electrons are involved in the redox reaction. The equilibrium constant for the standard electrochemical reaction is e²31. O The cell potential (Ecell) is 1.00 V.
Consider a voltaic cell in which the following reaction takes place. 2Fe 2+ (aq) + H₂O2 (aq) + 2 H+ (aq) --→2Fe ³+ (aq) +2H₂O (1) calculate Eº Calculate E and Gibbs free energy when [Fe²+] = 0.00813 M, [H₂O₂] = 0.914 M, [Fe ³+] = 0.199 M, [H] = 1.32 x 10³ M
Which statement is correct for the cell with a notation Pt /Cl2(g)/Cl¯(aq) // Zn+2(aq)/Zn ? Cl2 + 2e- --> 2Cl¯ E°=1.360 V Zn+2 + 2e- --> Zn E°= - 0.760 V choose: This is an electrolytic cell. The anode of this cell is negative and the cathode is positive. Work is being done by the cell. This is a voltaic or galvanic cell.
A lithium battery is being developed. Its voltaic cell is constructed based on Li metal electrode and PbsO4 solid electrode. Their standard reduction potentials at 25 °C are given below. E°(Li* (aq) → Li (s)) = -3.040 Volt E°(PbSO4 (S) > Pb (s) + SO42 (aq) = - 0.356 Volt. Which of the following statements is true about this working (spontaneous) voltaic cell? a. The anode is PbsO4 (s) electrode. The standard cell potential of this voltaic cell is E°(cell) = 2.328 Volt O. PBSO4 (s) is a weaker oxidizing agent than Lit. To make a commercial product, the voltaic cell is adjusted to have [Lit] = 2.1 M and [SO42] = 3.5 M. The cell d. potential E under this condition should be less than the standard cell potential E°(cell). e. None of the above
A voltaic cell is constructed with an Ag/Ag+ half-cell and a Pb/Pb+2 half cell. All solutions are 1.0 M. Ag+(aq) + e- → Ag(s) E° = 0.80 V Pb+2(aq) + 2e- → Pb(s) E° = -0.13 V a. If the cell were made with [Pb+2] = 0.10 M and [Ag3+] = 3.0 M, would the voltage increase, decrease, or remain the same? Explain using Q. b. Identify the electrode that is gaining mass.
In a Voltaic cell composed of CuôCu(NO3)2 and AgôAgNO3 half-cells, what is the spontaneous cell reaction and the Eocell, respectively? The standard reduction potentials are as follows: Ag+(aq) + e– --> Ag(s); Eo = 0.80 V Cu2+(aq) + 2e– --> Cu(s); Eo = 0.34 V (A) 2Ag(s) + Cu2+(aq) --> 2Ag+(aq) + Cu(s); Eocell = 1.14 V (B) 2Ag(s) + Cu2+(aq) --> 2Ag+(aq) + Cu(s); Eocell = 1.94 V (C) Cu(s) + 2Ag+(aq) --> Cu2+(aq) + 2Ag(s); Eocell = 0.46 V (D) Cu(s) + 2Ag+(aq) --> Cu2+(aq) + 2Ag(s); Eocell = 1.26 V

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