1. A student constructed a voltaic cell using nickel and lead as electrodes. He also used 0.50 M N (NO) as the anolyte and 0.25 M Pb(NO₂), as the catholyte. Ni2+ (aq) + 2e-→ Ni(s). Ered--025 V Pb2+ (aq) + 2e-→ Pb(s), Ed--0.13V A Write the balanced reaction occurring in the voltaic cell. Write your answers in your solution sheet. B. Compute the standard cell potential, Ee C Calculate the cell potential at 28 °C. Ecel D. If the concentration of Pb(NO3), solution uled was increased, what will be the effect on the measured potential? Gincrease, decrease, no effect)

1. A student constructed a voltaic cell using nickel and lead as electrodes. He also used 0.50 M N (NO) as the anolyte and 0.25 M Pb(NO₂), as the catholyte. Ni2+ (aq) + 2e-→ Ni(s). Ered--025 V Pb2+ (aq) + 2e-→ Pb(s), Ed--0.13V A Write the balanced reaction occurring in the voltaic cell. Write your answers in your solution sheet. B. Compute the standard cell potential, Ee C Calculate the cell potential at 28 °C. Ecel D. If the concentration of Pb(NO3), solution uled was increased, what will be the effect on the measured potential? Gincrease, decrease, no effect)

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

BALANCING REDOX REACTIONS, VOLTAIC CELL AND ELECTROLYSIS 1. A student constructed a voltaic cell using nickel and lead as electrodes. He also used 0.50 M Ni(NO3)2 as the anolyte and 0.25 M Pb(NO3)2 as the catholyte. Ni2+ (aq) + 2e → Ni(s), Eºred = -0.25 V Pb2+ (aq) + 1) + 2e → Pb(s), Ered. = -0.13 V A. Write the balanced reaction occurring in the voltaic cell. Write your answers in your solution sheet. B. Compute the standard cell potential, Eºcell- C. Calculate the potential at 28 °C, Ecell. D. If the concentration of Pb(NO3)2 solution used was increased, what will be the effect on the measured potential? (increase, decrease, no effect)
The diagram below is an electrochemical cell based on a redox reaction that needs to be completed by a student in the laboratory. Zn(s) + Br₂(1)→ Zn²+ (aq) + 2 Br¯(aq) C electron flow? B A H G Salt Bridge Zn E F D Which of the following is true for the cell? O a. The cathode is A, the anode is B and the electrons travel from left to right O b. The cathode is A, the anode is B, however there is no current Oc. The cathode is A, the anode is B and the electrons travel from left to right O d. The anode is A, the cathode is B and the electrons travel from left to right O e. The anode is A, the cathode is B and the electrons travel from right to left
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.Diagram the cell, labeling electrodes and solutions, show the direction of electron flow in the circuit and what occurs in the salt bridge. b. 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. c.Identify the electrode that is gaining mass
Can you break down the problem attached?
22. The diagram below represents a voltaic cell. What is the balanced electrochemical reaction represented by this cell? Al(s))Al³*(1.0 M)||Cu²*(1.0 M)|Cu(s) a. Al(s) + Cu (ag)→ Al** (aq) + Cu(s) b. 2H,0) + 3A1*(aq) + 2Cu(s) → 2A1(s) + 3Cu?*(aq) + 4H*(aq) + 0,(g) c. 2Al(s) + 3Cu?*(aq) → 3AI** (aq) + 2Cu(s) d. Al*(aq) + Cu(s) → Al(s) + Cu?*(aq) e. 3A* (aq) + 2Cu(s) → 2Al(s) + 3Cu²*(aq)
6, Which of the following statements is false about zinc–copper voltaic cell : Zn(s) | Zn2+(1.0 M) || Cu2+(1.0 M) | Cu(s) Group of answer choices A, Electrons flow through the external circuit from the zinc electrode to the copper electrode B, The mass of the zinc electrode increases during discharge C, Reduction occurs at the copper electrode D, The zinc electrode is the anode. E, The concentration of Cu2+ decreases during discharge. 7, What is the SI unit of potential difference? Group of answer choices joule ampere coulomb farad volt
Consider the following half-reactions and their standard reduction potentials then give the standard line (cell) notation for a voltaic cell built on these half reactions. Mn2*(aq) + 2 e Mn(s) E° = -1.18 V Fe(aq) +3 e Fe(s) E° = -0.036 V A. Fe(s) | Fe3t(aq, 1.0 M) || Mn (s) | Mn 2*(aq. 1.0 M) B. Mn (s) | Mn 2*(aq, 1.0 M) | | Fe(s) | Fe(aq. 1.0 M) C. Fe(s) | Fe3t(aq. 1.0 M) || Mn2*(aq, 1.0 M) | Mn(s) D. Mn (s) | Mn 2*(aq. 1.0 M) || Fe(aq, 1.0 M) | Fe(s)
A digital watch battery draws 0.10 milliamperes of current, which is provided by a mercury battery whose net reaction is: HgO(s) + Zn(s) → ZnO(s) + Hg(l) If a partially used battery contains 1.10 g of each of these four substances, for how many hours will the watch continue to run?
Consider the electrochemical cell diagram shown below. As you observe the reaction in the cell, you notice that the tin electrode seems to be disappearing while there are deposits forming on the silver electrode. Which of the following is a correct statement? Sn KNO3(aq) Ag IM Sn (NO3)2 IM AgNO3 O The tin electrode is the cathode and the silver electrode is the anode. O Electrons are flowing from the silver electrode to the tin electrode. O Potassium ions are flowing through the salt bridge to the silver solution. O The half-reaction occurring at the tin electrode is Sn4+ + 2e → Sn2+