1. A student constructed a voltaic cell using nickel and lead as electrodes. He also used 0.25 M Ni(NO3)2 as the anolyte and 0.50 M Pb(NO3)2 as the catholyte. Ni²+ (aq) + 2e → Ni(s), Eºred = -0.25 V Pb²+ (aq) + 2e → Pb(s), Eºred = -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 cell potential at 30 °C, Ecell- D. If the concentration of Ni(NO3)2 solution used was increased, what will be the effect on the measured potential? (increase, decrease, no effect)
1. A student constructed a voltaic cell using nickel and lead as electrodes. He also used 0.25 M Ni(NO3)2 as the anolyte and 0.50 M Pb(NO3)2 as the catholyte. Ni²+ (aq) + 2e → Ni(s), Eºred = -0.25 V Pb²+ (aq) + 2e → Pb(s), Eºred = -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 cell potential at 30 °C, Ecell- D. If the concentration of Ni(NO3)2 solution used was increased, what will be the effect on the measured potential? (increase, decrease, no effect)
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter17: Electrochemistry And Its Applications
Section: Chapter Questions
Problem 84QRT
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Transcribed Image Text:1. A student constructed a voltaic cell using nickel and lead as electrodes. He also used 0.25 M Ni(NO3)2 as the anolyte and 0.50 M Pb(NO3)2 as the catholyte.
Ni2+ (aq) + 2e → Ni(s), Eºred = -0.25 V
Pb²+ (aq) + 2e → Pb(s), Eºred = -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 cell potential at 30 °C, Ecell-
D. If the concentration of Ni(NO3)2 solution used was increased, what will be the effect on the measured potential? (increase, decrease, no effect)
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