A galvanic cell is constructed at 25°C by connecting two half-cells; an aluminium electrode in1.0 M aluminium nitrate, Al(NO3)3 and a lead electrode in 1.0 M lead(II) nitrate, Pb(NO3)2 usingexternal wire and a potassium nitrate, KNO3 salt bridge.1.(a)Draw and label the cell diagram.(b)State the function of a salt bridge.(c)Write reaction at the anode and the cathode and the overall cell reaction.(d)Calculate the standard cell potential, E°cell-(e)Which electrode will increase in weight? Explain your answer.Calculate the cell potential, Ecell if the concentration of aluminium nitrate and lead(II)nitrate are 0.50 M and 3.00 M respectively.(f)(g)What would happen to the value of cell potential if:i.the concentration of aluminium nitrate solution is increased?i.the concentration of lead(II) nitrate solution is increased?iii.the diameter of lead electrode is decreased?

A galvanic cell is the one in which the reaction in the electrode results in the generation of…

A galvanic cell is constructed at 25°C by connecting two half-cells; an aluminium electrode in 1.0 M aluminium nitrate, Al(NO3)3 and a lead electrode in 1.0 M lead(II) nitrate, Pb(NO3)2 using external wire and a potassium nitrate, KNO3 salt bridge. (a) Draw and label the cell diagram. (b) State the function of a salt bridge. (c) Write reaction at the anode and the cathode and the overall cell reaction. (d) Calculat

A galvanic cell is constructed at 25°C by connecting two half-cells; an aluminium electrode in 1.0 M aluminium nitrate, Al(NO3)3 and a lead electrode in 1.0 M lead(II) nitrate, Pb(NO3)2 using external wire and a potassium nitrate, KNO3 salt bridge. (a) Draw and label the cell diagram. (b) State the function of a salt bridge. (c) Write reaction at the anode and the cathode and the overall cell reaction. (d) Calculat

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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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.

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A galvanic cell is constructed at 25°C by connecting two half-cells; an aluminium electrode in
1.0 M aluminium nitrate, Al(NO3)3 and a lead electrode in 1.0 M lead(II) nitrate, Pb(NO3)2 using
external wire and a potassium nitrate, KNO3 salt bridge.
1.
(a)
Draw and label the cell diagram.
(b)
State the function of a salt bridge.
(c)
Write reaction at the anode and the cathode and the overall cell reaction.
(d)
Calculate the standard cell potential, E°cell-
(e)
Which electrode will increase in weight? Explain your answer.
Calculate the cell potential, Ecell if the concentration of aluminium nitrate and lead(II)
nitrate are 0.50 M and 3.00 M respectively.
(f)
(g)
What would happen to the value of cell potential if:
i.
the concentration of aluminium nitrate solution is increased?
i.
the concentration of lead(II) nitrate solution is increased?
iii.
the diameter of lead electrode is decreased?

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