Voitmeter Cr(s) Ag(s) Cr*(aq) Ag (aq) 1) The Galvanic cell pictured above is constructed with chromium metal immersed in a Cr(NO,), solution in one half-cell and silver metal immersed in a AgNO, solution in the other half-cell. When the cell operates, a reaction occurs according to the net-ionic equation below. Cr(s) + 3 Ag*(aq) → Cr*(aq) + 3 Ag(s) a) The diagram of the Galvanic cell is incomplete. Draw and label the missing component that is necessary for the cell to operate. b) What is the purpose of this component drawn in part a? c) Write the oxidation half equation. d) Write the reduction half equation. स e) Which metal is the cathode? f) Which metal is the anode? g) Indicate if the values listed below increase, decrease or remain the same as the reaction proceeds. Recall - brackets around a chemical means the Molarity of. i) Mass of Cr(s) iii) [Ag'] ii) Mass of Ag(s) iv) [Cr*]

Voitmeter Cr(s) Ag(s) Cr(aq) Ag (aq) 1) The Galvanic cell pictured above is constructed with chromium metal immersed in a Cr(NO,), solution in one half-cell and silver metal immersed in a AgNO, solution in the other half-cell. When the cell operates, a reaction occurs according to the net-ionic equation below. Cr(s) + 3 Ag(aq) → Cr(aq) + 3 Ag(s) a) The diagram of the Galvanic cell is incomplete. Draw and label the missing component that is necessary for the cell to operate. b) What is the purpose of this component drawn in part a? c) Write the oxidation half equation. d) Write the reduction half equation. स e) Which metal is the cathode? f) Which metal is the anode? g) Indicate if the values listed below increase, decrease or remain the same as the reaction proceeds. Recall - brackets around a chemical means the Molarity of. i) Mass of Cr(s) iii) [Ag'] ii) Mass of Ag(s) iv) [Cr]

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.

Question

Voitmeter
Cr(s)
Ag(s)
Cr*(aq)
Ag*(aq)
1) The Galvanic cell pictured above is constructed with chromium metal immersed in a Cr(NO3); solution in one
half-cell and silver metal immersed in a AgNO, solution in the other half-cell. When the cell operates, a
reaction occurs according to the net-ionic equation below.
Cr(s) + 3 Ag*(aq) → Cr*(aq) + 3 Ag(s)
+3,
a) The diagram of the Galvanic cell is incomplete. Draw and label the missing component that is necessary for
the cell to operate.
b) What is the purpose of this component drawn in part a?
c) Write the oxidation half equation.
d) Write the reduction half equation.
e) Which metal is the cathode?
f) Which metal is the anode?
g) Indicate if the values listed below increase, decrease or remain the same as the reaction proceeds, Recall -
brackets around a chemical means the Molarity of.
Mass of Cr(s)
iii) [Ag']
i)
athe seyt
ii)
Mass of Ag(s)
iv)
[Cr*]

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