An electrochemical cell consists of a half-cell in which a piece of platinum wire is dipped into a solution that is 2.5 M in KI and 0.046 M in I2. The other half-cell consists of magnesiummetal immersed in a 0.37 M Mg2+ solution. Assume that the temperature is 25°C.(a) Which electrode is the anode and which is the cathode?anode:Pt|I2, I-O Mg²+|Mgcathode:O Pt|I2, I-Mg2+|Mg(b) What is the emf of the cell?4.02.869X V(c) What is the spontaneous cell reaction?chemPadOHelpGreek -Mg2+(aq)+21 (aq)Mg(s)+I2(aq)Mg(s)+l_2(aq)-->Mg^2+(aq)+2l^-(aq)Your answer appears to have inconsistent states-of-matter.(d) What is the equilibrium constant of the cell reaction?2.42e98

Solution: In electrochemical cell, oxidation takes place at anode while reduction takes place at cathode. The emf of cell is calculated by using nernst equation. It looks like your answer is nearly correct. Please check it By taking above value or we need to apply significant rule to E0.

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An electrochemical cell consists of a half-cell in which a piece of platinum wire is dipped into a solution that is 2.5 M in KI and 0.046 M in I2. The other half-cell consists of magnesium metal immersed in a 0.37 M Mg2+ solution. Assume that the temperature is 25°C. (a) Which electrode is the anode and which is the cathode? anode: O Pt|I2, I- O Mg2+|Mg cathode: O Pt|I2, I- O Mg2+|Mg

An electrochemical cell consists of a half-cell in which a piece of platinum wire is dipped into a solution that is 2.5 M in KI and 0.046 M in I2. The other half-cell consists of magnesium metal immersed in a 0.37 M Mg2+ solution. Assume that the temperature is 25°C. (a) Which electrode is the anode and which is the cathode? anode: O Pt|I2, I- O Mg2+|Mg cathode: O Pt|I2, I- O Mg2+|Mg

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

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An electrochemical cell consists of a half-cell in which a piece of platinum wire is dipped into a solution that is 2.5 M in KI and 0.046 M in I2. The other half-cell consists of magnesium
metal immersed in a 0.37 M Mg2+ solution. Assume that the temperature is 25°C.
(a) Which electrode is the anode and which is the cathode?
anode:
Pt|I2, I-
O Mg²+|Mg
cathode:
O Pt|I2, I-
Mg2+|Mg
(b) What is the emf of the cell?
4.0
2.869
X V
(c) What is the spontaneous cell reaction?
chemPad
OHelp
Greek -
Mg2+(aq)+21 (aq)
Mg(s)+I2(aq)
Mg(s)+l_2(aq)-->Mg^2+(aq)+2l^-(aq)
Your answer appears to have inconsistent states-of-matter.
(d) What is the equilibrium constant of the cell reaction?
2.42e98

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