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 a0.37 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+|Mgcathode:O Pt|I2, I-O Mg²+|Mg(b) What is the emf of the cell?4.0 2.869V(c) What is the spontaneous cell reaction?chemPadHelpGreek -|-563-563Your answer differs too much from the expected answer to provide useful feedback.(d) What is the equilibrium constant of the cell reaction?6.09e98

The standard reduction potential values are: Mg2+(aq) + 2e- ---> Mg(s) ; Eo = - 2.37 V I2(s) + 2e- -----> 2I-(aq) ; Eo = 0.54 V #(b): Since I2(s) has a higher reduction potential, Pt|I2, I- acts as cathode, whereas Mg2+|Mg acts as anode. The half-reactions are: Anode: Mg(s) ----> Mg2+(aq) + 2e- ; Eoanode = - 2.37 V Cathode: I2(aq) + 2e- ----> 2I-(aq) ; Eocathode = 0.54 V Since 2e- are transferred, n = 2 Standard emf, Eocell = Eocathode - Eoanode = 0.54 V - (-2.37V) = (0.54+2.37) V = 2.91 V EMF of the cell can be calculated using Nernst equation: Ecell = Eocell - 0.0591n*log[Mg2+(aq)]*[I-(aq)]2[I2(aq)]⇒Ecell =2.91V - 0.05912*log0.37*(2.5)20.046⇒Ecell =2.86 V EMF of the cell = 2.86 V (Answer)#(c): Spontaneous cell reaction can be found by adding the anode and cathode half-reactions. Anode: Mg(s) ----> Mg2+(aq) + 2e- + + Cathode: I2(aq) + 2e- ----> 2I-(aq) ------------------------------------------- Spontaneous cell reaction: Mg(s) + I2(aq) -----> Mg2+(aq) + 2I-(aq) (Answer) #(d): ∆Go = - n*F*Eocell => ∆Go = - 2*96485*2.91 = 561542.7 J Also, ∆Go = - RT*ln(K) => - 561542.7 J = - 8.314 * 298.15 * ln(K) => 561542.7 J = 8.314 * 298.15 * ln(K) ⇒ ln(K) = 561542.78.314 * 298.15⇒ln(K) = 226.5⇒ K = e226.5 = 2.42*1098 Equilibrium constant = 2.42*1098 (Answer)

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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|12, 1- O Mg2+|Mg cathode: O Pt|I2, I~ O Mg2+|Mg (b) What is the emf of the cell? 2.869 x V (c) What is the spontaneous cell reaction? chemPad O Help Greek |-563 -563 Your answer differs too much from the expected answer to provide useful feedback. (d) What is the equilibrium constant of the cell reaction? 6.09e98

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|12, 1- O Mg2+|Mg cathode: O Pt|I2, I~ O Mg2+|Mg (b) What is the emf of the cell? 2.869 x V (c) What is the spontaneous cell reaction? chemPad O Help Greek |-563 -563 Your answer differs too much from the expected answer to provide useful feedback. (d) What is the equilibrium constant of the cell reaction? 6.09e98

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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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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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
(b) What is the emf of the cell?
4.0 2.869
V
(c) What is the spontaneous cell reaction?
chemPad
Help
Greek -
|-563
-563
Your answer differs too much from the expected answer to provide useful feedback.
(d) What is the equilibrium constant of the cell reaction?
6.09e98

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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