For given voltaic cell with given half cells, the [ Pb 2+ ] has to be calculated when [ Mn 2+ ] =1 .4 and E cell = 0 .44 V Concept Introduction: An electrochemical cell is a device in which a redox reaction is used to convert chemical energy into electrical energy. Such device is also known as the galvanic or voltaic cell. Galvanic cell consists of two half-cells. The redox reaction occurs in these half-cells. The half-cell in which the reduction reaction occurs is known as the reduction half-cell, whereas the half-cell in which the oxidation reaction occurs is known as the oxidation half-cell. Anode: The electrode where the oxidation occurs is called as an anode. It is a negatively charged electrode. Cathode: The electrode where reduction occurs is called as a cathode. It is a positively charged electrode. Oxidation: The gain of oxygen or the loss of hydrogen or the loss of an electron in a species during a redox reaction is called as oxidation. Reduction: The loss of oxygen or the gain of hydrogen or the gain of an electron in a species during a redox reaction is called as reduction. The Standard Gibb’s free energy change and the standard cell potential are related as followed: Δ ° G = -nFE ° cell n - Number of electrons involved per equivalent of the net redox reaction in the cell F - Faraday’s Constant (96500 C) E ° cell - Standard cell potential. The Nernst equation depicts the relationship between E c e l l and E o cell as follows, E cell =E o cell − 0.0592 V n log Q w h e r e , E cell = c e l l p o t e n t i a l E o cell = Standard c e l l p o t e n t i a l n = N o . o f e l e c t r o n s Q = Reaction Q u o t i e n t

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Chapter 21, Problem 21.69P

Interpretation Introduction

Interpretation:

For given voltaic cell with given half cells, the [Pb2+] has to be calculated when [Mn2+]=1.4 and Ecell= 0.44 V

Concept Introduction:

An electrochemical cell is a device in which a redox reaction is used to convert chemical energy into electrical energy. Such device is also known as the galvanic or voltaic cell.

Galvanic cell consists of two half-cells. The redox reaction occurs in these half-cells. The half-cell in which the reduction reaction occurs is known as the reduction half-cell, whereas the half-cell in which the oxidation reaction occurs is known as the oxidation half-cell.

Anode: The electrode where the oxidation occurs is called as an anode. It is a negatively charged electrode.

Cathode: The electrode where reduction occurs is called as a cathode. It is a positively charged electrode.

Oxidation: The gain of oxygen or the loss of hydrogen or the loss of an electron in a species during a redox reaction is called as oxidation.

Reduction: The loss of oxygen or the gain of hydrogen or the gain of an electron in a species during a redox reaction is called as reduction.

The Standard Gibb’s free energy change and the standard cell potential are related as followed:

Δ°G = -nFE°cell

n - Number of electrons involved per equivalent of the net redox reaction in the cell

F - Faraday’s Constant (96500 C)

E°cell - Standard cell potential.

The Nernst equation depicts the relationship between Ecell and Eocell as follows,

Ecell=Eocell−0.0592 Vnlog Qwhere, Ecell=cell potentialEocell= Standard cell potentialn= No. of electronsQ = Reaction Quotient

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