The batteries used in automobiles are rechargeable and consist of Pb and PbO2 anodes and cathodes respectively immersed in 6 M H2SO4 solution. Standard reduction potentials at 25°C are as follow: E°( PbSO4/Pb) = - 0.35 V and E°( PbO2/PbSO4) = 1.69 VIf temperature change of battery is given by the following equation:E(volt) = -0.096 + 1.9 x 10-3 T -3.04 x 10-6 T2 Calculate the equilibrium constant and the thermodynamic functions of the battery (H °, S °) at 298 K.

Calculation of E˚cell: Ecell of the reaction is given as: Calculation of temperature coefficient,…

Answered: The batteries used in automobiles are…

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 90AP: Consider a galvanic cell for which the anode reaction is 3 Pb(s)Pb2+(1.0102M)+2e and the cathode...

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The batteries used in automobiles are rechargeable and consist of Pb and PbO₂ anodes and cathodes respectively immersed in 6 M H₂SO₄ solution. Standard reduction potentials at 25°C are as follow: E°( PbSO₄/Pb) = - 0.35 V and E°( PbO₂/PbSO₄) = 1.69 V

If temperature change of battery is given by the following equation:

E(volt) = -0.096 + 1.9 x 10^-3 T -3.04 x 10-6 T²

Calculate the equilibrium constant and the thermodynamic functions of the battery (H °,

S °) at 298 K.

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