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 a)Write the anode and cathode reactions when using the battery (i.e., it is the galvanic battery it generates electricity and discharge). b)Find battery potential and standard free energy. c)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 (DH °, DS °) at 298 K.
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
a)Write the anode and cathode reactions when using the battery (i.e., it is the galvanic battery it generates electricity and discharge).
b)Find battery potential and standard free energy.
c)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
d)An automobile’s headlights typically draw 6.1 amperes of current. A typical electrode contains about 260 g PbO2 . How long will it take for a battery to run down (until all the PbO2 has been consumed) if the lights are left on after the engine is turned off?
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