Use the tabulated half-cell potentials to calculate Delta G degree for the follo

Question

Use the tabulated half-cell potentials to calculate Delta G degree for the following redox reactions. 2 AI(s) + 3 mg^2+(aq) reversiblearrow 2 Al^3+(aq) + 3 Mg(s) -7.8 times 10^2 kJ +6.8 times 10^2 kJ +4.1 times 10^2 kJ +1.4 times 10^2 kJ -2.3 times 10^2 kJ Given that E degree _red = -0.40 V for Cd^2+/Cd at 25 degree C, find E degee and E for the concentration cell expressed using shorthand notation below. Cd(s) | cd^2+(1.0 times 10^-5 M)| | Cd^2+ (0.100 m)| Cd(s) E degree cell = -0.40 V and E_cell = 0.16 V E degree cell = -0.40 V and E_cell = 0.28 V E degree cell = 0.00 V and E_cell = +0.12 V E degree cell = 0.40 V and E_cell = +0.24 V E degree cell = -0.00 V and E_cell = + 0.24 V How long would a constant current of 4.5 amperes be required to flow in order to plate out 45 g of chromium from a chromium(II) sulfate solution? 23.2 hr 1.72 hr 309 hr 268 hr 5.15 hr

Explanation / Answer

15)

Eo(Al3+|Al) = -1.662 V
Eo (Mg2+|Mg) = -2.372 V

Eo cell = Eo (Mg2+|Mg) - Eo(Al3+|Al)
= -2.372 - (-1.662)
= -0.71 V

n = 6 since 6 electrons are being transferred

use:
G = -n*F*Eo
= -6*96500*(-0.71)
= 411,090 J
= 4.11*10^2 KJ
Answer: C

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