Use the Standard Reaction Potentials as a sorce of half-reaction equations and E^o values for the following reaction, and use them to answer part a) and b).
Mg^2+ + 2 e- -->Mg E^o = -2.37V
Al^3+ + 3 e - --> Al E^o = - 1.66V

Solid Mg reacts with a solution containing aluminum ions , forming a solution that contains magnesium ions and solid Al. Write the balanced net equation:

Then the sum half reactions:

a) calculate E^o for the reaction as written
b) State and breifly justify the favored direction of the reaction based on Gibbs Free Energy. Faraday Constant F= 96485 J/Volt•mol e-

a) E°=3*2.37 -2*1.66 = 3.79 V

b) the favored direction is 3Mg +2Al^(3+) > 3Mg^(2+) + 2Al

Explanation:

3Mg + 2Al^(3+) ---> 3Mg^(2+) + 2Al

a)

Mg                ---> Mg^(2+) + 2e-  , E°= +2.37V     /*3

Al^(3+) + 3 e - --> Al                     , E° = - 1.66V  /*2

3Mg +2Al^(3+) > 3Mg^(2+) + 2Al ,     E°=3*2.37 -2*1.66 = 3.79 Volt

b)  ΔG°= − nFE° = - 6 mol e-*96485 J/Volt*mol e- * 3.79Volt  < 0,

so the favored direction is 3Mg +2Al^(3+) > 3Mg^(2+) + 2Al

6.4 cm (max) - 25 cm (min)

the correct answer is b. a strong acid completely dissociates to its ions when dissolved in water. completely dissociates to and ions. a is incorrect because does not fully ionize to and ions and some remain as the compound . c and d are incorrect because, and do not fall into the category of bronsted lowry acids. a bronsted lowry acid is a proton donor and since both molecules do not have a proton to donate they are not bronsted lowry acids. likewise,   if we use the lewis acid definition, they cannot be acids. a lewis acid is an electron pair acceptor. both and have a complete octet so can not accept any electrons which disqualifies them as acids.