Balance redox reaction calculator an electrochemical cell has the following standard cell notation: al(s) | al3+(aq) || mg2+(aq) | mg(s) a. write the balanced oxidation and reduction half-reactions, labeling the oxidation reaction and reduction reaction. (4 points) standard cell notation

Al(s) ⇄ Al³⁺(aq) + 3e⁻  (oxidation)

Mg⁺²(aq) + 2e⁻ ⇄ Mg(s) (reduction)

Explanation:

In the cell notation, first is placed the anode and then the cathode, so Al(s) is in the anode, where an oxidation reaction is taking place, and Mg²⁺ is in the cathode, where a reduction reaction is taking place. The half-reactions are:

Al(s) ⇄ Al³⁺(aq) + 3e⁻  (oxidation)

Mg⁺²(aq) + 2e⁻ ⇄ Mg(s) (reduction)

For the global reaction, it'll be necessary that the number of electrons (e⁻) is equal in the half-reactions, so the first one is multiplied by 2 and the second by three and the global reaction is:

2Al(s) + 3Mg⁺²(aq) ⇄ 2Al³⁺(aq) + 3Mg(s)

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.