For the following reaction, if the reaction uses 5.75g of Mg, what is the theoretical yield (in grams) of MgCl2? (molar mass of Mg = 24.305 g/mol, Molar mass of MgCl2 = 95.211 g/mol)
2HCl(aq) + Mg(s) -> MgCl2(s) + H2(g)
a. 24.3 g
b. 5.75 g
c. 22.5 g
d. 95.2 g

Ais stronge

The correct answer is "false"

Ithink that’s it’s b

Answerthe half-reaction having the greatest tendency to occur at the anode:     i₂(aq) + 2e⁻  ⇄ 2i⁻  ;   e = +0.53 v======oxidation occurs at the anode. we must therefore find the half-reaction with the greatest tendency to oxidize.the given values of e are reduction potentials (the form of the half-reactions are of reduction).the lower the reduction potential, the higher the potential to oxidize. the half-cell with the lowest reduction potential will have the greatest tendency to oxidize at the anode.the half-reaction having the greatest tendency must be    i₂(aq) + 2e⁻  ⇄ 2i⁻    e = +0.53 vbecause its reduction potential is the lowest out of the three.