Question

Question in photo answer all don’t need to do the start pathway end math thing that’s a thing teacher added to help the student out. I just need an understanding on how to do this so I can do the other problems like this so pls be thorough.

Answer 1

a. The balanced chemical equation for the reaction is:

2 CuCl2(aq) + 4 KI(aq) → 2 CuI(s) + 4 KCl(aq) + b(g)

We need to determine how many moles of CuI are formed when 0.56 moles of CuCl2 and 0.64 moles of KI react. From the balanced chemical equation, we can see that the stoichiometric ratio of CuCl2 to CuI is 2:2, or 1:1. Therefore, the number of moles of CuI formed will be equal to the number of moles of CuCl2 used in the reaction, which is 0.56 moles.

b. To determine the limiting reactant, we need to compare the number of moles of each reactant to the stoichiometric ratio in the balanced chemical equation. The stoichiometric ratio of CuCl2 to KI is 2:4, or 1:2. Therefore, for every mole of CuCl2 used in the reaction, we need 2 moles of KI.

The number of moles of KI available is 0.64 moles, which is enough to react with 0.32 moles of CuCl2 (since the stoichiometric ratio is 1:2). However, we have 0.56 moles of CuCl2 available, which is more than enough to react with 1.12 moles of KI. Therefore, CuCl2 is in excess and KI is the limiting reactant.

c. Since KI is the limiting reactant, we can use the stoichiometry of the balanced chemical equation to determine how many moles of CuCl2 are used up in the reaction. The stoichiometric ratio of CuCl2 to KI is 2:4, or 1:2. Therefore, for every 2 moles of CuCl2 used, we need 4 moles of KI.

Since we have 0.64 moles of KI, this would require 0.32 moles of CuCl2. However, we have 0.56 moles of CuCl2 available, so 0.24 moles of CuCl2 will be left over at the end of the reaction.