Silver is reacted with excess mercury (II) chloride, producing a solid silver chloride precipitate. If the actual yield of 25.5 g silver chloride represents a 77% yield, how much silver was initially present?
Ag (s) + HgCl2 (aq) ——> AgCl (s) + Hg (l)
I already balanced the equation:
2 Ag + HgCl2 ——-> 2 AgCl + Hg
I am just so confused on how to solve this! What I know for sure is that the percent yield is actual yield/theoretical yield * (100), but I am not sure if that formula even matters in this question. I would love to learn though!