1. I am doing step number 9 to determine the limiting reactant for this lab. http://www.lahc.edu/classes/chemistry/arias/Exp 4 - Limiting RF11.pdf Basically I have two vials labeled A and B filled with filtrate that is yellow. For vial A, I added 10 drops of 0.2 M K2CrO4, but nothing happened. The color stayed the same. For vial B, I added 10 drops of 0.1 M AgNO3, and the whole thing turned red. I am thinking since AgNO3 made the filtrate turn red then it is the limiting reactant, but I am not sure. Can somebody help me? Furthermore, when I do the math the grams of AgNO3 is always bigger than K2CrO4. I am wondering if it is possible for the limiting reactant to weigh more (in grams) than the excess reactant? 2. Relevant equations 3. Finding the weight of the limiting and excess reactant: The precipitate (Ag2CrO4) that forms weights 0.193 g and the moles are 5.82 x 10^-4 mol. Finding for mass for AgNO3: (5.82 x 10^-4 mol Ag2CrO4) (2 mol AgNO3 / 1 mol Ag2CrO4) (169.872 g AgNO3 / 1 mol AgNO3) = 0.198 g AgNO3 Finding for mass for K2CrO4: (5.82 x 10^-4 mol Ag2CrO4) (1 mol K2CrO4 / 1 mol Ag2CrO4) (194.188 g K2CrO4 / 1 mol K2CrO4) = 0.113 g K2CrO4 AgNO3 always comes out bigger than K2CrO4. So is it possible for AgNO3 to be the limiting reactant?