Find the mass of a product

I have found the answer to this question and there is a another question exactly like this that I have to do but I got an incorrect answer. So I am wonder how did I do this right and why.

Determine the mass (in g) of Ag2CrO4 that is produced when 858 mL of a 7.63×10^-2 M K2CrO4 solution completely reacts with 359 mL of a 2.40×10^-2 M AgNO3 solution according to the following balanced chemical equation.

K2CrO4(aq) + 2AgNO3(aq) → Ag2CrO4(s) + 2KNO3(aq)

(0.858L)(7.63x10^-2M) = 0.065mols K2CrO4

(0.065mols)(178.189g/mol) = 11.6g K2CrO4
--------------------------------------…
(0.359L)(2.40x10^-2) = 0.0086mols AgNO3

( 0.0086mols)(169.872g/mol) = 1.46g AgNO3



1.46 is the correct answer for AgCrO4 but I have no idea why it is. I think that the math I did is irrelevant to finding the answer for AgCrO4. By luck i think that the mass of AgNO3 = the mass of AgCrO4

K2CrO4 + 2 AgNO3 → Ag2CrO4 + 2 KNO3

(858 mL) x (7.63×10^-2 M K2CrO4) = 0.065465 mol K2CrO4
(359 mL) x (2.40×10^-2 M AgNO3) = 0.0086160 mol AgNO3

0.0086160 mole of AgNO3 would react completely with 0.0086160 x (1/2) = 0.004308 mole of K2CrO4, but there is much more K2CrO4 present than that, so K2CrO4 is in excess and AgNO3 is the limiting reactant.

(0.0086160 mol AgNO3) x (1 mol Ag2CrO4/ 2 mol AgNO3) x
(331.73032 g Ag2CrO4/mol) = 1.43 g Ag2CrO4