When aqueous solutions of silver nitrate and potassium dichromate are mixed, an exchange reaction occurs, and

silver dichromate is obtained as a red solid. The overall chemical equation for the reaction is as follows:

$2AgN{O}_3(aq)+K_{2}C{r}_2{O}_7(aq)A{g}_{2}C{r}_2{O}_7(s)+2KN{O}_3(aq)$

What mass of $A{g}_{2}C{r}_2{O}_7$ is formed when $500mL$ of $0\mathrm{.}17M{K}_{2}C{r}_2{O}_7$ are mixed with $250mL$ of $0\mathrm{.}57MAgN{O}_3?$

a$.$ What is the limiting reagent?

b$.$ How many moles of the excess reactant are left?

c$.$ What mass of $A{g}_{2}C{r}_2{O}_7$ is formed when $500mL$ of $0\mathrm{.}17M{K}_{2}C{r}_2{O}_7$ are mixed with $250mL$ of $0\mathrm{.}57MAgN{O}_3?$