The reaction below shows aqueous chromium $($II$)$ nitrate $(Cr(N{O}_3{)}_2)$ reacting with aqueous potassium phosphate $(K_{3}P{O}_4)$ to produce solid chromium $($II$)$ phosphate $(C{r}_3(P{O}_4{)}_2)$ and aqueous potassium nitrate $(KN{O}_3).$ If $46\mathrm{.}8g$ of chromium $($II$)$ nitrate $(Cr(N{O}_3{)}_2)$ is added to $44\mathrm{.}7g$ of potassium phosphate $(K_{3}P{O}_4),$ identify the limiting reactant and calculate the theoretical yield, in grams, of chromium $($II$)$ phosphate $(C{r}_3(P{O}_4{)}_2)?$

Reaction:

$3Cr(N{O}_3{)}_2(aq)+2K_{3}P{O}_4(aq)C{r}_3(P{O}_4{)}_2(s)+6KN{O}_3(aq)$

Given: Molar Masses $=Cr(N{O}_3{)}_2=176\mathrm{.}02$;$K_{3}P{O}_4=212\mathrm{.}27$;$C{r}_3(P{O}_4{)}_2=345\mathrm{.}94$;

Limiting Reactant $=K_{3}P{O}_4$; Theoretical Yield of $C{r}_3(P{O}_4{)}_2=30\mathrm{.}7g$

Limiting Reactant $=Cr(N{O}_3{)}_2$; Theoretical Yield of $C{r}_3(P{O}_4{)}_2=30\mathrm{.}7g$

Limiting Reactant $=Cr(N{O}_3{)}_2$; Theoretical Yield of $C{r}_3(P{O}_4{)}_2=36\mathrm{.}4g$

Limiting Reactant $=K_{3}P{O}_4$; Theoretical Yield of $C{r}_3(P{O}_4{)}_2=36\mathrm{.}4g$