The addition of a hot (60 °C) solution of copper sulfate pentahydrate, CuSO4 · 5H₂0, to a hot (60 °C) solution of potassium oxalate monohydrate, K₂C₂O4. H₂O, yields blue crystals that have the following mass composition:

→ Determine the empirical formula and molar mass of the blue salt. (Show all work).nation*1²+5,0%+1+2 50²entireorbbunforestThe indide ion, Ipenene clestronrachng perplest example offormalaToten carbonBalance the following equation, use the empirical formula of the blue salt that youdetermined.The peroxodsplit betweenand the \mathrm{CuSO}_{4} \cdot 5 \mathrm{H}_{2} \mathrm{O}+\mathrm{K}_{2} \mathrm{C}_{2} \mathrm{O}_{4} \cdot \mathrm{H}_{2} \mathrm{O} \rightarrow \mathrm{K}_{\mathrm{a}} \mathrm{Cu}_{\mathrm{b}}\left(\mathrm{C}_{2} \mathrm{O}_{4}\right)_{\mathrm{c}} \cdot \mathrm{dH}_{2} \mathrm{O}+\mathrm{SO}_{4}^{2-}+\mathrm{K}^{1+}+\mathrm{H}_{2} \mathrm{O} Calculate the theoretical yield of the blue salt given that 5.0 grams of CuSO4.5H₂0 and 7.8 grams of K₂C₂O4 H₂O are used in the synthesis. Show the moles of each reactant, which is the limiting reagent, and calculate the theoretical yield