3. Given the following equation: underline ( )K_(2)PtCl_(4)+underline ( )NH_(3) arrow underline (2)Pt(NH_(3))_(2)Cl_(2)+underline ( )KCl a) Determine the theoretical yield of KCU you start with 34.5 grams of NH3 Answer: __ b) Starting with 64.5g of NH3 and you actually obtain 86.4gof Pt(NH_(3))_(2)Cl_(2) what is the percent yield __

a) To determine the theoretical yield of KCl, we first need to balance the chemical equation. The balanced equation is: From the balanced equation, we can see that 2 moles of NH3 produce 2 moles of KCl. The molar mass of NH3 is 17.03 g/mol, and the molar mass of KCl is 74.55 g/mol.First, we calculate the moles of NH3: Since the reaction is 1:1, the moles of KCl produced will be the same as the moles of NH3 used. Now we calculate the mass of KCl produced: So, the theoretical yield of KCl is 151.5 grams.b) To calculate the percent yield, we use the formula: The theoretical yield of \( Pt(NH_3)_2Cl_2 \) can be calculated using the stoichiometry of the reaction. From the balanced equation, 2 moles of NH3 produce 2 moles of \( Pt(NH_3)_2Cl_2 \). The molar mass of \( Pt(NH_3)_2Cl_2 \) is 237.73 g/mol.First, we calculate the moles of \( Pt(NH_3)_2Cl_2 \) produced: Now we calculate the theoretical yield of \( Pt(NH_3)_2Cl_2 \): Now we can calculate the percent yield: