Silver iodide is a photosensitive material used in photography. One method of forming silver iodide is the reaction between magnesium iodide and silver nitrate in solution. 6. Assume aqueous solutions of Magnesium Iodide and Silver Nitrate are the starting substances (reactants) in the reaction. a. Write a balanced molecular chemical equation describing the formation of Silver Iodide. Include phase labels. b. State the name and formula of the other product in this reaction. c. Write complete ionic and net ionic reactions based on the balanced equation in part (a). Please include phase labels. d. What type of reaction(s) is/are being represented by the chemical reaction in part (a)? e. Based on your answers to parts (a) - (d), determine if a solid precipitate is formed in this reaction. If yes, state its chemical formula. f. If 0.35 g of magnesium iodide and 1.58 g of silver nitrate are combined, then what is the limiting reactant? Theoretically what mass of the solid product could form from these amounts of reactants? g. What is the percent yield if 0.199 g of the solid product was actually obtained in lab? h. How many atoms are in 0.887 g of magnesium iodide?