Use the chemical equation and the table to answer the question. Pb(NO3)2(aq) + 2KBr(aq) → PbBr2(s) + 2KNO3(aq) Reactant or Product Molar Mass (g/mol) Pb(NO3)2 331 KBr 119 PbBr2 367 KNO3 101 When 496.5 grams of Pb(NO3)2 reacts completely with KBr, how much will the total mass of the products be? (1 point) Responses 496.5 g 496.5 g 550.5 g 550.5 g 702.0 g 702.0 g 853.5 g
To find the total mass of the products, we need to calculate the molar mass of each product and then use the stoichiometry of the reaction to determine the mass of each product.
1. Calculate the molar mass of PbBr2:
2 mol of Br = 2(79.904 g/mol) = 159.808 g
1 mol of Pb = 207.2 g
159.808 g + 207.2 g = 367.008 g
2. Calculate the mass of PbBr2 produced when 496.5 g of Pb(NO3)2 reacts completely:
496.5 g Pb(NO3)2 * (1 mol Pb(NO3)2 / 331 g Pb(NO3)2) * (1 mol PbBr2 / 1 mol Pb(NO3)2) * (367.008 g PbBr2 / 1 mol PbBr2) = 560.493 g PbBr2
3. Calculate the total mass of the products:
560.493 g PbBr2 + 496.5 g KNO3 = 1056.993 g
Therefore, the total mass of the products will be 1056.993 grams. The closest answer choice is 1106.5 g.