Calculating Mass Quick Check 5 of 55 of 5 Items Question 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 550.5 g 550.5 g 496.5 g 496.5 g 853.5 g 853.5 g 702.0 g

Answer 1

To calculate the total mass of the products, we need to first calculate the molar mass of Pb(NO3)2, which is 331 g/mol.

Next, we need to determine the moles of Pb(NO3)2 present in 496.5 grams:
496.5 g Pb(NO3)2 x (1 mol Pb(NO3)2 / 331 g Pb(NO3)2) = 1.5 mol Pb(NO3)2

According to the balanced chemical equation, 1 mole of Pb(NO3)2 reacts with 2 moles of KBr to produce 1 mole of PbBr2. Therefore, 1.5 moles of Pb(NO3)2 will produce 0.75 moles of PbBr2.

Now, calculate the molar mass of PbBr2, which is 367 g/mol.
0.75 mol PbBr2 x 367 g/mol PbBr2 = 275.25 g PbBr2

Finally, calculate the total mass of the products:
Total mass = mass of PbBr2 + mass of KNO3
Total mass = 275.25 g + 2(101 g) = 275.25 g + 202 g = 477.25 g

Therefore, the total mass of the products when 496.5 grams of Pb(NO3)2 reacts completely with KBr will be approximately 477.25 grams.

The closest response option is 496.5 g.