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Answer :
Final answer:
To find the mass of PbI2 produced from the reaction of 1.70 g of Pb(NO3)2 with 3.40 g of KI, a stoichiometric calculation is performed according to the balanced chemical equation. The molar masses are used to calculate the moles of each reactant, identify the limiting reactant, calculate the moles of PbI2 produced, and then convert this to grams.
Explanation:
To determine how many grams of PbI2 will be produced from the reaction of 1.70 g of Pb(NO3)2 with 3.40 g of KI, we have to perform stoichiometric calculations based on the balanced chemical equation:
Pb(NO3)2 (aq) + 2 KI (aq)
arr PbI2 (s) + 2 KNO3 (aq)
First, we need to calculate the moles of Pb(NO3)2 and KI using their respective molar masses. Then, using the stoichiometry of the balanced equation, we determine which reactant is the limiting reactant. The reaction shows that 1 mole of Pb(NO3)2 reacts with 2 moles of KI to produce 1 mole of PbI2.
Once we identify the limiting reactant, we can calculate the theoretical yield of PbI2 in moles and subsequently convert this to grams using the molar mass of PbI2. In this scenario, as the reaction produces a brilliant yellow precipitate of PbI2, we expect the calculated mass of PbI2 to be the mass of product formed from the reaction.
The strong attractive forces between Pb2+ and I- ions result in the formation of this insoluble compound, and it is the only precipitate that forms in this reaction since potassium nitrate remains soluble.
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