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If pb + Cl2 → PbCl4rnrn266.2 grams of pb are reacted with 376.45 grams of Cl2, how many moles of PbCl4 will be produced?
Accepted Answer
From the balanced chemical equation:
Pb + 2Cl2 → PbCl4
1 mole of Pb reacts with 2 moles of Cl2 to produce 1 mole of PbCl4.
Converting the given masses to moles:
moles of Pb = 266.2 g / 207.2 g/mol = 1.285 mol
moles of Cl2 = 376.45 g / 70.906 g/mol = 5.309 mol
Determining the limiting reactant:
From the stoichiometry of the balanced equation, 1 mole of Pb reacts with 2 moles of Cl2. The mole ratio of Pb to Cl2 is 1:2.
Comparing the mole ratio to the actual mole ratio:
Actual mole ratio: 1.285 mol Pb / 5.309 mol Cl2 = 1:4.13
Since the actual mole ratio is different from the stoichiometric mole ratio, Cl2 is the limiting reactant because it will be completely consumed in the reaction.
Using the stoichiometry of the balanced equation and the moles of the limiting reactant (Cl2), we can calculate the moles of PbCl4 produced:
moles of PbCl4 = 5.309 mol Cl2 × (1 mol PbCl4 / 2 mol Cl2) = 2.654 mol
Therefore, 2.654 moles of PbCl4 will be produced.
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