3Cl2 + 2N2N2 → 2N2Cl3N2Cl3 Molar masses: chlorine gas = 70.9 g/mol nitrogen gas = 28.02 g/mol dinitrogen trichloride = 134.27 g/mol a. 1.98 mol of chlorine reacts with 1.98 moles of nitrogen. What is the limiting reactant? (chlorine) b. What mass of dinitrogen trichloride is produced from the reaction? (177.2364) c. How many moles of the excess reactant is left over? (0.66) d. If the percent yield of dinitrogen trichloride is 95.5%, what is the actual yield of the product? (169.2607)
3Cl2 + 2N2N2 → 2N2Cl3N2Cl3 Molar masses: chlorine gas = 70.9 g/mol nitrogen gas = 28.02 g/mol dinitrogen trichloride = 134.27 g/mol a. 1.98 mol of chlorine reacts with 1.98 moles of nitrogen. What is the limiting reactant? (chlorine) b. What mass of dinitrogen trichloride is produced from the reaction? (177.2364) c. How many moles of the excess reactant is left over? (0.66) d. If the percent yield of dinitrogen trichloride is 95.5%, what is the actual yield of the product? (169.2607)
Chapter3: Stoichiometry
Section: Chapter Questions
Problem 124E: DDT, an insecticide harmful to fish, birds, and humans, is produced by the following reaction: In a...
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3Cl2 + 2N2N2 → 2N2Cl3N2Cl3
Molar masses:
chlorine gas = 70.9 g/mol
nitrogen gas = 28.02 g/mol
dinitrogen trichloride = 134.27 g/mol
a. 1.98 mol of chlorine reacts with 1.98 moles of nitrogen. What is the limiting reactant? (chlorine)
b. What mass of dinitrogen trichloride is produced from the reaction? (177.2364)
c. How many moles of the excess reactant is left over? (0.66)
d. If the percent yield of dinitrogen trichloride is 95.5%, what is the actual yield of the product? (169.2607)
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