100 g manganese dioxide reacts with 300g hydrochloric acid in the reaction shown bellow. MnO2 + 4 HCl -> 2 H2O + Cl2 use the following molar masses: MnO2 = 86.9g HCl = 36.5g MnCl2= 125.8g H2O= 18.02g Cl2= 70.9g 1.) Which reactant is limiting? 2) Which reactant is excess? 3) What is the theoretical yield of Cl2?
100 g manganese dioxide reacts with 300g hydrochloric acid in the reaction shown bellow. MnO2 + 4 HCl -> 2 H2O + Cl2 use the following molar masses: MnO2 = 86.9g HCl = 36.5g MnCl2= 125.8g H2O= 18.02g Cl2= 70.9g 1.) Which reactant is limiting? 2) Which reactant is excess? 3) What is the theoretical yield of Cl2?
Introductory Chemistry: A Foundation
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Author:Steven S. Zumdahl, Donald J. DeCoste
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Chapter9: Chemical Quantities
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Problem 12CR: What is meant by a limiting reactant in a particular reaction? In what way is the reaction...
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100 g manganese dioxide reacts with 300g hydrochloric acid in the reaction shown bellow.
MnO2 + 4 HCl -> 2 H2O + Cl2
use the following molar masses:
MnO2 = 86.9g
HCl = 36.5g
MnCl2= 125.8g
H2O= 18.02g
Cl2= 70.9g
1.) Which reactant is limiting?
2) Which reactant is excess?
3) What is the theoretical yield of Cl2?
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