Consider the gaseous reaction at 347 C N2 + 3H2 ---> 2NH3 if 2.00 mole of N2 and 3.00 mole of H2 react, a) which of the two reactants is the limiting reagent b) if the reaction goes completely, how many grams of NH3 should be produced c) calculate the percent yield of 2.50 g of NH3 are actually obtained
Consider the gaseous reaction at 347 C N2 + 3H2 ---> 2NH3 if 2.00 mole of N2 and 3.00 mole of H2 react, a) which of the two reactants is the limiting reagent b) if the reaction goes completely, how many grams of NH3 should be produced c) calculate the percent yield of 2.50 g of NH3 are actually obtained
World of Chemistry, 3rd edition
3rd Edition
ISBN:9781133109655
Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste
Chapter9: Chemical Quantities
Section: Chapter Questions
Problem 30A
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Consider the gaseous reaction at 347 C
N2 + 3H2 ---> 2NH3
if 2.00 mole of N2 and 3.00 mole of H2 react,
a) which of the two reactants is the limiting reagent
b) if the reaction goes completely, how many grams of NH3 should be produced
c) calculate the percent yield of 2.50 g of NH3 are actually obtained
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