3H2(g)+N2(g)--->2NH3(g)
Given:
1.81 g H2 is allowed to react with 9.96 g N2, producing 1.13 g NH3.
1.)What is the theoretical yield for this reaction under the given conditions?
2.)What is the percent yield for this reaction under the given conditions?
Copyright © 2024 VQUIX.COM - All rights reserved.
Answers & Comments
Verified answer
moles N2 = 9.96 g / 28.0134 g/mol=0.356
moles H2 needed = 0.356 x 3 =1.07
actual moles H2 = 1.81 / 2.016 =0.898 => limiting reactant
theoretical moles NH3 = 0.898 x 2 /3=0.599
theoretical mass NH3 = 0.599 x 17.0307 g/mol=10.2 g
% = 1.13x 100/ 10.2 =11.1