Consider the formation of lithium nitride from lithium and nitrogen: 6 Li + N2 → 2 Li3N How much Li (molar mass: 6.94 g/mol) is needed to produce 2.00 kg Li3N (molar mass: 34.83 g/mol) if the percent yield of the process is 70.5%? a.sp.843 kg Li b.0.188 kg Li c.0.565 kg Li d.1.70 kg Li

Consider the formation of lithium nitride from lithium and nitrogen: 6 Li + N2 → 2 Li3N How much Li (molar mass: 6.94 g/mol) is needed to produce 2.00 kg Li3N (molar mass: 34.83 g/mol) if the percent yield of the process is 70.5%? a.sp.843 kg Li b.0.188 kg Li c.0.565 kg Li d.1.70 kg Li

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter3: Stoichiometry

Section: Chapter Questions

Problem 7RQ: Consider the hypothetical reaction between A2 and AB pictured below. What is the balanced equation?...

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Concept explainers

Stoichiometry

Stoichiometry is a chemical division that evaluates the quantitative content of the chemical process with the help of the reacting molecules or products taking part in the reaction. The term “stoicheion” in “Stoichiometry”, is an old Greek term for "element" whereas “metron” means "measure".

Question

answer.....

Consider the formation of lithium nitride from lithium and nitrogen:
6 Li + N2 → 2 LI3N
How much Li (molar mass: 6.94 g/mol) is needed to produce 2.00 kg Li3N (molar mass: 34.83 g/mol) if
the percent yield of the process is 70.5%?
a.sp.843 kg Li
b.0.188 kg Li
c.0.565 kg Li
d.1.70 kg Li

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