Ammonia can be produced by the Haber process: ___ N2(g) + ___ H2(g) → ___ NH3(g) 11. Balance the equation. 12. When 25.0 g of nitrogen and 5.00 g of hydrogen are mixed, what is the theoretical yield of ammonia, in grams? 13. Which reactant is limiting and which is in excess? 14. How much (g) of each reactant is left over? 15. What is the percent yield of ammonia if 21.3 g are actually produced?
Ammonia can be produced by the Haber process: ___ N2(g) + ___ H2(g) → ___ NH3(g) 11. Balance the equation. 12. When 25.0 g of nitrogen and 5.00 g of hydrogen are mixed, what is the theoretical yield of ammonia, in grams? 13. Which reactant is limiting and which is in excess? 14. How much (g) of each reactant is left over? 15. What is the percent yield of ammonia if 21.3 g are actually produced?
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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Ammonia can be produced by the Haber process: ___ N2(g) + ___ H2(g) → ___ NH3(g)
11. Balance the equation.
12. When 25.0 g of nitrogen and 5.00 g of hydrogen are mixed, what is the theoretical yield of ammonia, in grams?
13. Which reactant is limiting and which is in excess?
14. How much (g) of each reactant is left over?
15. What is the percent yield of ammonia if 21.3 g are actually produced?
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