Ammonia, NH3, may react with oxygen to form nitrogen gas and water.4NH3(aq)+302(g)→2N2(g)+6H2O(1)If 3.45 g NH3 reacts with 5.18g 02 and produces 0.950L N2 at 295 K and 1.00 bar, how many moles of N2N2 canbe produced by each reactant? It may be useful to consult the periodic table.mol N2NH3:02:mol N2Based on the theoretical yields, which reactant is limiting?NH3(aq)O2(g)What is the percent yield of the reaction?percent yield:

Recall the given reaction, 4 NH3 aq + 3 O2 g → 2 N2 g + 6 H2O l3.45 g…

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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

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Ammonia, NH3, may react with oxygen to form nitrogen gas and water.
4NH3(aq)+302(g)→2N2(g)+6H2O(1)
If 3.45 g NH3 reacts with 5.18g 02 and produces 0.950L N2 at 295 K and 1.00 bar, how many moles of N2N2 can
be produced by each reactant? It may be useful to consult the periodic table.
mol N2
NH3:
02:
mol N2
Based on the theoretical yields, which reactant is limiting?
NH3(aq)
O2(g)
What is the percent yield of the reaction?
percent yield:

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$Recall the given reaction, 4 {NH}_{3} (aq) + 3 O_{2} (g) \to 2 N_{2} (g) + 6 H_{2} O (l) 3.45 g {NH}_{3} reacts with 5.18 g O_{2} to produce 0.950 L N_{2} at 295 K and 1.00 bar . We have to determine - Moles of N_{2} produced by each reactant . Limiting reactant . Percent yield .$

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hi, sorry the typing is a little cramed together can you seperate the answers

NH₃ molN₂

O₂ molN₂

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