Question

4NH3 (g) + 5O2 (g) → 4NO (g) + 6H2O (l) (a) How many moles of nitric oxide (NO) can be produced if 0.523 moles of NH3 were used and oxygen gas is in excess? (b) What is the theoretical mass of NO if 0.523 moles of NH3 were used and oxygen gas is in excess? (c) What is the percent yield of the reaction if the actual yield of NO was 6.625 g?

Name: 4nh3 g 5o2 g 4no g 6h2o l a how many moles of nitric oxide no can be produced if 0523 moles of nh3 was used and oxygen gas is in excess b what is the theoretical mass of no if 0523 moles of 84018
Uploaded: 2022-01-06T02:13:06-08:00
Duration: 4 min 18 s
Channel: Preeti Kumari
Description: 4nh3 g 5o2 g 4no g 6h2o l a how many moles of nitric oxide no can be produced if 0523 moles of nh3 was used and oxygen gas is in excess b what is the theoretical mass of no if 0523 moles of 84018

          4NH3 (g) + 5O2 (g) → 4NO (g) + 6H2O (l)

(a) How many moles of nitric oxide (NO) can be produced if 0.523 moles of NH3 were used and oxygen gas is in excess?
(b) What is the theoretical mass of NO if 0.523 moles of NH3 were used and oxygen gas is in excess?
(c) What is the percent yield of the reaction if the actual yield of NO was 6.625 g?

Added by Cody S.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

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Solved by Expert Preeti Kumari

01/06/2022

Step 1

523 moles From the balanced chemical equation, 4 moles of NH3 produce 4 moles of NO Therefore, 0.523 moles of NH3 will produce 0.523 moles of NO Show more…

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4NH3 (g) + 5O2 (g) → 4NO (g) + 6H2O (l) (a) How many moles of nitric oxide (NO) can be produced if 0.523 moles of NH3 were used and oxygen gas is in excess? (b) What is the theoretical mass of NO if 0.523 moles of NH3 were used and oxygen gas is in excess? (c) What is the percent yield of the reaction if the actual yield of NO was 6.625 g?