Answer to Question #184995 in Inorganic Chemistry for kyle

Question #184995

A reaction to convert ammonia into nitric acid involves following chemical

equation:

4 NH3 (g) + 5 O2 (g)à 4 NO(g) + 6 H2O(g)

Assume that 1.50 g of NH3 reacts with 2.75 g O2, then:


1. Calculate how many grams of the excess reactant will remain after the

reaction is complete.


2. If the yield obtained for NO is 1.80 grams and yield obtained for H2O is 1.50

grams, calculate the percent yield of NO and H2O in this reaction.

(Atomic mass of N = 14 ; O = 16 ; H = 1).


1
Expert's answer
2021-04-25T03:48:44-0400

Moles of Ammonia =


Moles of Oxygen




Mass of excess reactant that remain =



Moles of NO


Moles of H2O=



Need a fast expert's response?

Submit order

and get a quick answer at the best price

for any assignment or question with DETAILED EXPLANATIONS!

Comments

No comments. Be the first!

Leave a comment

Ask Your question

LATEST TUTORIALS
New on Blog
APPROVED BY CLIENTS