Answer to Question #211093 in Inorganic Chemistry for Siti

Question #211093

A reaction to convert ammonia into nitric acid involves the following chemical equation: 

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

 Assume that 1.50 g of NH3 reacts with 2.75 g O2. 

i. Determine the limiting reactant.

ii. Calculate how many grams of NO and H2O will form in the reaction above.

iii. Calculate how many grams of the excess reactant will remain after the reaction is complete. 

iv. 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)

Expert's answer

Moles of Ammonia = 

Moles of Oxygen

Mass of excess reactant that remain = 

Moles of NO 

Moles of H2O=

Limiting reactants is NH3

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!


No comments. Be the first!

Leave a comment

Ask Your question

New on Blog