Question 14 One of the steps in the commercial process for converting ammonia to nitric acid is...

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Chemistry

Question 14
One of the steps in the commercial process for convertingammonia to nitric acid is the conversion of NH3 to NO:

4NH3(g)+5O2(g)â†’4NO(g)+6H2O(g)

In a certain experiment, 2.10 g of NH3 reacts with 3.85 g ofO2.
Part B
How many grams of NO and of H2O form?
Enter your answers numerically separated by a comma.
mNO,mH2O =
g
Part C
How many grams of the excess reactant remain after the limitingreactant is completely consumed?
m =

Answer & Explanation Solved by verified expert

3.7 Ratings (588 Votes)

Let is first calculate the number of moles of NH3 and moles of O2 used in the reaction The molar mass of NH3 and O2 are 15 gmol and 32 gmol respectively The number of moles of NH3 Weight of NH3 molar mass NH3 210 g 15 gmol 014 moles The number of moles of O2 Weight of O2 molar mass of O2 385 g 32 gmol 012 mol From the balanced chemical equation it is clear that 4 mole of NH3 requires 5 moles of O2 Therefore the ideal ratio of number of moles See Answer

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