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One of the steps in the commercial process for converting ammonia to nitric acid is the conversion of NH3 to NO:
4NH3(g)+5O2(g)â4NO(g)+6H2O(g)
In a certain experiment, 1.25 g of NH3 reacts with 2.29 g of O2.
(I have already got Part A & B correct, but thought you may need the info. Just need Part C please)
Part A
Which is the limiting reactant? O2
NH3 O2
Correct
Part B
How many grams of NO and of H2O form?
Enter your answers numerically separated by a comma.
mNO,mH2O = 1.72,1.55
g
Correct
Part C
How many grams of the excess reactant remain after the limiting reactant is completely consumed?
Express your answer in grams to three significant figures.
One of the steps in the commercial process for converting ammonia to nitric acid is the conversion of NH3 to NO:
4NH3(g)+5O2(g)â4NO(g)+6H2O(g)
In a certain experiment, 1.25 g of NH3 reacts with 2.29 g of O2.
(I have already got Part A & B correct, but thought you may need the info. Just need Part C please)
Part A
Which is the limiting reactant? O2
| NH3 |
| O2 |
Correct
Part B
How many grams of NO and of H2O form?
Enter your answers numerically separated by a comma.
| mNO,mH2O = | 1.72,1.55 | g |
Correct
Part C
How many grams of the excess reactant remain after the limiting reactant is completely consumed?
Express your answer in grams to three significant figures.
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Collen VonLv2
17 Aug 2019
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