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In a certain experiment, 1.50 g of NH3 reacts with 2.75 g of O2. One of the steps in the commercial process for converting ammonia to nitric acid is the conversion of NH3 to NO:

 

How many grams of the excess reactant remain after the limiting reactant is completely consumed?

How many grams of NO and of H2O form?

Enter your answers numerically separated by a comma.

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Kenneth Duque
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Related questions

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)→4NO(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:

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

In a certain experiment, 2.00 g of NH3 reacts with 2.50 g of O2. (a) Which is the limiting reactant? (b) How many grams of NO and H2O form? (c) How many grams of the excess reactant remain after the limiting reactant is completely consumed? (d) Show that your calculations i parts (b) and (c) are consistent with the law of conservation of mass.

one step in the commercial process for the converting ammonia to nitric acid is the conversion of NH3 to NO:

NH3(g) + O2(g) -------------} NO(g) + H2O(g)

In certain experiment 2.00 g of NH3 reacts with 2.50 g of O2. (a)Is the reaction equation balanced? (If not, balanced it).(b) What is the limiting reactant? (c)How many grams of NO and H2O form?

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