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Problem: Nitric oxide (an older name for NO) is made from the oxidation of ammonia. What mass of nitric oxide (NO) can be made from the reaction of 8.00 g NH3 with 17.0 g O2?        4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O(g)a. 4.54 gb. 12.8 gc. 14.1 gd. 15.9 ge. 25.0 g 

FREE Expert Solution

We’re being asked to calculate the mass of nitric oxide, NO, that will be formed in the reaction of 8.00 g NH3 with 17.0 g O2. First, we need to find the chemical equation:

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


Since we have a balanced equation, we can determine how much NO is produced.


Notice that we are given the mass of both reactants: this means we need to determine the limiting reactant, which is the reactant that forms the less amount of product. This is because once the limiting reactant is all used up, the reaction can no longer proceed and make more products.


This means the limiting reactant determines the maximum mass of the product formed.


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Problem Details

Nitric oxide (an older name for NO) is made from the oxidation of ammonia. What mass of nitric oxide (NO) can be made from the reaction of 8.00 g NH3 with 17.0 g O2?

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

a. 4.54 g

b. 12.8 g

c. 14.1 g

d. 15.9 g

e. 25.0 g

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What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Limiting Reagent concept. If you need more Limiting Reagent practice, you can also practice Limiting Reagent practice problems.

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