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Problem: 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, 1.65 g of NH3 reacts with 3.02 g of O2. How many grams of NO and of H2O form?

FREE Expert Solution

The balanced reaction is:

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

From the reaction:

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Problem Details

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, 1.65 g of NH3 reacts with 3.02 g of O2. How many grams of NO and of H2O form?

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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.