# 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?

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

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