Nitric oxide is made from the oxidation of ammonia. What mass of nitric oxide can be made from the reaction of 8.00 g NH 3 with 17.0 g O 2? 4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O(g)

The mass of nitric oxide is 12.72 grams

Explanation:

To calculate the number of moles, we use the equation:

    .....(1)

Given mass of ammonia = 8.00 g

Molar mass of ammonia = 17 g/mol

Putting values in equation 1, we get:

Given mass of oxygen gas = 17.0 g

Molar mass of oxygen gas = 32 g/mol

Putting values in equation 1, we get:

The given chemical reaction follows:

By Stoichiometry of the reaction:

5 moles of oxygen gas reacts with 4 moles of ammonia

So, 0.53 moles of oxygen gas will react with = of ammonia

As, given amount of ammonia is more than the required amount. So, it is considered as an excess reagent.

Thus, oxygen gas is considered as a limiting reagent because it limits the formation of product.

By Stoichiometry of the reaction:

5 moles of oxygen gas produces 4 moles of NO

So, 0.53 moles of oxygen gas will produce = of NO

Now, calculating the mass of NO from equation 1, we get:

Molar mass of NO = 30 g/mol

Moles of NO = 0.424 moles

Putting values in equation 1, we get:

Hence, the mass of nitric oxide is 12.72 grams

1 is the answer to this problem