How many moles of NH3 are produced from 48.5 g of H2?

Just follow the steps. This will solve all of your stoichiometry problems.

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To determine the number of moles of NH3 produced from 48.5 g of H2, you need to follow these steps:

1. Write a balanced chemical equation for the reaction that produces NH3 from H2. In this case, it is the following reaction:
N2 + 3H2 --> 2NH3

2. Find the molar mass of H2. Hydrogen has an atomic mass of 1 g/mol, and since H2 is a diatomic molecule, the molar mass of H2 is 2 g/mol.

3. Convert the given mass of H2 (48.5 g) to moles. Use the formula:
Moles = Mass / Molar mass

Therefore, Moles of H2 = 48.5 g / 2 g/mol = 24.25 mol

4. Use stoichiometry to relate the moles of H2 to the moles of NH3 using the balanced equation from step 1. From the equation, we can see that 3 moles of H2 produce 2 moles of NH3.

Therefore, Moles of NH3 = (Moles of H2) * (2 moles of NH3 / 3 moles of H2)

Substituting the value, Moles of NH3 = 24.25 mol * (2/3) = 16.17 mol

So, from 48.5 g of H2, approximately 16.17 moles of NH3 are produced.