If 30.0 g of H2 were used, how many grams of NH3 would be made?
N2 + 3H2 ==> 2NH3
Convert 30.0 g H2 to moles.
Convert moles H2 to moles NH3.
Convert moles NH3 to grams.
Here is a link if you get stuck.
http://www.jiskha.com/science/chemistry/stoichiometry.html
10 mole of NH3
507 g; use proportions with value to find as the x thus on top. 34.088x30/2.016
To determine the number of grams of NH3 produced, we need to first establish the balanced chemical equation for the reaction between H2 and NH3. The balanced equation is as follows:
N2 + 3H2 -> 2NH3
From the equation, we can see that it takes 3 moles of H2 to produce 2 moles of NH3.
To find the amount of NH3 produced, we need to convert the given mass of H2 (30.0 g) to moles. To do this, we divide the mass of H2 by its molar mass. The molar mass of H2 is approximately 2.02 g/mol (1.01 g/mol for each hydrogen atom).
30.0 g H2 * (1 mol H2 / 2.02 g H2) ≈ 14.85 mol H2
Since the stoichiometry of the reaction tells us that 3 moles of H2 produce 2 moles of NH3, we can set up a mole-to-mole ratio:
14.85 mol H2 * (2 mol NH3 / 3 mol H2) ≈ 9.90 mol NH3
Finally, to convert moles of NH3 to grams, we multiply the number of moles by the molar mass of NH3. The molar mass of NH3 is approximately 17.03 g/mol (14.01 g/mol for nitrogen and 3.02 g/mol for each hydrogen atom).
9.90 mol NH3 * (17.03 g NH3 / 1 mol NH3) ≈ 168.57 g NH3
Therefore, approximately 168.57 grams of NH3 would be produced if 30.0 grams of H2 were used.