N2 + 3H2 --> 2NH3
how many grams of ammonia is produced in the reaction?
It depends upon how much N2 and H2 are reacted.
If you have 0.230 moles of nitrogen, how much ammonia can be produced with an excess of hydrogen?
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To determine the grams of ammonia produced in the reaction, we need to use stoichiometry, which relates the ratio of reactants and products in a chemical equation.
Step 1: Balance the equation:
The balanced chemical equation is:
N2 + 3H2 → 2NH3
Step 2: Determine the molar masses:
N2 = 28.0134 g/mol
H2 = 2.0159 g/mol
NH3 = 17.0305 g/mol
Step 3: Use stoichiometry to find the grams of ammonia produced:
According to the balanced equation, 1 mole of N2 reacts with 3 moles of H2 to produce 2 moles of NH3.
Let's assume we have "x" grams of N2. We need to find the grams of ammonia produced, so we can set up a proportion:
(x g N2) / (28.0134 g/mol N2) = (y g NH3) / (17.0305 g/mol NH3)
Using the molar ratios from the balanced equation, we know that:
1 mole of N2 = 2 moles of NH3
So, the molar ratio between N2 and NH3 is 1:2.
Therefore, we can set up the proportion as follows:
(x g N2) / (28.0134 g/mol N2) = (y g NH3) / (17.0305 g/mol NH3) = (2 mol NH3) / (1 mol N2)
Now, solve for y (grams of NH3):
y = (x g N2) * (17.0305 g/mol NH3) / (28.0134 g/mol N2)
Substitute the given values and calculate the result.