theoretical yield of nitrogen trihydride
The theoretical yield of a reaction is the maximum amount of product that can be produced from the given amount of reactants, assuming complete conversion and no side reactions.
Nitrogen trihydride, also known as ammonia (NH3), can be obtained by the reaction of nitrogen gas (N2) with hydrogen gas (H2) according to the following balanced equation:
N2 + 3H2 → 2NH3
From the equation, it is clear that one mole of nitrogen gas reacts with three moles of hydrogen gas to produce two moles of ammonia.
To calculate the theoretical yield of ammonia (NH3), you need to know the amount of nitrogen gas (N2) or hydrogen gas (H2) present. Let's assume we have one mole of nitrogen gas (N2).
Using the mole ratio from the balanced equation, we can determine the moles of hydrogen gas required:
1 mole of N2 → 3 moles of H2
Therefore, if we have one mole of N2, we will require three moles of H2.
Now, using the mole ratio from the balanced equation, we can determine the moles of ammonia produced:
1 mole of N2 → 2 moles of NH3
Therefore, if we have one mole of N2, we will produce two moles of NH3.
To calculate the theoretical yield of NH3, we can use the following steps:
1. Determine the moles of N2: Given that we have one mole of N2.
2. Determine the moles of H2 required: Using the mole ratio, since one mole of N2 requires three moles of H2, we will need three moles of H2.
3. Determine the moles of NH3 produced: Using the mole ratio, since one mole of N2 produces two moles of NH3, we will produce two moles of NH3.
4. Determine the mass of NH3 produced: Multiply the moles of NH3 by its molar mass, which is the sum of the molar masses of nitrogen (N) and hydrogen (H): molar mass of NH3 = (14.01 g/mol) + (3 × 1.01 g/mol) = 17.03 g/mol. Therefore, the theoretical yield of NH3 would be (2 moles) × (17.03 g/mol) = 34.06 g.
Hence, the theoretical yield of nitrogen trihydride (NH3) would be 34.06 grams.