How many grams of H2 are needed to react with 2.50 g of N2?
Exoress vour answer with the appropriate units
To determine the amount of H2 needed to react with 2.50 g of N2, we need to first write and balance the chemical equation for the reaction.
The balanced equation for the reaction between H2 and N2 is:
N2 + 3H2 -> 2NH3
From the balanced equation, we can see that 1 mole of N2 reacts with 3 moles of H2.
To calculate the amount of H2 required, we can use the molar mass of N2 and H2:
Molar mass of N2 = 28.0134 g/mol
Molar mass of H2 = 2.01588 g/mol
First, let's convert the mass of N2 to moles:
2.50 g of N2 * (1 mol N2 / 28.0134 g N2) = 0.08925 mol N2
Since the balanced equation tells us that 1 mole of N2 reacts with 3 moles of H2, we can set up a ratio:
0.08925 mol N2 * (3 mol H2 / 1 mol N2) = 0.26775 mol H2
Finally, we can convert moles of H2 to grams:
0.26775 mol H2 * (2.01588 g H2 / 1 mol H2) = 0.539 g H2
So, 0.539 grams of H2 are needed to react with 2.50 grams of N2.
To answer this question, we need to know the balanced chemical equation for the reaction between H2 and N2. Assuming the reaction is as follows:
N2 + 3H2 → 2NH3
From the equation, we can see that one mole of N2 reacts with three moles of H2 to produce 2 moles of NH3.
First, we need to convert the mass of N2 given (2.50 g) into moles. We can do this by dividing the mass by the molar mass of N2, which is approximately 28 g/mol.
2.50 g N2 * (1 mol N2 / 28 g N2) = 0.0893 mol N2
Next, we determine the mole ratio between N2 and H2 from the balanced equation. From the equation, we can see that the ratio is 1:3 between N2 and H2.
Therefore, we can calculate the number of moles of H2 required:
0.0893 mol N2 * (3 mol H2 / 1 mol N2) = 0.268 mol H2
Finally, we convert the moles of H2 to grams:
0.268 mol H2 * (2 g H2 / 1 mol H2) = 0.536 g H2
So, 0.536 grams of H2 are needed to react with 2.50 g of N2.
To determine the amount of H2 needed to react with 2.50 g of N2, we can use the balanced chemical equation for the reaction. Without the equation, it's not possible to determine the amount of H2. However, assuming the balanced chemical equation is:
N2 + 3H2 -> 2NH3
From this equation, we can see that 1 mole of N2 reacts with 3 moles of H2 to produce 2 moles of NH3. Now we can proceed with the calculation.
Step 1: Convert the given mass of N2 to moles.
To do this, we need to know the molar mass of N2, which is 28.02 g/mol (2 x 14.01 g/mol).
Moles of N2 = (Mass of N2) / (Molar mass of N2)
= 2.50 g / 28.02 g/mol
≈ 0.089 moles
Step 2: Determine the moles of H2 required.
Using the mole ratio from the balanced chemical equation, we can find the moles of H2 needed.
Moles of H2 = 3 moles of H2 / 1 mole of N2 * Moles of N2
= 3 * 0.089 moles of H2
≈ 0.267 moles
Step 3: Convert moles of H2 to grams.
To convert moles of H2 to grams, we need to know the molar mass of H2, which is 2.02 g/mol (2 x 1.01 g/mol).
Mass of H2 = Moles of H2 * Molar mass of H2
= 0.267 moles * 2.02 g/mol
≈ 0.539 g
Therefore, approximately 0.539 grams of H2 are needed to react with 2.50 grams of N2.