How many grams of H2 are needed to react with 100g of N2 to produce 121g of NH3

Answer 1

To calculate the amount of H2 needed to react with 100g of N2 to produce 121g of NH3, we can use the balanced chemical equation for the reaction:

N2 + 3H2 -> 2NH3

First, calculate the molar masses of each compound:
- N2: 2(14.01) = 28.02 g/mol
- H2: 2(1.008) = 2.016 g/mol
- NH3: 1(14.01) + 3(1.008) = 17.03 g/mol

Next, calculate the moles of N2 and NH3 using their respective molar masses:
- Moles of N2: 100g / 28.02 g/mol = 3.57 mol
- Moles of NH3: 121g / 17.03 g/mol = 7.11 mol

According to the balanced equation, 1 mole of N2 reacts with 3 moles of H2 to produce 2 moles of NH3. Therefore, the moles of H2 needed can be calculated as follows:
- Moles of H2 = (3.57 mol N2) / (1 mol N2) x (3 mol H2) = 10.71 mol H2

Finally, calculate the mass of H2 needed using the molar mass of H2:
- Mass of H2 = 10.71 mol x 2.016 g/mol = 21.61 g

Therefore, 21.61 grams of H2 are needed to react with 100g of N2 to produce 121g of NH3.