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