Final answer:
For a 0.1 g sample of N2, approximately 0.0214 g of H2 is required for a complete reaction.
Step-by-step explanation:
Given that the balanced equation for the reaction is:
N₂ + 3 H₂ → 2 NH₃
The molar mass of N₂ is 28 g/mol, so for a 0.1 g sample of N₂, we can use the molar mass to find the number of moles of N₂:
0.1 g N₂ x (1 mol N₂/28 g N₂) = 0.00357 mol N₂
According to the stoichiometry of the balanced equation, the ratio of moles between N₂ and H₂ is 1:3. So, for every 1 mole of N₂, we need 3 moles of H₂. Therefore, the number of moles of H₂ required is:
0.00357 mol N₂ x (3 mol H₂/1 mol N₂) = 0.0107 mol H₂
Finally, we can use the molar mass of H₂ to find the mass of H₂ required:
0.0107 mol H₂ x (2 g H₂/1 mol H₂) = 0.0214 g H₂
Therefore, the mass of H₂ required for a complete reaction with a 0.1 g sample of N₂ is approximately 0.0214 g.