Final answer:
To determine the limiting reactant and calculate the mass of NH₃ produced, compare the moles of each reactant to their stoichiometric ratio. The molar ratio of N₂ to H₂ is 1:3. To find the excess reactant and calculate the mass remaining, subtract the consumed moles from the original amount. The percentage yield of NH₃ can be calculated by comparing the actual and theoretical yields.
Step-by-step explanation:
To determine the limiting reactant and calculate the mass of NH₃ produced, we need to compare the number of moles of each reactant to their stoichiometric ratio in the balanced equation. First, calculate the number of moles of N₂ and H₂ using their respective masses and molar masses. Next, divide the number of moles of each reactant by their stoichiometric coefficients to determine the number of moles of NH₃ that can be produced. The limiting reactant is the one that produces the smaller number of moles of NH₃. To calculate the mass of NH₃ produced, multiply the number of moles of NH₃ by its molar mass.
The molar ratio of N₂ to H₂ in the reaction is 1:3. This means that for every 1 mole of N₂, 3 moles of H₂ are needed for the reaction to occur. This ratio is determined by the coefficients in the balanced equation.
To find the excess reactant and calculate the mass remaining after the reaction, subtract the amount (in moles) of the limiting reactant that reacted from the amount that was originally present. Convert the remaining moles to grams using the molar mass of the excess reactant.
The percentage yield of NH₃ can be calculated by dividing the actual yield (the mass of NH₃ produced) by the theoretical yield (the mass of NH₃ calculated from the limiting reactant) and multiplying by 100. This gives the percentage of NH₃ that was actually obtained compared to the maximum possible yield.