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Sagot :
SOLUTION:
Step 1: Write the balanced chemical equation.
N₂ + 3H₂ → 2NH₃
Step 2: Calculate the number of moles of NH₃ formed by each reactant.
• Using N₂
Based on the balanced chemical equation, 1 mole of N₂ is stoichiometrically equivalent to 2 moles of NH₃.
[tex]\begin{aligned} \text{moles of} \: \text{NH}_3 & = \text{4.42 mol} \: \text{N}_2 \times \frac{\text{2 mol} \: \text{NH}_3}{\text{1 mol} \: \text{N}_2} \\ & = \text{8.84 mol} \end{aligned}[/tex]
• Using H₂
Based on the balanced chemical equation, 3 moles of H₂ is stoichiometrically equivalent to 2 moles of NH₃.
[tex]\begin{aligned} \text{moles of} \: \text{NH}_3 & = \text{6.60 mol} \: \text{H}_2 \times \frac{\text{2 mol} \: \text{NH}_3}{\text{3 mol} \: \text{H}_2} \\ & = \text{4.40 mol} \end{aligned}[/tex]
Step 3: Determine the limiting reagent.
Since H₂ produced less amount of NH₃ than N₂, H₂ is the limiting reagent.
Step 4: Determine the number of moles of NH₃ formed.
Note that the number of moles of a product formed is dictated by the limiting reagent.
[tex]\text{moles of} \: \text{NH}_3 = \boxed{\text{4.40 mol}}[/tex]
Hence, the number of moles of NH₃ that will be produced is 4.40 mol.
[tex]\\[/tex]
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