Question

Ammonia, NH3, is produced from the reaction of gaseous nitrogen and hydrogen at high temperatures. 3...

Ammonia, NH3, is produced from the reaction of gaseous nitrogen and hydrogen at high temperatures.

3 H2 (g) + N2 (g)  → 2 NH3 (g)

For the reaction of 3.77 g of H2 with 8.66 g of N2, you determined that 21.2 g and 10.5 g of ammonia could be produced, respectively. In the laboratory, you reacted these masses of H2 and N2 and collected 7.70 g of NH3. What is the percentage yield of this reaction to the correct number of significant figures?


_____Units_______

Homework Answers

Answer #1

3 H2 (g) + N2 (g)  → 2 NH3 (g)

No. of moles of H2 = 3.77 / 2 = 1.885 moles

No. of moles of N2 = 8.66 / 28 = 0.309 moles

no. of moles of H2 needed to react with 0.309 moles of N2 = 3 x 0.309 = 0.928 moles

Here, No. of moles of H2 present in excess.

So, limiting reagent is N2

No. of moles of NH3 produced = 2 x 0.309 = 0.618 moles

Weight of NH3 produced = 0.618 x 17 = 10.515 grams

Actual weight of NH3 collected = 7.70 g

Percentage yield = (7.70 / 10.515) x 100 = 73.2 %

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