Question

N2 + 3H2 ---> 2NH3 We want to produce 2.75 mol of NH3. How many moles of nitrogen would be required?
A. 5.5 moles
B. 1.38 moles
C. 1.83 moles
D. 4.13 moles
N2 + 3H2 ---> 2NH3 Suppose 6.00 mol of H2 reacted with sufficient nitrogen. How many moles of ammonia would be produced?
A. 1 mole
B. 2 moles
C. 3 moles
D. 4 moles

Answer 1

Hope this helps you.

Answer 2

The number of moles of nitrogen that would be required is 1.38 moles. The correct option is B. 1.38 moles

The number of moles of ammonia that would be produced is 4 moles. The correct option is D. 4 moles.

Stoichiometry

From the question,

We are to determine how many moles of nitrogen would be required.

From the given balanced chemical equation,

N₂ + 3H₂ → 2NH₃

This means

1 mole of N₂ reacts with 3 moles H₂ to produce 2 moles of NH₃

Now,

If 1 mole of N₂ is required to produce 2 moles of NH₃

Then,

x moles of N₂ will be required to produce 2.75 moles of NH₃

x = $\frac{2.75 \times 1}{2}$

x = 1.375 moles

x ≅ 1.38 moles

Hence, the number of moles of nitrogen that would be required is 1.38 moles. The correct option is B. 1.38 moles

To determine how many moles of ammonia would be produced is 6.00 mol of H₂ reacted with sufficient nitrogen

Since,

1 mole of N₂ reacts with 3 moles H₂ to produce 2 moles of NH₃

Then,

Sufficient N₂ will react with 6.00 moles H₂ to produce 4 moles of NH₃

Hence, the number of moles of ammonia that would be produced is 4 moles. The correct option is D. 4 moles.

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