Question

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30 points
You carry out the reaction represented by the following balanced equation: N2(g) + 3H2(g) → 2NH3(g) You add an equal number of moles of nitrogen and hydrogen gases in a balloon. The volume of the balloon is 1.00 L before any reaction occurs. Determine the volume of the balloon after the reaction is complete. Assume constant temperature,
A) 0.330 L
B) 0.670 L
C) 1.00 L
D) 1.50 L
E) 3.00 L​

Answer 1

B.

Avogadro Law was used and the stoichometric ratios and number of moles.

Thank you for this question mate. It was challenging but I hope you understand the formula.

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Answer 2

The volume of the balloon can be found by making use of Avogadro's Law

and the given chemical equation.

• The volume of the balloon after the reaction is B. 0.670 L

Reason:

The given reaction is; N₂(g) + 3H₂(g) → 2NH(g)

From the given reaction, we have;

One mole of nitrogen reacts with three moles of hydrogen to produce two

moles of ammonia.

Therefore, the reaction requires three moles of hydrogen, H₂, which is the

limiting reactant.

According to Avogadro's Law, which states that equal volumes of gas

contain equal number of molecules at the same temperature and

pressure, we have;

0.5 L of H₂ will react with $0.5 \, L \times \frac{1}{3} = \frac{1}{6}$ L, of N₂ to produce

$0.5 \, L \times \frac{2}{3} = \frac{1}{3}$ L of NH₃

The remaining gases in the balloon after the reaction are;

• Volume of the unreacted nitrogen gas = $(\frac{1}{2} \, L - \frac{1}{6}\, L) = \frac{1}{3}\, L$

• Volume of the ammonia gas produced, NH₃ = $\frac{1}{3} L$

The volume of the balloon after the reaction is therefore;

• $\frac{1}{3} L$ of ammonia + $\frac{1}{3}\, L$ of nitrogen gas = $\frac{2}{3}$ ≈ 0.670 Liters

The correct option is option B. 0.670 L.

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