Question

When 4.50 L of hydrogen gas react with an excess of nitrogen gas at standard temperature and pressure, how many liters of ammonia gas will be produced?

N2 (g) + 3H2 (g) yields 2NH3 (g)

Answer 1

When 4.50 L of hydrogen gas reacts with an excess of nitrogen gas at STP, 3.00 L of ammonia gas will be produced according to the balanced chemical equation.

Step-by-step explanation:

To determine how many liters of ammonia gas will be produced when 4.50 L of hydrogen gas reacts with an excess of nitrogen gas at standard temperature and pressure (STP), we can use the balanced chemical equation:

N2(g) + 3 H2(g) → 2 NH3(g)

At STP, gases occupy the same volume per mole, so the stoichiometry of the reactants and products is reflected in their volumes. The balanced equation shows that three volumes of hydrogen gas produce two volumes of ammonia gas. Hence, if 4.50 L of hydrogen reacts, they will produce 2/3 of that volume of ammonia, because for every 3 L of H2, 2 L of NH3 is produced.

Therefore, the calculation will be:

(4.50 L H2) × (2 L NH3 / 3 L H2) = 3.00 L NH3

So, 3.00 L of ammonia gas will be produced under the conditions provided.

Answer 2

3.0 L of NH₃

Solution:

The equation is as follow,

N₂ + 3 H₂ → 2 NH₃

According to equation,

67.2 L (3 mole) H₂ at STP produces = 44.8 L (3 mole) of NH₃

So,

4.50 L of H₂ will produce = X L of NH₃

Solving for X,

X = (4.50 L × 44.8 L) ÷ 67.2 L

X = 3.0 L of NH₃