Question

Please help!

N2 + 3H2 —> 2NH3
Suppose you have 2.0 L of nitrogen. How many liters of hydrogen do you need for a
complete reaction? (One mole of any gas occupies 22.4 L under certain conditions of
temperature and pressure. Assume those conditions for this question.)

Answer 1

To react completely with 2.0 L of nitrogen, you would need 6.0 L of hydrogen according to the stoichiometric ratio of the balanced chemical reaction N2 + 3 H2 → 2 NH3.

Step-by-step explanation:

For a complete reaction of nitrogen (N2) to form ammonia (NH3), you need three times the volume of hydrogen (H2) as the provided volume of nitrogen. Given that the balanced equation is N2 + 3 H2 → 2 NH3, and we know that one mole of a gas occupies 22.4 L at standard conditions, you can calculate the required volume of hydrogen. If you have 2.0 L of nitrogen, using the mole ratio of nitrogen to hydrogen from the balanced equation which is 1:3, you would need 3 times the volume of hydrogen gas. Hence you would need 2.0 L * 3 = 6.0 L of hydrogen for a complete reaction with 2.0 L of nitrogen.

Answer 2

`\large \boxed{\text{6 L}}`

Step-by-step explanation:

We can use Gay-Lussac's Law of Combining Volumes to solve this problem.

Gases at the same temperature and pressure react in the same ratios as their coefficients in the balanced equation.

1. Write the chemical equation.

Ratio: 1 L 3 L

N₂ + 3H₂ ⟶ 2NH₃

V/L: 2

2. Calculate the volume of H₂.

According to Gay-Lussac, 3 L of H₂ react with 1 L of N₂.

Then, the conversion factor is (3 L H₂/1 L N₂).

`\text{Volume of H}_(2) = \text{2 L N}_(2) * \frac{ \text{3 L H}_(2) }{\text{1 L N}_(2)}= \textbf{6 L H}_(2)\\\text{You need $\large \boxed{\textbf{6 L}}$ of hydrogen,}`