The chemically balanced equation presented below illustrates the reaction between nitrogen (N2) and hydrogen (H2) resulting in the formation of ammonia (NH3).

Question

N2 + 3H2 → 2NH3

In the event that 10.0 grams of nitrogen participate in a reaction to produce 12.0 grams of ammonia, what would be the quantity of hydrogen, in grams, have been during this reaction?

(1 point)
Responses

2.0 g of H2
2.0 g of H 2

10 g of H2
10 g of H 2

12 g of H2
12 g of H 2

3.0 g of H2

Answer 1

To find the quantity of hydrogen (H₂) used in the reaction, we first need to establish the moles of nitrogen (N₂) and ammonia (NH₃) involved.

1. Calculate the molar mass of nitrogen (N₂):

   • Nitrogen has a molar mass of approximately 14.01 g/mol.
   • Therefore, N₂ = 2 * 14.01 g/mol = 28.02 g/mol.

2. Calculate the moles of nitrogen (N₂) used in the reaction:

   • Moles of N₂ = mass (g) / molar mass (g/mol) = 10.0 g / 28.02 g/mol ≈ 0.357 moles of N₂.

3. From the balanced chemical equation:

   • 1 mole of N₂ reacts with 3 moles of H₂ to produce 2 moles of NH₃.
   • Therefore, 0.357 moles of N₂ would react with: \[ 0.357 , \text{moles N₂} \times 3 , \text{moles H₂/mole N₂} = 1.071 , \text{moles H₂}. \]

4. Calculate the molar mass of hydrogen (H₂):

   • Hydrogen has a molar mass of approximately 1.008 g/mol.
   • Therefore, H₂ = 2 * 1.008 g/mol = 2.016 g/mol.

5. Calculate the mass of hydrogen (H₂) used in the reaction:

   • Mass of H₂ = moles * molar mass = 1.071 moles * 2.016 g/mol ≈ 2.16 g of H₂.

Based on the options provided, the closest answer is 2.0 g of H₂.