How many grams of hydrogen are necessary to react completely with 50.0 g of nitrogen in the above reaction? How many grams of ammonia are produced in the reaction

1 answer

First, we need to write and balance the chemical equation for the reaction:

N2 + 3H2 → 2NH3

From the balanced equation, we can see that 1 mole of nitrogen reacts with 3 moles of hydrogen to produce 2 moles of ammonia.

1 mole of N2 has a molar mass of 28.02 g
So, 50.0 g of N2 is equal to 50.0 / 28.02 ≈ 1.784 moles of N2

To react completely with the nitrogen, we need 3 moles of hydrogen for every mole of nitrogen, so we need:

1.784 moles of N2 * 3 moles H2/mole N2 = 5.35 moles H2

The molar mass of hydrogen is 2.016 g/mol, so the mass of hydrogen needed is:

5.35 moles of H2 * 2.016 g/mol ≈ 10.79 g of H2

Therefore, 10.79 grams of hydrogen are necessary to react completely with 50.0 g of nitrogen.

To find the mass of ammonia produced, we first calculate the number of moles of ammonia produced:

From the balanced equation, 1 mole of N2 produces 2 moles of NH3
So, from 1.784 moles of N2, we get 1.784 * 2 = 3.568 moles of NH3

The molar mass of ammonia (NH3) is 17.03 g/mol, so the mass of ammonia produced is:

3.568 moles of NH3 * 17.03 g/mol ≈ 60.77 g of NH3

Therefore, approximately 60.77 grams of ammonia are produced in the reaction.
Similar Questions
  1. Question 18 (2 points)In the equation below, Nitrogen gas (N2) and Hydrogen gas (H2) react to produce Ammonia (NH3). If 6.30
    1. answers icon 1 answer
  2. Question 18 (2 points)In the equation below, Nitrogen gas (N2) and Hydrogen gas (H2) react to produce Ammonia (NH3).
    1. answers icon 1 answer
  3. According to the following chemical equation:N2 + 3H2 → 2NH3 How many grams of hydrogen are needed to completely react with
    1. answers icon 1 answer
    1. answers icon 1 answer
more similar questions