Recap - Fertilizer Plant

Part of the Stoichiometry section of Coddy's Chemistry journey. Lesson 29 of 41.

Challenge

Ammonium sulfate, (NH₄)₂SO₄ (132 g/mol), is one of the most common nitrogen fertilizers. A pilot plant makes it in two steps. First, nitrogen and hydrogen gases give ammonia:

N₂(g) + 3H₂(g) → 2NH₃(g)

Then the ammonia is led into a solution of sulfuric acid:

2NH₃(g) + H₂SO₄(aq) → (NH₄)₂SO₄(aq)

A container of ammonia gas labeled 6.8 g beside a beaker of sulfuric acid solution, 200 mL

Ammonia gas is led into 200 mL of sulfuric acid solution

In one test run the plant makes 6.8 g of ammonia and leads all of it into 200 mL of sulfuric acid solution. The ammonia and the acid react completely, and the volume of the solution stays 200 mL. Assume that 1 mol of gas takes 25 L at room conditions.

Calculate the mass of ammonium sulfate, m_S, that forms from the 6.8 g of ammonia (NH₃, 17 g/mol).

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