# What is the maximum mass of ammonium sulfate that can be obtained from 2 kg of sulfuric acid and 1 kg of ammonia?

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Sulfuric acid (H2SO4) reacts with ammonia (NH3) to produce the fertilizer ammonium sulfate ((NH4)2SO4) according to the following equation:

H2SO4(aq)+2NH3(g)→(NH4)2SO4(aq)

What is the maximum mass of ammonium sulfate that can be obtained from 2 kg of sulfuric acid and 1 kg of ammonia?

by (56.5k points)

$H_2SO_4 (aq) + 2NH_3(g) \longrightarrow (NH_4)_2 SO_4 (aq)$

Number of moles of $H_2SO_4 = \frac{2000}{98} = 20.4 \,moles$

Number of moles of $NH_3 = \frac{1000}{17} = 58.8\, moles$

$\because$ 1 mole of H2SO4 react with 2 mole of NH3 to form = 1 mole (NH4)2 SO4

$\therefore$ Number of moles of NH3 required to complete reaction with 20.4 mole of H2SO4 = 20.4 x 2 = 40.8 mole

but we have NH3 = 58.8 mole

$\therefore$ H2SO4 is a limiting reagent.

$\therefore$ Number of moles of (NH4)2 SO4 formed = 20.4 mol

$\therefore$ Mass of (NH4)2 SO4 formed = 20.4 x 132

= 2692.8 g

= 2.7 kg

Hence, maximum mass of (NH4)2 SOcan be formed = 2.7 kg.