Question

Combustion of coal releases sulfur dioxide into the atmosphere. The following process converts this gas into sulfuric acid, a component of acid rain

2SO2(g) + O2(g) → 2SO3(g)

SO3(g) + H2O(l) → H2SO4(aq)

If each metric ton of coal produces 1.16 x 104 L of sulfur dioxide (measured at STP), what mass (kg) of sulfuric acid can result from combustion of each metric ton of coal? (1 metric ton = 1000 kg)

Answer 1

50,8 kg of H₂SO₄

Step-by-step explanation:

Moles in 1,16x10⁴L of sulfur dioxide at STP can be obtained using:

n = PV/RT

Where pressure is 1 atm and temperature is 273,15K at STP, knowing R: 0,082atmL/molK:

n = 1atm* 1,16x10⁴L/0,082atmL/molK*273,15K

n = 518 moles

As 1 mol of SO₃(g) produce 1 mol of H₂SO₄(aq), moles of H₂SO₄(aq) can result from the combustion of each metric ton of coal are 518 moles, in grams:

518 moles of H₂SO₄(aq)×
`(98,08g)/(1mol)` = 50805g = 50,8 kg of H₂SO₄

I hope it helps!