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Question

Unlike science fair volcanoes, real volcanoes realease many dangerous gases. One of the gases released is sulfur dioxide, which is a major component of acid rain. In order to remove sulfur dioxide from the atmosphere, government clean-up programs combine it with calcium oxide to form calcium sulfite, a much safer compound.

Here is the balanced equation:
SO2CaO --> CaSO3

Here are the questions:
1. How many molecules of sulfur dioxide can be neutralized using 3 kilograms of calcium oxide?


2. How many liters of sulfur dioxide gas are neutralized in Question 3? (assume STP)

Answer 1

Ans 1)
CaO has a molecular weight = 40+16 = 56.
So 56 gms of CaO will contain 6.023 * 10^23 molecules (Avogardro's Number).
Hence, 3 Kgs of CaO will contain (3000 gm/56 gm) * 6.023 * 10^23 molecules. = 322.66 * 10^23 molecules.
Now 1 molecule CaO Neutralises 1 molecule SO2
[SO2 + CaO = CaSO3]
So 322.66 * 10^23 molecules will neutralise same number of molecules of SO2.

Ans 2)
Now, 1 mole of all gas at NTP has a volume of 22.4 litres (One of the derivation of Avogadro's Law).
1 mole of SO2 (contains 6.023 * 10^23 molecules) will occupy a volume of 22.4 litres at NTP.
or 322.66 * 10^23 molecules of SO2 (derived in Q 1 above) will occupy 22.4 * (322.66/6.023) litres = 22.4 * 54 litres = 1210 litres (apx).
This calculation is for NTP (Normal Temperature and Pressure, i.e, 273 K and 1 atm). But in volcanic condition, the temperature and pressure will be higher., and the actual volume may therefore vary.