Coal power plants burn large amounts of coal, C(s), in an 02(g) atmosphere to generate electricity. The chemical reaction responsible for producing this energy is shown below: c(s) +O2(g) ? CO2(g) Determine the volume of cop in liters produced when 100 metric ton of C(s) is completely burned in an 0p atmosphere. The density of co2 is 1.98 kg/m3 (1 metric ton 1000 kg: 1 m3- 1000 L)

Coal power plants burn large amounts of coal, C(s), in an O₂(g) atmosphere to generate electricity. The chemical reaction responsible for producing this energy is shown below:

C(s) + O₂(g) → CO₂(g)

Determine the volume of CO₂ in liters produced when 100 metric ton of C(s) is completely burned in an O₂ atmosphere. The density of CO₂ is 1.98 kg/m³ (1 metric ton = 1000 kg: 1 m³ = 1000 L)

We can establish the following relations:

1 metric ton = 1000 kg
1 kg = 1000 g
The molar mass of C(s) is 12.01 g/mol
The molar ratio of C(s) to CO₂(g) is 1:1
The molar mass of CO₂(g) is 44.01 g/mol
1.98 kg of CO₂(g) occupy a volume of 1 m³ (density = 1.98 kg/m³)
1 m³ = 1000 L

The volume of CO₂ produced when 100 metric ton of C(s) react is:

[tex]100metric/tonC.\frac{10^{6}gC}{1metric/tonC} .\frac{1molC}{12.01gC} .\frac{1molCO_{2}}{1molC} .\frac{44.01 \times 10^{-3} kgCO_{2}}{1molCO_{2}} .\frac{1m^{3}CO_{2}}{1.98kgCO_{2}} .\frac{1000LCO_{2}}{1m^{3}CO_{2}} =1.85 \times 10^{8} LCO_{2}[/tex]