Question

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)

Answer 1

1.85 × 10⁸ L

Step-by-step explanation:

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:

`100metric/tonC.(10^(6)gC)/(1metric/tonC) .(1molC)/(12.01gC) .(1molCO_(2))/(1molC) .(44.01 * 10^(-3) kgCO_(2))/(1molCO_(2)) .(1m^(3)CO_(2))/(1.98kgCO_(2)) .(1000LCO_(2))/(1m^(3)CO_(2)) =1.85 * 10^(8) LCO_(2)`