Question

Part A. What mass of carbon dioxide is produced from the complete combustion of 5.70×10⁻³ g of methane?

Part B. What mass of water is produced from the complete combustion of 5.70×10⁻³ g of methane?

Part C. What mass of oxygen is needed for the complete combustion of 5.70×10⁻³g of methane?

Express your answer with the appropriate units.

Answer 1

Solution :-

Balanced reaction equation for the combustion of methane is as follows

CH4 + 2O2 ------ > CO2 + 2 H2O

Part A. What mass of carbon dioxide is produced from the complete combustion of 5.70×10⁻³ g of methane?

solution :- mole ratio of the methane to CO2 is 1 : 1

that is 16.04 g CH4 = 44.01 g CO2

therefore 5.70*10^-3 g CH4 * 44.01 g CO2 / 16.04 g CH4 = 1.56*10^-2 g CO2

So the amount of CO2 that can be produced = 1.56*10^-2 g

Part B. What mass of water is produced from the complete combustion of 5.70×10⁻³ g of methane?

Solution :-

mole ratio of the CH4 to H2O is 1 : 2

this means 16.04 g CH4 = (2*18.0148 g ) H2O that is 36.03 g H2O

hence

5.7*10^-3 g CH4 * 36.03 g H2O / 16.04 g CH4 = 1.28*10^-2 g H2O

Therefore the mass of H2O that can be formed = 1.28*10^-2 g

Part C. What mass of oxygen is needed for the complete combustion of 5.70×10⁻³ g of methane?

Solution :-

mole ratio of the CH4 to O2 is 1 : 2

16.04 g CH4 = 64.0 g O2

therefore 5.7*10^-3 g CH4 * 64.0 g O2 / 16.04 g CH4 = 2.27*10^-2 g O2

Therefore mass of the O2 needed to react with given mass of CH4 is 2.27*10^-2 g