When methane (CH4) burns, it reacts with oxygen gas to produce carbon dioxide an

Question

When methane (CH4) burns, it reacts with oxygen gas to produce carbon dioxide and water. The unbalanced equation for this reaction is

CH4(g)+O2(g)CO2(g)+H2O(g)

This type of reaction is referred to as a complete combustion reaction.

1. What mass of carbon dioxide is produced from the complete combustion of 4.20×103 g of methane?

2. What mass of water is produced from the complete combustion of 4.20×103 g of methane?

3. What mass of oxygen is needed for the complete combustion of 4.20×103 g of methane?

Explanation / Answer

The balanced reaction is: CH4 + 2O2 ---> CO2 + 2H2O

1. 4.2x10-3g Methane / 16.04246g/mol = 2.62x10-4 moles of Methane (1mol CO2 / 1mol CH4) = 2.62x10-4 moles of CO2.

2.62x10-4 mol CO2 (44.0095g/mol) = 0.0115g of CO2

2.- 2.62x10-4 moles of CH4 (2moles H2O / 1mol CH4) = 5.24x10-4 moles H2O (18.01528g/mol) = 0.0094g of Water

3.- 2.62x10-4 moles of CH4 (2moles O2 / 1mol CH4) = 5.24X10-4 moles of O2 (31.9988g/mol) = 0.0168g of O2

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