What mass of carbon dioxide is produced from the complete combustion of 8.00*10-3 g of methane? Express your answer with the appropriate units.

22*10-3 g

Explanation:

Combustion equation of methane:

CH4 + 2O2 → CO2 + 2H2O

Given dа ta:

mass of methane = 8.00 * 10-3 g

mass of carbon dioxide=?

Solution 1:

m (CH4) = 8.00 * 10-3 g

v=m / M

v (CH4) = m (CH4) / M (CH4)

v (CH4) = 8.00 * 10-3 g / 16 g / mol

v (CH4) = 0.5 * 10-3 mol

according to balance chemical equation:

v (CH4) : v (CO2) = 1:1

v (CH4) = v (CO2)

M (CO2) = 44 g/mol

m (CO2) = M (CO2) * v (CO2)

m (CO2) = 44 g/mol * 0.5 * 10-3 mol = 22*10-3 g

Second method:

molecular weight of methane = 16 g/mol

molecular weight of carbon dioxide = 44 g/mol

mass of methane = 8.00*10-3 g

mass of carbon dioxide=?

Solution:

mass of carbon dioxide = mass of methane * molecular weight of carbon dioxide / molecular weight of methane

mass of carbon dioxide = 8.00*10-3 g * 44 g/mol / 16 g/mol

mass of carbon dioxide = 22 * 10-3 g