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 data:

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

plants need sunlight, water, and carbon dioxide to make food. plants use the raw materials of water, nutrients they absorb from soil, and carbon dioxide to make sugars the plant can use. energy from the sun and chlorophyll are also needed.