Question

2. ^{Considerthefollowingequationwhichdescribesthecombustionofmethane.Note:methaneisCH}4(g)

^CH4(g) ^{+ 2O}2(g) → ^CO2(g) ^+2H2^O(g)

a. How many grams of carbon dioxide can be formed from the complete combustion of 100. grams of methane?

b. How many moles of carbon dioxide can be formed from the combustion of methane with

100. grams of oxygen?

c. How many moles of water will be formed from the combustion of methane with 100. grams of oxygen?

Answer 1

a) Moles of CH4 = 100 g/16 g.mol^-1 = 6.25 mol

The mole ratio CH4:CO2 = 1:1

Therefore, the mass of CO2 produced = 6.25 mol * 44 g/mol = 275 g

b) Moles of O2 = 100 g/32 g.mol^-1 = 3.125 mol

The mole ratio O2:CO2 = 2:1

Therefore, the mass of CO2 produced = (3.125/2) mol = 1.5625 mol

c) Moles of O2 = 100 g/32 g.mol^-1 = 3.125 mol

The mole ratio O2:H2O = 1:1

Therefore, the mass of CO2 produced = 3.125 mol