Explanation
Given
[tex]2C_8H_{18}+25O_2\rightarrow16CO_2+18H_2O[/tex]Mass of O2 = 500 g
Required: Mass of CO2 and H2O that will be produced.
Solution
CO2 that will be produced.
Step 1: Find the moles of O2
n = m/M where n is the moles, m is the mass and M is the molar mass
n = 500 g/31.998 g/mol
n = 15.63 mol
Step 2: Use the stoichiometry to find moles of CO2
The molar ratio between O2 and CO2 is 25:16
Therefore the moles of CO2 = 15.63 x (16/25) = 10.00 mol
Step 3: Calculate the mass of CO2 that will be produced.
m = n x M
m = 10.00 mol x 44,01 g/mol
m = 440.13 g
H2O mass that will be produced
Step 1: Use the stoichiometry to find moles of H2O
The molar ratio between O2 and H2O is 25:18
Therefore the moles of CO2 = 15.63 x (18/25) = 11.25 mol
Step 3: Calculate the mass of H2O that will be produced.
m = n x M
m = 11.25 mol x 18.01528 g/mol
m = 203 g
Answers
Mass of CO2 = 440 g
Mass of H2O = 203 g