Answer:
1558.27 ml or 1.56 L
Step-by-step explanation:
The molecular mass of octane is 114.23 g/mol so 1.00 g of octane equals to:
(1.00 g( x (1 mol/114.23g) = 0.00875 mol
From the chemical equation:
2C8H18 + 25O2 --> 16CO2 + 18H2O
you know that 2 mol of octane will produce 16 mol of CO2
so 0.00875 mol of octane will produce:
0.00875 x (16/2) = 0.07 moleof CO2
The molecular mass of CO2 is 44.01 g/mol so 0.07 mol will equal to
44.01 x 0.07 = 3.0807 g of CO2
Under “standard” conditions of 0 degrees Celsius and 1 atmosphere of pressure, carbon dioxide exhibits a density of 0.001977 g/mL
since d = m/V => V = m/d = 3.0807/0.001977 = 1558.27 ml or 1.56 L
NOTE: if you have a specific temperature or pressure, you can use the formula for ideal gas PV=nRT to solve for volume.
I hope this helps you to understand the question