Answer:
3.0g of C6H6 would produce 10.03 grams of CO2 upon combustion.
Explained:
To determine the amount of CO2 produced from 3.0g of C6H6 (benzene), we need to first balance the chemical equation for the combustion of benzene:
C6H6 + 15O2 -> 6CO2 + 3H2O
From the balanced equation, we can see that for every 1 mole of C6H6, 6 moles of CO2 are produced. The molar mass of C6H6 is 78.11 g/mol, so we can convert the given mass of 3.0g to moles:
3.0g C6H6 / 78.11 g/mol = 0.038 moles C6H6
Now we can use the mole ratio from the balanced equation to calculate the number of moles of CO2 produced:
0.038 moles C6H6 x (6 moles CO2 / 1 mole C6H6) = 0.228 moles CO2
Finally, we can convert the number of moles of CO2 to grams using the molar mass of CO2, which is 44.01 g/mol:
0.228 moles CO2 x 44.01 g/mol = 10.03 g CO2
Therefore, 3.0g of C6H6 would produce 10.03 grams of CO2 upon combustion.