The balanced equation for the combustion of octane is:
(2C_8H_{18} + 25O_2 \rightarrow 16CO_2 + 18H_2O)
How many grams of CO2 are formed from 8.7 mol of C8H18?
To find the grams of CO2 formed from 8.7 mol of C8H18, we first need to use the stoichiometry of the balanced equation to convert moles of C8H18 to moles of CO2, and then finally to grams of CO2.
From the balanced equation, we can see that 2 moles of C8H18 react to form 16 moles of CO2.
Step 1: Convert moles of C8H18 to moles of CO2
8.7 mol C8H18 x (16 mol CO2 / 2 mol C8H18) = 69.6 mol CO2
Step 2: Convert moles of CO2 to grams of CO2
Using the molar mass of CO2 (44.01 g/mol):
69.6 mol CO2 x 44.01 g/mol = 3059.6 g CO2
Therefore, 8.7 mol of C8H18 will produce 3059.6 grams of CO2.