How many grams of CO2 are produced when 11.47 moles hexane combust?
Show work please
2C6H14 + 19O2 ==> 12CO2 + 14H2O
Use the coefficients in the balanced equation to convert mols C6H14 to mols CO2
Then convert mols CO2 to grams. g = mols x molar mass.
I balanced the equation like so C6H14 + 19/2 O2 ==> 6CO2 + 7H2O
My teacher taught us the 19/2 was valid
My work:
11.47 mol C6H14 * 6 CO2/1 mol C6H14 * 44g/mol/1 mol CO2 = 3, 028 g of CO2
To find the number of grams of CO2 produced when 11.47 moles of hexane (C6H14) combust, we need to determine the balanced chemical equation for the combustion of hexane.
The balanced chemical equation for the combustion of hexane is:
C6H14 + 19/2 O2 -> 6 CO2 + 7 H2O
From the equation, we can see that 1 mole of hexane (C6H14) produces 6 moles of CO2.
Now, we can use the mole-mole conversion to calculate the number of moles of CO2 produced:
moles of CO2 = moles of hexane (C6H14) × (6 moles CO2 / 1 mole hexane)
moles of CO2 = 11.47 moles × (6 moles CO2 / 1 mole hexane)
moles of CO2 = 68.82 moles CO2
Finally, we can convert moles of CO2 to grams of CO2 using the molar mass of CO2, which is about 44.01 grams/mole:
grams of CO2 = moles of CO2 × molar mass of CO2
grams of CO2 = 68.82 moles × 44.01 grams/mole
grams of CO2 ≈ 3029.52 grams (rounded to two decimal places)
Therefore, approximately 3029.52 grams of CO2 are produced when 11.47 moles of hexane combust.