Consider the reaction below.
2C6H14 + 19O2 mc032-1.jpg 12CO2 + 14H2O
How many moles of hexane (C6H14) must burn to form 18.4 mol of carbon dioxide?
1.53 mol
3.07 mol
110. mol
175. mol
Rx shows a 2 to 12 Hexane to CO2 ratio, or (if reduced) a 1 to 6 mole Hexane:CO2 ratio; that is, for each mole of hexane burned, 6 moles of CO2 are produced. So, if given 18.4 moles Hexane then... 6 times more in moles of CO2 will be formed. = 110 moles.
To determine the number of moles of hexane (C6H14) required to form 18.4 moles of carbon dioxide (CO2), we need to use the balanced equation for the combustion of hexane.
The balanced equation is:
2C6H14 + 19O2 → 12CO2 + 14H2O
From the equation, we can see that 2 moles of hexane are required to produce 12 moles of carbon dioxide. Therefore, the ratio is 2 moles of hexane to 12 moles of carbon dioxide.
To find the number of moles of hexane needed to form 18.4 moles of carbon dioxide, we can set up a proportion:
(2 moles of hexane / 12 moles of carbon dioxide) = (x moles of hexane / 18.4 moles of carbon dioxide)
Cross multiplying the proportions, we get:
12 moles of carbon dioxide * x moles of hexane = 2 moles of hexane * 18.4 moles of carbon dioxide
12x = 2 * 18.4
12x = 36.8
x = 36.8 / 12
x ≈ 3.07 mol
Therefore, approximately 3.07 moles of hexane are required to form 18.4 moles of carbon dioxide. Therefore, the correct answer is 3.07 mol.