Liquid hexane, C₆H₁₄, burns in oxygen gas to yield carbon dioxide and water. What is the minimum mass of oxygen required for the complete reaction of 10.0 mL of hexane? (density of hexane = 0.660 g/mL) A)3.71 g B)2.45 g C)23.3 g D)46.6 g E)35.3 g

Question

Quizplus · Accepted Answer

First, we need to determine the mass of 10.0 mL of hexane:

mass = volume x density = 10.0 mL x 0.660 g/mL = 6.60 g

Next, we can use the balanced chemical equation to determine the amount of oxygen required for the complete combustion of 1 mole of hexane:

C6H14 + 19/2 O2 → 6 CO2 + 7 H2O

From this equation, we can see that 19/2 moles of O2 are required for every mole of hexane.

Using the molar mass of hexane (86.18 g/mol), we can determine the number of moles of hexane in 6.60 g:

moles of hexane = mass/molar mass = 6.60 g/86.18 g/mol = 0.0766 mol

Therefore, the minimum mass of oxygen required for the complete reaction of 6.60 g of hexane is:

mass of O2 = (19/2) x moles of hexane x molar mass of O2 
               = (19/2) x 0.0766 mol x 32.00 g/mol 
               = 23.3 g

So the answer is (C) 23.3 g.

Liquid Hexane, C6H14, Burns in Oxygen Gas to Yield Carbon

Liquid Hexane, C₆H₁₄, Burns in Oxygen Gas to Yield Carbon