When 0.136 moles of 1-pentanol react with excess oxygen in a combustion reaction?

Answer 1

Let's assume all propanol reacts fully with the oxygen.

First let's set up the reaction equation.

2 C3H8O1 + 9 O2 --> 8 H2O + 6 CO2

2 mole propanol reacts with oxygen to form 6 mole of CO2.

Thus the mole ratio is 2:6 = 1:3

So 0.136 mole of propanol forms 0.136 * 3 = 0.408 mole CO2

Answer 2

The excess oxygen ensures that full combustion to dioxide occurs and no carbon monoxide nor carbon is produced. The reaction is given by:

2 C3 H7 OH + 9 O2 → 6 C O2 + 8 H2 O

(Spaces used to make the formulae easier to read as subscripts not available for the numbers)

So for every 3 moles of propanol 6 moles of carbon dioxide are produced; thus there will be:

0.136 ÷ 2 × 6 = 0.136 × 3 = 0.408 moles of carbon dioxide produced.

Answer 3

The combustion reaction of 1-pentanol (C5H12O) with oxygen produces carbon dioxide (CO2) and water (H2O) as the main products. The balanced equation for this reaction is:

C5H12O + 8O2 -> 5CO2 + 6H2O

Since we have 0.136 moles of 1-pentanol, it will produce 0.136 moles of CO2 and 0.1632 moles of H2O in this reaction.

Answer 4

0.95 - 0.954

Answer 5

0.680

Answer 6

58.5 - 58.9