How many moles of CO2 will be produced from the complete reaction of 5.59 moles of C4H10? 2 C4H10 + 13 O2 → 8 CO2 + 10 H2O

The balanced chemical equation for the reaction is:

`2C_4H_10 + 13O_2 -> 8CO_2 + 10H_2O`

In this reaction, butane undergoes combustion to produce carbon dioxide and water. 

Using stoichiometry, we can see that 2 moles of butane react with 13 moles of oxygen to form 8 moles of carbon dioxide and 10 moles of water.

Since 2 moles of butane form 8 moles of carbon dioxide,

1 mole of butane will form 4 moles (= 8/2 moles) of carbon dioxide

and 5.59 moles of butane will form 4 x 5.59 moles = 22.36 moles of carbon dioxide.

Since the molar mass of carbon dioxide is 44 g/mole, this translates to 938.84 g (= 22.36 moles x 44 g/mole) of carbon dioxide.

Along with 22.36 moles of carbon dioxide, 27.95 moles (= 10/2 x 5.59 moles) of water are also formed.

Hope this helps.