Read the given chemical reaction.

c2h6 + o2 → co2 + h2o

how many moles of co2 are produced during the complete combustion of 3.6 moles of c2h6? (5 points)

1.8 moles

4.4 moles

7.2 moles

9.2 moles

During the complete combustion of 3.6 moles of ethanol, there is produced 7.2 moles of CO2

Explanation:

The balanced equation is: 2 C2H6 + 7O2 → 4 CO2 + 6 H2O

This is the combustion reaction of ethanol. Ethanol will be completely consumed.

This means that for 2 moles of C2H6 consumed, there is consumed 7 moles of O2, and there is produced 4 moles of CO2 and 6 moles of H2O.

This means that for 3.6 moles of C2H6 consumed, there is produced 3.6 * 2 moles = 7.2 moles of CO2

During the complete combustion of 3.6 moles of ethanol, there is produced 7.2 moles of CO2

2h2o2--> 2h2o + o2

this reaction is of the spontaneous decomposition of hydrogen peroxide down into water and oxygen.

add 2 molecules of hydrogen peroxide and 2 molecules of water. since oxygen is naturally diatomic, the total number of atoms of each element is now the same on both sides of the equation so it is balanced.

this may not be entirely correct but let me know.

c. 75.7

i think that is the right