Question

The reaction below shows the combustion of butane (C4H10). Why is the mole ratio (8 moles CO2/2 mol C4H10) used to determine the amount of carbon dioxide (CO2) produced when butane (C4H10) combusts in excess oxygen?

Answer 1

C4H10 + O2 yields CO2 + H2O + heat

Butane has a mass that is 4 times greater than CO2, so only 2 moles of C4H10 are needed to produce 8 moles of CO2.
Carbon dioxide has a volume of about one-quarter that of C4H10, so 4 moles of CO2 are needed to react with each mole of C4H10.
During combustion, CO2 is approximately 4 times more reactive than C4H10, so less C4H10 will partici

Answer 2

@sweetburger

Answer 3

@Jesstho.-. @JhonyLovesSchool @Jessica47 @sleepyjess @scapeplan @Sheraz12345 @Schleifspur @RosieF @lexiistarr @Lethal @Luigi0210

Answer 4

@DW101796

Answer 5

@dhiraj123

Answer 6

When the chemical equation for butane combustion is balanced, 2 moles of C4H10 are needed to produce 8 moles of CO2.

Answer 7

so you mean it is the first option Butane has a mass that is 4 times greater than CO2, so only 2 moles of C4H10 are needed to produce 8 moles of CO2. @DW101796

Answer 8

Yep. Good job. :)

Answer 9

thank you!!!!

Answer 10

Welcome. :)

Answer 11

retriceole

Answer 12

thank you