I refer to the following question. Is my explanation correct, that step two

Question

I refer to the following question. Is my explanation correct, that step two

C6H14(g)--> 6CO2(g) + 7H2O(g)
can be considered combustion reaction?
Thank you!

Posted by jan on Tuesday, March 31, 2009 at 10:28pm.

C6H14(l)->C6H14(g) ->6CO2(g) + 7H2O(g) ->6CO2(g) + 7H2O(l)
Hexane is a liquid at room temp. It can be converted into carbon dioxide and water through the above processes. There are 3 steps. Steps 2 & 3 are exothermic, right? I think step 2
C6H14(g)->6CO2(g) + 7H2O(g) is something like combustion so it is exothermic.Please help.

Responses

Chemistry pls help - bobpursley, Tuesday, March 31, 2009 at 10:50pm
correct.

Chemistry pls help - DrBob222, Tuesday, March 31, 2009 at 10:56pm
But step 1 is endothermic.

Answer 1

You have omitted the oxygen that is responsible for combustion. If you will copy this as three steps and not run them together you will be less likely to omit reacts you need PLUS you will not confuse products with reactants.

C6H14(l) + heat ->C6H14(g) (step 1)
2C6H14(g) + 19O2 ->12CO2(g) + 14H2O(g)+ heat (step 2)
14H2O(g) ==> 14H2O(l) + heat (step 3)
Steps 2 and 3 are exothermic as you suggest. Step 2 is a combustion reaction. Step 1 is endothermic.

Answer 2

Yes, your explanation is correct. Step 2 (C6H14(g) -> 6CO2(g) + 7H2O(g)) can be considered a combustion reaction. In combustion reactions, a fuel combines with oxygen gas to produce carbon dioxide and water, releasing heat. In this case, hexane (C6H14) is the fuel and it reacts with oxygen gas to produce carbon dioxide and water. Since the reaction releases heat, it is considered exothermic. Step 1 is mentioned as endothermic, which means it requires heat input in order to occur.