Determining Heat of Formation of n-Butane

[Nellen2222]

Homework Statement

The standard heat of formation of n butane cannot be measured directly but can be determined indirectly from other heats of reaction by applying hess's law. Given the folowing data for the combustion of carbon hydrogen and n butane in oxygen:

C + O2---> CO2 H=-393.5
H2 + 1/2O2 --> H2O
C4H10 + 6.5O2 ---> 4CO2 + 5H2O

Homework Equations

The Attempt at a Solution

Tried several times on scratch paper. The formation of butane is as so : 4C + 5H2-->C4H10

Ive tried the actual formation using CO2 + H2O --> C4H10 But i can't cancel the carbons

Sticking with my other normal equation 4C + 5H2 --> C4H10 (This is what I want, No?)

Tell me if my equation is wrong, cause it proabably is.

I tried multiplying the first step by 4, the second step by 5, and reversing the third step only to get everything to cancel except the oxygen. I get stuck with 6.5 oxygens on the left side and 9.5 Oxygens on the right. Dont know where to g ofrom there. Help please!

 

[Borek]

$$4 \times 1 + 5 \times \frac 1 2 = 6.5$$

 

[Nellen2222]

elaborate...?

 

[Nellen2222]

Here is another question: Write the chemical equation for the standard molar enthalpy of formation of proponol. c3h8O
Is this simply :: 3C + 8H + O2 ----> C3H8O ( I am pretty sure its this one.)

?

Or is it 3CO2 + 4H2O ----> C3H8O + 9/2O2

Thanks

 

[Borek]

elaborate...?

Where did you get 9.5 molecules of oxygen from?

 

[Borek]

Is this simply :: 3C + 8H + O2 ----> C3H8O ( I am pretty sure its this one.)

It is not balanced and it uses substances in non standard state. But it is much better than the other one.