## 8.51

Miranda 1J
Posts: 51
Joined: Fri Sep 29, 2017 7:06 am

### 8.51

Can someone please explain this problem to me? I'm super confused! Are we just supposed to use enthalpies of formation and if so what do we do next?

Thanks!

torieoishi1A
Posts: 32
Joined: Sat Jul 22, 2017 3:00 am

### Re: 8.51

Yes, you use enthalpies of formation to find the enthalpy of reaction for the reaction.
28(-393.51kJ/mol)+10(-241.82kJ/mol)-4(067kJ/mol)=-13168kJ/mol (the energy released per mole of reaction)
Since it is asking "per mole," 1/4 of the energy (3292kJ/mol) will be released per mole of TNT consumed.
In order to get the energy density in "kJ/L," you need to take 3292kJ/mol and divide it by the mass of one mole of TNT (227.14 g/mol) and then multiply it by the density of TNT (1.65 g/cm^3) and then convert cm^3 to L (10^3cm^3/L).
The answer should be 23.9x10^3kJ/L

Return to “Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)”

### Who is online

Users browsing this forum: No registered users and 2 guests