WILL GIVE MEDAL AND FAN FOR WHO EVER ANSWERS THIS! PLZZ HELP!!

Calculate ?H0for the following reaction.

2NO2(g) à N2O4(g)

?H f 0 NO2 (g) =33.85 kJ/mol; ?Hf 0 N2O4 (g) = 9.7 kJ/mol)

A.

58 kJ

B.

-58 kJ

C.

24.2 kJ

D.

-24.2 kJ

Question

WILL GIVE MEDAL AND FAN FOR WHO EVER ANSWERS THIS! PLZZ HELP!!

Calculate ?H0for the following reaction.

2NO2(g)  à N2O4(g)

?H f 0 NO2 (g) =33.85 kJ/mol; ?Hf 0 N2O4 (g) = 9.7 kJ/mol)
	
A. 	
	
	 

58 kJ
 
	
B. 	
	
	 

-58 kJ
 
	
C. 	
	
	 

24.2 kJ
 
	
D. 	
	
	 

-24.2 kJ

anonymous · Answer

didn't you already post this?

anonymous · Answer

either way; you need to use Hess's law to solve.

anonymous · Answer

I dont know how!,

anonymous · Answer

that's all i know.... ummm

anonymous · Answer

@TuringTest  do u know this?

anonymous · Answer

@anthonysnyder200 
sorry i couldnt help :(

anonymous · Answer

@thomaster  what about u?

anonymous · Answer

anyway... i'll help the best i can :D

anonymous · Answer

http://en.wikipedia.org/wiki/Hess's_law

anonymous · Answer

http://openstudy.com/study#/updates/52fd6d45e4b0332f69f755e5 http://answers.yahoo.com/question/index?qid=20090316090322AAsllON

anonymous · Answer

idk... maybe thiis will help :( sorry :(

aaronq · Answer

it's $H_{run}=\Sigma \underbrace{\nu_i H^i_f}_{products} -\Sigma \underbrace{\nu_i H^i_f}_{reactants}$