1) 1 Cu2O(s)+ (1/2)O2(g) -> 2CuO(s) Change in H = -144 kj

2 Cu2O(s) -> Cu(s) + CuO(s) Change in H = +11

Calculate the standard enthalpy of formation of CuO

 

This is what i did, i reversed the 2nd equation so i get Cu(s) + CuO(s) -> Cu2O(s) by applying hess law, and Change in H becomes -11, then i added both equation 1 and 2 and got Cu(s)+(1/2)O2 -> CuO(s) after balancing, and the standard enthalpy becomes -144 kj - 11 kj which equals -155 kj.. Did i do this problem correctly?

 

The following questions i got wrong and i have no idea why...

 

1) Calculate the S*net for the following reaction, Given the S* vales: Na(s)=51.4 e.u, H20 (l) = 69.9 e.u , Na+ (aq) = 60.2 e.u., OH- (aq) = -10.5 e.u. H2(g) = 130.6

Reaction = Na(s) + H20(l) <---> Na+(aq) +OH- + H2(g)

 

This is how i solved it.. After balancing the equation, i got Na(s)+2H2O(l)<----> Na+(aq) +2OH- +H2(g)...And S*net = products - reactans, and after plugging it all in i got (60.2-2(10.5)+130.6) - (51.4 +2(69.9) which is -21.4 e.u. However, my answer was wrong and the answer was -12.6 e.u. How the heck did the professor get -12.6 ??

 

2) For the process:

benzene(l) --(1 atm)--> benzene (g), Change in Enthalpy = 30.5 kj/mol

Change in S*vap=86.4 J/mol*K

 

Assuming these vales are independent of T, what is the normal boiling point of benzene?

 

This is how i solved it, since it is in 1 atm , it is simply Change in enthalpy - T*change in entropy= Change in G (free energy) = 0

 

0 = Change in H - T*Change in S

 

After plugging it in.. 0 = 30,500 J/mol*k - T(86.4 J/mol*k) = 0

 

Solving for T you get 353degree Celcius..BUt that is not the answer, the answer is 80 degree celcius.. Where did i go wrong?

2) Solving for T, you actually get 353 K. Then, 353 - 273 = 80 C.