Samples: Multiple-Choice Questions
- Given the following information:
Reaction (1): HOHO 22 __ggii+^12 " 2 ^,h ∆H°= −286 kJ
Reaction (2): CO 22 _ggi"C s^h+O _ i ∆H°= 394 kJ
Reaction (3): 2 CO 22 _gggi++H O^,h"C H 22 __ii 25 O 2 ∆H°= 1300 kJ
Find ∆H°for the reaction C 2 H 2 (g) →2 C(s) + H 2 (g).
A. −226 kJ
B. −113 kJ
C. 113 kJ
D. 226 kJ
E. 452 kJ
Answer: A
Recognize that this is a Hess’s law problem, which basically requires that you rearrange the
three reactions listed if necessary (remembering to reverse the sign of ∆H°if you reverse the
reaction) and then add up the reactions and the ∆H°’s for the answer.
Looking at the first reaction, you notice that H 2 (g) is on the wrong side. This requires that you
reverse the reaction, thus changing the sign of ∆H°. In the second reaction, C is on the correct
side of the equation, so the second equation should be left as is. In the third reaction, C 2 H 2 (g) is
on the wrong side of the equation, so the reaction and the sign of ∆H°must be reversed. At this
point the set-up should look like
HO 22 ^,h"H__ggii+ 12 / O 2 ∆H°= +286 kJ
CO 22 _gs gi"C^h+O _ i ∆H°= +394 kJ
CH 22 ___gggiii++ 52 / O 22 " 2 CO HO 2 ^,h ∆H°= −1300 kJ
Before you add up the three reactions, note that there is no CO 2 (g) in the final reaction. The 2
CO 2 (g) in the third reaction must be able to cancel with two CO 2 (g)’s in the second reaction. In
order to get 2 CO 2 (g) in the second reaction, multiply everything in the second equation by 2,
which yields
/
/
()
gg
sg
ggg
ggs
g
12
222
52 2
2
HO H O
CO C O
CH O CO HO
CH H C
22
22
22
2
2
22 2
22
"
"
"
"
,
,
+
+
++
+
^ __
^ _
___^
__^
h ii
h i
iiih
iih
H
H
H
H
kJ
kJ
kJ
∆
∆
∆
∆
286
788
1300
=+
=+
=-
=- 226 kJ
%
%
%
%
Thermochemistry