L. Using Table 1, calculate AH; for each of the following reactions. Tell if each is exothermic or endothermic. a. 2 NO(g) + 0:(8) → 2 NO:(g) b. 2 C,Hlg) + 70:(g) → 4 CO.(g) + 6 H;0(g) c. N:(g) + 3 H:(g) - 2 NH:(g) d. 2 CH;OH(1) + 3 0:(g) → 2 CO:(g) + 4 H;0(g) e. 2 SO:(g) + 0:(8) + 2 S0,(g) f. 2 CH«(g) + 30:(8) → 2 CO:(g) + 2 H;0(g) & 2 CO(g) + O:(8) → 2 CO:(g) h. N;(8) + O:[g) → 2 NO(8) II. Calculate AH, for each of the following (using Table 1). i CHxo from the reaction 2 C;H:(B) + 5 0:(g) → 4 CO:(g) + 2 H;0(g) + 600kcal i CHo from the reaction CH«(g) • 2 0:(g) CO:(g) + 2 H;0(g) + 192 kcal III. Given the following reactions k S+ 0: - So: 71.0 kcal 2 so, + 0: - 2 s0, + 47.0 kcal Calculate AH, for 2 S + 3 0: - 2 SO, L 2C + 0, - 2 co + 52.8 kcal 2 co + 0; - 2 CO; + 125 kcal Calculate AlH, for C + 0z - co: IV. Calculate AH, AS and AG at 25 C, and tell if the reaction will go spontaneously (use Table 1 and 2) m. N:(g) + 3 H:(R) → 2 NH:(8) n. 2 CO(g) + 0:(g) - 2 CO:(8) a 2 CH:(g) + 5 0:(8) - 4 CO:(8) + 2 H:0(g)
L. Using Table 1, calculate AH; for each of the following reactions. Tell if each is exothermic or endothermic. a. 2 NO(g) + 0:(8) → 2 NO:(g) b. 2 C,Hlg) + 70:(g) → 4 CO.(g) + 6 H;0(g) c. N:(g) + 3 H:(g) - 2 NH:(g) d. 2 CH;OH(1) + 3 0:(g) → 2 CO:(g) + 4 H;0(g) e. 2 SO:(g) + 0:(8) + 2 S0,(g) f. 2 CH«(g) + 30:(8) → 2 CO:(g) + 2 H;0(g) & 2 CO(g) + O:(8) → 2 CO:(g) h. N;(8) + O:[g) → 2 NO(8) II. Calculate AH, for each of the following (using Table 1). i CHxo from the reaction 2 C;H:(B) + 5 0:(g) → 4 CO:(g) + 2 H;0(g) + 600kcal i CHo from the reaction CH«(g) • 2 0:(g) CO:(g) + 2 H;0(g) + 192 kcal III. Given the following reactions k S+ 0: - So: 71.0 kcal 2 so, + 0: - 2 s0, + 47.0 kcal Calculate AH, for 2 S + 3 0: - 2 SO, L 2C + 0, - 2 co + 52.8 kcal 2 co + 0; - 2 CO; + 125 kcal Calculate AlH, for C + 0z - co: IV. Calculate AH, AS and AG at 25 C, and tell if the reaction will go spontaneously (use Table 1 and 2) m. N:(g) + 3 H:(R) → 2 NH:(8) n. 2 CO(g) + 0:(g) - 2 CO:(8) a 2 CH:(g) + 5 0:(8) - 4 CO:(8) + 2 H:0(g)
Chemistry & Chemical Reactivity
9th Edition
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Chapter5: Principles Of Chemical Reactivity: Energy And Chemical Reactions
Section: Chapter Questions
Problem 95IL: Insoluble AgCl(s) precipitates when solutions of AgNO3(aq) and NaCl(aq) are mixed. AgNO3(aq) +...
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Exergonic Reaction
The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.
Question
Transcribed Image Text:L. Using Table 1, calculate AH; for each of the following reactions. Tell if each is exothermic or
endothermic.
a. 2 NO(g) + 0:(8) → 2 NO:(g)
b. 2 C,Hlg) + 70:(g) → 4 CO.(g) + 6 H;0(g)
c. N:(g) + 3 H:(g) - 2 NH:(g)
d. 2 CH;OH(1) + 3 0:(g) → 2 CO:(g) + 4 H;0(g)
e. 2 SO:(g) + 0:(8) + 2 S0,(g)
f. 2 CH«(g) + 30:(8) → 2 CO:(g) + 2 H;0(g)
& 2 CO(g) + O:(8) → 2 CO:(g)
h. N;(8) + O:[g) → 2 NO(8)
II. Calculate AH, for each of the following (using Table 1).
i CHxo from the reaction
2 C;H:(B) + 5 0:(g) → 4 CO:(g) + 2 H;0(g) + 600kcal
i CHo from the reaction
CH«(g) • 2 0:(g)
CO:(g) + 2 H;0(g) + 192 kcal
III. Given the following reactions
k S+ 0: - So: 71.0 kcal
2 so, + 0: - 2 s0, + 47.0 kcal
Calculate AH, for 2 S + 3 0: - 2 SO,
L 2C + 0, - 2 co + 52.8 kcal
2 co + 0; - 2 CO; + 125 kcal
Calculate AlH, for C + 0z - co:
IV. Calculate AH, AS and AG at 25 C, and tell if the reaction will go spontaneously (use Table 1
and 2)
m. N:(g) + 3 H:(R) → 2 NH:(8)
n. 2 CO(g) + 0:(g) - 2 CO:(8)
a 2 CH:(g) +
5 0:(8)
- 4 CO:(8) + 2 H:0(g)
Transcribed Image Text:Compound
AH ( kcal/mol)
AH (kJ/mol)
H20(g)
-57.8
-242
H20(1)
-68.3
-285
NO(g)
NOz(g)
21.5
89.9
8.0
33.4
NH3(g)
-11.0
-46.0
NH&NOs(g)
HNO3(aq)
SO:({g)
-87.3
-365
-41.4
-173
-71.0
-297
So(g)
H2SO«(aq)
-94.5
-395
-217
-907
-26.4
CO(g)
CO2(g)
CH3OH(g)
-110
-94.1
-393
-57.0
-238
Cı2HzzO11(s)
C2H2(g)
C2H4(g)
C2H«(g)
-530
-2215
54.2
227
12.5
52.2
-20.2
-84.4
Heat of Formation of Some Common
Substances, at 25 °C and 1 atm
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