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)

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Chapter1: Chemical Foundations
Section: Chapter Questions
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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: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)
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
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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