39. Calculate AG for each of the following reactions from the equilibrium constant at the temperature given. (a) N₂(g) + O2 (8) → 2NO(g) T = 2000 °C Kp =4.1 × 10-4 (b) H₂(g) + 12 (8) 2HI(g) T = 400 °C Kp = 50.0 (c) CO2 (g) + H₂(g) T = 980 °C Kp = 1.67 (d) CaCO3(s) -> CaO(s)+CO2(g) T = 900 °C Kp = 1.04 T = 25 °C (e) HF(aq) + H₂O(1) -> H3O+ (aq) + F(aq) Ag+ (aq) + Br(aq) (f) AgBr(s) T = 25 °C - - - CO(g) + H₂O(g) Kp = 7.2 × 10-4 Kp = 3.3 × 10-13
39. Calculate AG for each of the following reactions from the equilibrium constant at the temperature given. (a) N₂(g) + O2 (8) → 2NO(g) T = 2000 °C Kp =4.1 × 10-4 (b) H₂(g) + 12 (8) 2HI(g) T = 400 °C Kp = 50.0 (c) CO2 (g) + H₂(g) T = 980 °C Kp = 1.67 (d) CaCO3(s) -> CaO(s)+CO2(g) T = 900 °C Kp = 1.04 T = 25 °C (e) HF(aq) + H₂O(1) -> H3O+ (aq) + F(aq) Ag+ (aq) + Br(aq) (f) AgBr(s) T = 25 °C - - - CO(g) + H₂O(g) Kp = 7.2 × 10-4 Kp = 3.3 × 10-13
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Please help with # 39.
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![state conditions?
37. Consider the decomposition of red mercury(II) oxide under standard state conditions.
2HgO(s, red) → 2Hg(1) + O₂(g)
(a) Is the decomposition spontaneous under standard state conditions?
(b) Above what temperature does the reaction become spontaneous?
38. Among other things, an ideal fuel for the control thrusters of a space vehicle should decompose in a
spontaneous exothermic reaction when exposed to the appropriate catalyst. Evaluate the following
substances under standard state conditions as suitable candidates for fuels.
(a) Ammonia: 2NH3(g)
(b) Diborane: B₂ H6 (g)
(c) Hydrazine: N₂ H4 (8)
-
(d) Hydrogen peroxide: H₂O₂ (1)
→
N₂(g) + 3H₂(g)
2B(g) + 3H₂(g)
N₂ (8) + 2H₂(g)
→
39. Calculate AG for each of the following reactions from the equilibrium constant at the temperature given.
(a) N₂(g) + O2 (8)
2NO(g)
T = 2000 °C
(b) H₂(g) + 12 (8)
Kp =4.1 × 10-4
Kp = 50.0
T = 400 °C
T = 980 °C
(c) CO₂(g) + H₂(g) → CO(g) + H₂O(g)
(d) CaCO3(s) ->> CaO(s)+CO2(g)
Kp = 1.67
T = 900 °C
Kp = 1.04
(e) HF(aq) + H₂O(1)
Kp = 7.2 × 10-4
T = 25 °C
T = 25 °C
(f) AgBr(s) → Ag+ (aq) + Br(aq)
Kp = 3.3 X 10-13
40. Calculate AG° for each of the following reactions from the equilibrium constant at the temperature given.
(a) Cl₂(g) + Br₂(g) → 2BrCl(g)
T = 25 °C
Kp=4.7 × 10-2
Kp = 48.2
2SO3 (8)
T = 500 °C
T = 60 °C
Kp = 0.196
T = 550 °C
Kp = 4.90 × 10²
CH3NH3 + (aq) + OH¯ (aq)
T = 25 °C
Kp =4.4 × 10-4
(e) CH3NH₂ (aq) + H₂O(1)
(f) Pbl₂ (s)
T = 25 °C
→ Pb²+ (aq) + 21- (aq)
Kp = 8.7 × 10-9
41. Calculate the equilibrium constant at 25 °C for each of the following reactions from the value of AG° given.
AG = -9.2 kJ
(a) O₂(g) + 2F2 (g) 20F2 (g)
(b) I2 (s) + Br2 (1)
21Br(g)
AG = 7.3 kJ
2HI(g)
→
H₂O(g) + 02 (8)
bus at room temperature under standard
H3O+ (aq) + F(aq)
(b) 2SO2(g) + O2 (8) =
(c) H₂O(l): = H₂O(g)
(d) CoO(s)+CO(g) = Co(s)+CO2(g)
-](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fdbf8765a-c0ab-46fe-8663-61e338d72b7c%2Fc5e875f1-25c4-4da6-9199-b65e27ff1db8%2Fpi5u6x7_processed.jpeg&w=3840&q=75)
Transcribed Image Text:state conditions?
37. Consider the decomposition of red mercury(II) oxide under standard state conditions.
2HgO(s, red) → 2Hg(1) + O₂(g)
(a) Is the decomposition spontaneous under standard state conditions?
(b) Above what temperature does the reaction become spontaneous?
38. Among other things, an ideal fuel for the control thrusters of a space vehicle should decompose in a
spontaneous exothermic reaction when exposed to the appropriate catalyst. Evaluate the following
substances under standard state conditions as suitable candidates for fuels.
(a) Ammonia: 2NH3(g)
(b) Diborane: B₂ H6 (g)
(c) Hydrazine: N₂ H4 (8)
-
(d) Hydrogen peroxide: H₂O₂ (1)
→
N₂(g) + 3H₂(g)
2B(g) + 3H₂(g)
N₂ (8) + 2H₂(g)
→
39. Calculate AG for each of the following reactions from the equilibrium constant at the temperature given.
(a) N₂(g) + O2 (8)
2NO(g)
T = 2000 °C
(b) H₂(g) + 12 (8)
Kp =4.1 × 10-4
Kp = 50.0
T = 400 °C
T = 980 °C
(c) CO₂(g) + H₂(g) → CO(g) + H₂O(g)
(d) CaCO3(s) ->> CaO(s)+CO2(g)
Kp = 1.67
T = 900 °C
Kp = 1.04
(e) HF(aq) + H₂O(1)
Kp = 7.2 × 10-4
T = 25 °C
T = 25 °C
(f) AgBr(s) → Ag+ (aq) + Br(aq)
Kp = 3.3 X 10-13
40. Calculate AG° for each of the following reactions from the equilibrium constant at the temperature given.
(a) Cl₂(g) + Br₂(g) → 2BrCl(g)
T = 25 °C
Kp=4.7 × 10-2
Kp = 48.2
2SO3 (8)
T = 500 °C
T = 60 °C
Kp = 0.196
T = 550 °C
Kp = 4.90 × 10²
CH3NH3 + (aq) + OH¯ (aq)
T = 25 °C
Kp =4.4 × 10-4
(e) CH3NH₂ (aq) + H₂O(1)
(f) Pbl₂ (s)
T = 25 °C
→ Pb²+ (aq) + 21- (aq)
Kp = 8.7 × 10-9
41. Calculate the equilibrium constant at 25 °C for each of the following reactions from the value of AG° given.
AG = -9.2 kJ
(a) O₂(g) + 2F2 (g) 20F2 (g)
(b) I2 (s) + Br2 (1)
21Br(g)
AG = 7.3 kJ
2HI(g)
→
H₂O(g) + 02 (8)
bus at room temperature under standard
H3O+ (aq) + F(aq)
(b) 2SO2(g) + O2 (8) =
(c) H₂O(l): = H₂O(g)
(d) CoO(s)+CO(g) = Co(s)+CO2(g)
-
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