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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 by OpenStax (2015-05-04)
Chemistry by OpenStax (2015-05-04)
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ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Chapter16: Thermodynamics
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Please help with # 39. I do not know how to solve
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) -
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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