Organic Chemistry: Structure and Function
8th Edition
ISBN: 9781319079451
Author: K. Peter C. Vollhardt, Neil E. Schore
Publisher: W. H. Freeman
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Chapter 2.1, Problem 2.1E
Interpretation Introduction
Interpretation: The value of free energy change is to be calculated at
Concept introduction: The formula that determines spontaneity of the reaction is,
Where,
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For the reaction of oxygen and nitrogen to form nitric oxide, consider the following thermodynamic data:
ΔrH∘ΔrH∘
182.6kJ mol−1
ΔrS∘ΔrS∘
24.80J K−1 mol−1
T= 7363 K.
Calculate the equilibrium constant for the following reaction at room temperature, 25 ∘C∘C:?
N2(g)+O2(g)→2NO(g)
Express your answer numerically to three significant figures.
consider the following general reaction:
2A(g)+3B(s)3C(g)
if the Kc for this reaction is 10.89 at 322K, calculate the Kp
1 During an experiment with the Haber process, a researcher determined that Kc =9,60 at 300°C.N2 (g) + 3 H2 (g) ↔ 2 NH3 (g)Calculate Kp for this reaction at 300°C.
Chapter 2 Solutions
Organic Chemistry: Structure and Function
Ch. 2.1 - Prob. 2.1ECh. 2.1 - Prob. 2.2ECh. 2.1 - Prob. 2.3ECh. 2.1 - Prob. 2.5TIYCh. 2.1 - Prob. 2.6ECh. 2.1 - Prob. 2.7ECh. 2.2 - Prob. 2.8ECh. 2.3 - Prob. 2.9ECh. 2.3 - Prob. 2.10ECh. 2.3 - Prob. 2.11E
Ch. 2.3 - Prob. 2.12ECh. 2.3 - Prob. 2.13ECh. 2.3 - Prob. 2.14ECh. 2.3 - Prob. 2.15ECh. 2.3 - Prob. 2.17TIYCh. 2.3 - Prob. 2.19TIYCh. 2.5 - Prob. 2.20ECh. 2.6 - Prob. 2.21ECh. 2.6 - Prob. 2.22ECh. 2.6 - Prob. 2.23ECh. 2.6 - Prob. 2.25TIYCh. 2.7 - Prob. 2.26ECh. 2.9 - Prob. 2.28TIYCh. 2 - Prob. 31PCh. 2 - Prob. 32PCh. 2 - Prob. 33PCh. 2 - Prob. 34PCh. 2 - Prob. 35PCh. 2 - Prob. 36PCh. 2 - Prob. 37PCh. 2 - Prob. 38PCh. 2 - Prob. 39PCh. 2 - Prob. 40PCh. 2 - Prob. 41PCh. 2 - Prob. 42PCh. 2 - Prob. 43PCh. 2 - Prob. 44PCh. 2 - Prob. 45PCh. 2 - Prob. 46PCh. 2 - Prob. 47PCh. 2 - Prob. 48PCh. 2 - Prob. 49PCh. 2 - Prob. 50PCh. 2 - Prob. 51PCh. 2 - Prob. 52PCh. 2 - Prob. 53PCh. 2 - Prob. 54PCh. 2 - Prob. 55PCh. 2 - Prob. 56PCh. 2 - Prob. 57PCh. 2 - Prob. 58PCh. 2 - Prob. 59PCh. 2 - Prob. 60PCh. 2 - Prob. 61PCh. 2 - Prob. 62PCh. 2 - Prob. 63PCh. 2 - Prob. 64PCh. 2 - Prob. 65PCh. 2 - Prob. 66P
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- a Calculate K1, at 25C for phosphoric acid: H3PO4(aq)H+(aq)+H2PO4(aq) b Which thermodynamic factor is the most significant in accounting for the fact that phosphoric acid is a weak acid? Why ?arrow_forwarda Calculate K1, at 25C for sulfurous acid: H2SO3(aq)H+(aq)+HSO3(aq) b Which thermodynamic factor is the most significant in accounting for the fact that sulfurous acid is a weak acid? Why?arrow_forwardConsider the reaction 2SO2(g)+O2(g)2SO3(g) (a) Calculate G at 25C. (b) If the partial pressures of SO2 and SO3 are kept at 0.400 atm, what partial pressure should O2 have so that the reaction just becomes nonspontaneous (i.e., G=+1.0 k J)?arrow_forward
- What information can be determined from G for a reaction? Does one get the same information from G, the standard free energy change? G allows determination of the equilibrium constant K for a reaction. How? How can one estimate the value of K at temperatures other than 25C for a reaction? How can one estimate the temperature where K = 1 for a reaction? Do all reactions have a specific temperature where K = 1?arrow_forwardFor the Haber process, N2(g) + 3 H2(g) = 2 NH3(g) Kc = 9.60 at 300 °C. Calculate Kp for this reaction at this temperature.arrow_forwardBelow is information for the reaction 2NO2(g) --> O2(g)+2NO(g) NO2(g) O2(g) NO(g) H (kJ/mol) 33.2 0 90.2 S (J/K) 240.1 0 210.76 a) Calculate the Gibbs-Free Energy, G, for the reaction at 5000K b) What is the spontaneity of the reaction at 5000K?arrow_forward
- During an experiment with the Haber process, a researcher determined that Kc=9.60 at 300°c N2(g)+3H2(g)____2NH3(g) Calculate Kp for this reaction at 300°carrow_forwardA reaction A(aq)+B(aq)−⇀↽−C(aq) has a standard free‑energy change of −4.65 kJ/mol at 25 °C. What are the concentrations of A, B, and C at equilibrium if, at the beginning of the reaction, their concentrations are 0.30 M, 0.40 M, and 0 M, respectively? [B]= M [A]= M [C]= M How would your answers change if the reaction had a standard free‑energy change of +4.65 kJ/mol? All concentrations would be higher. There would be no change to the answers. There would be less A and B but more C. There would be more A and B but less C. All concentrations would be lower.arrow_forwardreaction A(aq)+B(aq)↽−−⇀C(aq)A(aq)+B(aq)↽−−⇀C(aq) has a standard free‑energy change of −3.47 kJ/mol−3.47 kJ/mol at 25 °C.25 °C. What are the concentrations of A,A, B,B, and CC at equilibrium if, at the beginning of the reaction, their concentrations are 0.30 M,0.30 M, 0.40 M,0.40 M, and 0 M,0 M, respectively? [A]=[A]= MM [B]=[B]= MM [C]=[C]= MM How would your answers change if the reaction had a standard free‑energy change of +3.47 kJ/mol?+3.47 kJ/mol? There would be no change to the answers. All concentrations would be lower. There would be less AA and BB but more C.C. There would be more AA and BB but less C.C. All concentrations would be higher.arrow_forward
- Consider the following reaction at 25 °C: 3 Ni(s) + N₂(g) + 3 H₂O(g) → 3 NiO(s) + 2 NH₃(g) If ∆H° = -85.7 kJ/mol and ∆S° = -348.3 J/mol•K, determine the standard free energy for the reaction at 25 °C.arrow_forwardCalculate Kp for the following reaction at the given temperature. Give your answer to three sig figs 2A(g) + B (g) <--> 3C(g) + 2D (g) Kc= 0.0273 at 234 Karrow_forwardThe thermodynamic values from part A will be useful as you work through part B: ΔH∘rxn 243.5kJ/mol ΔS∘rxn 172.0J/(mol⋅K) Calculate the equilibrium constant for the following reaction at room temperature, 25 ∘C BaCO3(s)→BaO(s)+CO2(g)arrow_forward
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