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, Problem 32P
(a)
Interpretation Introduction
Interpretation: The value of
Concept introduction: The formula to calculate
(b)
Interpretation Introduction
Interpretation: The value of
Concept introduction: The formula that determines spontaneity of the reaction is,
Where,
(c)
Interpretation Introduction
Interpretation: The value of
Concept introduction: The formula that determines spontaneity of the reaction is,
Where,
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(a) Calculate the value of Kc for the reaction:
PCl5 (g) PCl3 (g) + Cl2 (g) ΔH = Positive
Given that when 8.4 mol of PCl5 (g) is mixed with 1.8 mol of PCl3 (g) and allowed to come to equilibrium in a 10 dm3container the amount of PCl5 (g) at equilibrium is 7.2 mol.
Kc =
(b) Explain the effect of the following changes below on the value of Kc:
Increasing temperature
Lowering the concentration of chlorine (Cl2)
Addition of a catalyst
The ΔHvap of a certain compound is 22.52 kJ·mol-1 and its ΔSvap is 56.75 J·mol-1·K -1.
What is the boiling point of this compound?
The Δ?vapΔHvap of a certain compound is 19.52 kJ·mol−1 and its ΔSvap is 81.67 J·mol−1·K−1.
What is the boiling point of this compound?
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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- Calculate ΔH for the following reaction: CH4 (g) + O2 (g) ⇌ CO2 (g) + H2O (l) Compound ΔH CH4 (g) -74.8 kJ/mol H2O (l) -285.8 kJ/mol CO2 (g) -393.5 kJ/moarrow_forwarda) As stated in question 5a, glucose (C6H12O6(s)) is a source of cellular energy. Calculate the standard free energy for the metabolism of glucose: Given ΔG°C6H12O6(s) = -911kJ/mol; ΔG°O2(g) = 0kJ/mol; ΔG°CO2 = -394kJ/mol; ΔG°H2O(l) = -237kJ/molC6H12O6(s) + 6O2(g) ➝ 6CO2(g) + 6H2O(l) b) Cells couple the hydrolysis of adenosine triphosphate (ATP) into adenosine diphosphate (ADP) andinorganic phosphate (PO43–) to drive chemical reactions (i.e. as a source of chemical energy). The reaction is: ATP(aq) + H2O(l) ➝ ADP(aq) + PO43–(aq) Calculate K for this reaction if ΔG° = –30.5 kJ/mole. c) If all of the energy from glucose metabolism went into ATP synthesis from ADP and inorganicphosphate, how many molecules of ATP could be generated from each molecule of glucose?arrow_forwardYou have a calorimeter with a heat capacity of 0.426 kJ/ºC. You combine 50.0 mL 1.50 M NaA (A- = conjugate base of weak acid HA) with an equal volume of HCl of higher molarilty. The temperature changes from 18.6 ºC to 21.1 ºC. What is ΔHºdissoc for the dissociation reaction of HA, in kJ?arrow_forward
- Assuming that neither standard enthalpy changes of formations (∆Hof) nor standard molar entropies (So) depend upon temperature, estimate using the Table of Thermodynamic Data : (a) the standard Gibbs free energy change for the reaction that forms rhombic sulfur at 600 K, and (b) the temperature (in oC) at which reaction will stop formation of products: 2H2S(g) + SO2(g) → 3S(rhombic, s) + 2H2O(g) Round off your answers to the nearest integer. Report the temperature in oC. and enter them with correct units: (a)∆Gorxn = (b) T =arrow_forwardWhy is ΔTmetal < 0? Why is ΔTwaterarrow_forward[2] [a] The forward reaction is spontaneous for a particular reversible reaction. What can you conclude about the reverse reaction? AG = [b] What does the sign of the free energy have to be such that a reaction is spontaneous? AS = [c] [i] Under what conditions of enthalpy and entropy change is a reaction always spontaneous? AH= [ii] Under what conditions of enthalpy and entropy change is a reaction never spontaneous? - ΔΗ AS [d] If the entropy change is unfavorable for a certain reaction, is the reaction more likely to be spontaneous at a high temperature or a low temperature? [e] If the enthalpy change is unfavorable, but the entropy change is favorable, would a high temperature or a low temperature be more likely to lead to a spontaneous reaction?arrow_forward
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