Organic Chemistry
4th Edition
ISBN: 9780077479824
Author: SMITH, Janice Gorzynski/
Publisher: McGraw-Hill College
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Textbook Question
Chapter 6, Problem 6.9P
Given each of the following values, is the starting material or product lower in energy?
a.
b.
c.
d.
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Consider the balanced reaction:
2Cr3+(aq)+3PbO2(s)+6H2O(l)→2CrO42-(aq)+3Pb2+(aq)+4H3O+ (aq)
d.How many valence electrons are in the CrO42- ion?
e. How many moles of electrons, ne, are transferred per mole of this reaction?
f. At a certain point the measured free energy is ∆G. Adding more PbO2 will cause the free energy change of the reaction, ∆G, to choose...(Increase, Stay the same, Decrease)
What is the free energy change for the reaction below?
2VO2+(aq) + 4H+(aq) + Ni(s) ® 2VO2+(aq) + 2H2O(l) + Ni(s)
E� = 1.23V
118.68 kJ
237.35 kJ
-237.35 kJ
-118.68 kJ
Calculate the standard free-energy changes for the following reactions at 25°C.
a. CH4(g) + 2O2(g) → CO2(g) + 2H2O(l)
b. 2MgO(s) → 2Mg(s) + O2(g)
Chapter 6 Solutions
Organic Chemistry
Ch. 6 - Prob. 6.1PCh. 6 - By taking into account electronegativity...Ch. 6 - Use curved arrows to show the movement of...Ch. 6 - Prob. 6.4PCh. 6 - Prob. 6.5PCh. 6 - Prob. 6.6PCh. 6 - aWhich Keq corresponds to a negative value of G,...Ch. 6 - Given each of the following values, is the...Ch. 6 - Given each of the following values, is the...Ch. 6 - The equilibrium constant for the conversion of the...
Ch. 6 - Prob. 6.11PCh. 6 - For a reaction with H=40kJ/mol, decide which of...Ch. 6 - For a reaction with H=20kJ/mol, decide which of...Ch. 6 - Draw an energy diagram for a reaction in which the...Ch. 6 - Prob. 6.15PCh. 6 - Prob. 6.16PCh. 6 - Problem 6.19 Consider the following energy...Ch. 6 - Draw an energy diagram for a two-step reaction,...Ch. 6 - Which value if any corresponds to a faster...Ch. 6 - Prob. 6.20PCh. 6 - Problem 6.23 For each rate equation, what effect...Ch. 6 - Prob. 6.22PCh. 6 - Identify the catalyst in each equation. a....Ch. 6 - Draw the products of homolysis or heterolysis of...Ch. 6 - Explain why the bond dissociation energy for bond...Ch. 6 - Classify each transformation as substitution,...Ch. 6 - Prob. 6.27PCh. 6 - Draw the products of each reaction by following...Ch. 6 - Prob. 6.29PCh. 6 - Prob. 6.30PCh. 6 - Prob. 6.31PCh. 6 - Prob. 6.32PCh. 6 - Prob. 6.33PCh. 6 - Prob. 6.34PCh. 6 - Prob. 6.35PCh. 6 - 6.39. a. Which value corresponds to a negative...Ch. 6 - Prob. 6.37PCh. 6 - At 25 C, the energy difference Go for the...Ch. 6 - For which of the following reaction is S a...Ch. 6 - Prob. 6.40PCh. 6 - Prob. 6.41PCh. 6 - 6.44 Consider the following reaction: .
Use curved...Ch. 6 - Prob. 6.43PCh. 6 - Draw an energy diagram for the Bronsted-Lowry...Ch. 6 - Prob. 6.45PCh. 6 - Prob. 6.46PCh. 6 - Prob. 6.47PCh. 6 - Prob. 6.48PCh. 6 - The conversion of acetyl chloride to methyl...Ch. 6 - Prob. 6.50PCh. 6 - Prob. 6.51PCh. 6 - 6.54 Explain why is more acidic than , even...Ch. 6 - Prob. 6.53PCh. 6 - Prob. 6.54PCh. 6 - Prob. 6.55PCh. 6 - Although Keq of equation 1 in problem 6.57 does...Ch. 6 - Prob. 6.57P
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- Which of the following reactions corresponds to the reaction corresponding to a free energy of formation, ΔGfo? Group of answer choices.... 6 C(l) + 11 H2(g) + 11 O(g) → C6H22O11(s) P(g) + 4 H(g) + Br(g) → PH4Br(l) 6 C(s) + 6 H(g) → C6H6(l) 1/2 N2(g) + O2(g) → NO2(g) 2 N2(g) + 4 H2(g) + 3 O2(g) → 2 NH4NO3(s)arrow_forwardA reaction has a standard free‑energy change of −14.80 kJ mol−1(−3.537 kcal mol−1). Calculate the equilibrium constant for the reaction at 25 °C.arrow_forwardThe change of state from gaseous H2O to liquid H2O has a ΔH of -9.72 kcal/mol and a ΔS of -26.1 cal/(mol·K). What is the change in free energy of this reaction at 200K?arrow_forward
- Which of these reactions or processes has a negative DS? (D = delta) (A) C2H5OH(l) --> C2H5OH(g) (B) 2NO2(g) --> 2NO(g) + O2(g) (C) NH3(g) --> NH3(aq) (D) H2(g) + F2(g) --> 2HF(g)arrow_forwardThe reaction CBr4(g) + H2(g) → CHBr3(g) + HBr(g) occurs at room temperature (20oC) with ΔHo = -137.8 kJ and ΔSo = −55.0 J/K. What is ΔSuniverse (in J/K.mol) for this reaction?arrow_forward1. Predict the sign of ∆S for the following reaction. a. negativeb. positivec. no change 2. What is an intermediate? a.A local maximum on the energy diagram. b. A point on the reaction pathway that has a discrete minima. c.A point half-way between the starting materials and products. d. The highest energy compound on an energy diagram.arrow_forward
- Consider the following reaction (rxn): A → C ΔG < 0 Which of the following MUST be true? I. The reaction is fast II. The reaction is spontaneous in the forward direction III. The equilibrium constant K > 1 IV. ΔSrxn > 0arrow_forwardWhen the reaction A + B ⇌ C is at equilibrium, the concentrations of reactants are as follows: [A] = 2 mM, [B] = 3 mM, and [C] = 9 mM. What is the standard free energy change for the reaction?arrow_forwardCalculate ∆S° for the following reactions in J K-1 a. 2 C2H6(g) + 7 O2(g) → 4 CO2(g) + 6 H2O(g)b. Ca(OH)2(s) + H2SO4(l) → CaSO4(s) + 2 H2O(l)arrow_forward
- Find the pKw of H2O and D2O at 60°C and 90°C (values in image). Write the balanced chemical reactions that pertain to these K values (values in image).arrow_forwardThe standard free energy change for the reaction CH4(g)+2O2(g) -> CO2(g) + 2H2O(l) is -194.8 kcal at 25ºC and -191.82 kcal at 75ºC. Calculate the heat of reaction at 25ºC.Ans: -212.6 kcalarrow_forwardchapter 12: 8) Calculate the free-energy change of the following reaction at 448°C and standard pressure. Values in the table are at standard pressure and 25°C. C2H4(g)+3O2(g)--->2CO2(g)+2H2O(g) ΔHºf,(kJ/mol) Sºf, J/mol•K ΔGºf, kJ/mol C2H4(g) 52.3 219.5 68.1 O2(g) 0 205.0 0 CO2(g) –393.5 213.6 –394.4 H2O(g) –241.8arrow_forward
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