Explain why each of the following statements is incorrect. a. Entropy increases in all spontaneous reactions. Ot's not the entropy of system, but the entropy of universe, that increases in all spontaneous reactions. Olt's not the entropy of system, but the entropy of surroundings, that increases in all spontaneous reactions. Ot's incorrect because entropy decreases in all spontaneous reactions. b. Reactions with a negative free energy change (A,G° < 0) are product-favored and occur with rapid transformation of reactants to products. O4,G° tells only about equilibrium state, not about the rate it establishes. OReactions with a negative free energy change are reactant-favored. OIf A;G° is rather close to zero (but still negative), the transformation won't be rapid. c. All spontaneous processes are exothermic. Endothermic processes with positive entropy change can also be spontaneous. All spontaneous processes are endothermic. O Endothermic processes with negative entropy change can also be spontaneous.

Explain why each of the following statements is incorrect. a. Entropy increases in all spontaneous reactions. Ot's not the entropy of system, but the entropy of universe, that increases in all spontaneous reactions. Olt's not the entropy of system, but the entropy of surroundings, that increases in all spontaneous reactions. Ot's incorrect because entropy decreases in all spontaneous reactions. b. Reactions with a negative free energy change (A,G° < 0) are product-favored and occur with rapid transformation of reactants to products. O4,G° tells only about equilibrium state, not about the rate it establishes. OReactions with a negative free energy change are reactant-favored. OIf A;G° is rather close to zero (but still negative), the transformation won't be rapid. c. All spontaneous processes are exothermic. Endothermic processes with positive entropy change can also be spontaneous. All spontaneous processes are endothermic. O Endothermic processes with negative entropy change can also be spontaneous.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

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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2&3
A. The Second Law of Thermodynamics Calculate the entropy change, ASºuniverse for the following reaction at 25°C. CO (g) + 2H2 (g) - CH3OH (1) Standard entropy, S° : CO (g) = 197.7 J/mol-K H2 (g) = 130.7 J/mol-K CH3OH (I) = 127.2 J/mol-K %3D %3D %3D Standard enthalpy of formation, AH,º : CO (g) = -110.5 kJ/mol H2 (g) = 0 CH3OH (I) = -238.4 kJ/mol %3D %3D %3D
Which substance has the higher entropy? a. a sample of pure silicon (to be used in a computer chip) or a piece of silicon containing a trace of another element such as boron or phosphorus a piece of silicon containing a trace of another element such as boron or phosphorus a sample of pure silicon b. CO2(g) at 0 °C or CO2 (g) at -50 °C O CO2 (g) at –50 °C O CO2 (g) at 0 °C c. I2 (s) or I2 (g) both at room temperature OL (g) OL (s) d. one mole of CO2(g) at 1 bar pressure or one mole of CO2(g) at 0.01 bar pressure (both at 298 K) one mole of CO2(g) at 0.01 bar pressure one mole of CO2(g) at 1 bar pressure
5. Consider the combustion reaction of octane (C8H18, mol. wt. = 114.23 g/mol, density = 0.703 g/mL). a. Write out the balanced chemical equation for this reaction. All products are in the gas phase. 2 C8H18 + 25 O2 ---> 16 CO2 + 18 H2O b. Calculate the standard free energy (in kJ/mol) released in this reaction. ∆Hfo (kJ/mol) Sfo (J/K mol) Octane(l) ─208.4 463.7 H2O(g) ─242 189 02 0 205 CO2(g) ─393.5 214 c. Making the approximation that gasoline consists of 100% octane, how much energy would 1.00 gallon of gasoline release? (1 quart = 946 mL, 1 gallon = 4 quarts)
Given the following enthalpy and entropy values, determine which reactions would not violate the 2nd law of thermodynamics at 298K. A. Enthalpy = -84 KJ/mole Entropy = 125 J/mol B. Enthalpy = -84 KJ/mol Entropy = -125 J/mol C. Enthalpy = 84 KJ/mol Entropy = 125 J/mol D. Enthalpy = 84 Kj/mol Entropy = -125 J/mol
4. Determine whether the hydrogenation of propene gas reaction at 298 is spontaneous or nonspontaneous by calculating AG C,H, (g) + H, (g) → CH, (1) Enthalpy of formation Entropy C,H, 267 J/mol*K 20.6kJ/mole. C,H, 270.2 J/mol*K-103.9 kJ/mol.
Now calculate the change in entropy (delta S) for the following reaction, using the thermodynamic tables P4 (g) + 10 Cl2 (g) → 4 PCl5 (g) a. 1412 J/K b. – 1.50 x 10^2 J/K c. – 856 J/K d. 2510 J/K e. – 113 J/K f. – 1098 J/K g. 3922 J/K h. 856 J/K i. none of these
Part b-- Standard entropy = 205 J/mol K
The answer may be One or more than One options Choose statements that describe ΔStotal ≥ 0. When we say that entropy is constant or unchanging, it may have infinitesimally small fluctuations about its average value. You may want to consult the entropy handout from Week 5. a. During a reversible process, the entropy of any systems is constant. b. The entropy of an isolated system at equilibrium is constant. c. As an isolated system relaxes to an equilibrium state its entropy increases. d. During an irreversible process, the entropy of any system increases. e. During an irreversible process, the entropy of an isolated system decreases. f. During a reversible process, the entropy of an isolated system is constant.
9
a. Calculate ΔH°f for methane (you will need to dust off Hess’s Law for this one, and recall that the heat of formation, ΔH°f , is the amount of energy required to form 1 mol of a substance from the elements under standard conditions- start by writing a balanced equation for this process.). b. From appropriate entropy data, calculate ΔS°f for methane. c. Use the above information to calculate ΔG°f for methane. d. Compare your results from part C with the reported ΔG°f for methane
A) for the reaction MgCo3(s) ---> MgO (s) +CO2 we can say that it is a reaction a. spontaneous b. not spontaneous c.in balance d. indeterminate B) Which substance in the following pair of compounds must have the highest standard molar entropy? C2H2 (g) or C2H6(g) a.C2H2(g) b.C2H6 c.C2H2=C2H6(g) d. undetermined