10) For a reaction that occurred at 197.0°C, the enthalpy change, AH, was found to be +26.5 kJ/mol and the free energy change, AG, was found to be - 46 kJ/mol. a. Find AS for this process as 197.0°C. b. What is the principal force that is driving this reaction in the forward direction, AS or AH? Explain. c. If the temperature of the system decreased dramatically, could this process become non-thermodynamically favored? Justify your answer.

10) For a reaction that occurred at 197.0°C, the enthalpy change, AH, was found to be +26.5 kJ/mol and the free energy change, AG, was found to be - 46 kJ/mol. a. Find AS for this process as 197.0°C. b. What is the principal force that is driving this reaction in the forward direction, AS or AH? Explain. c. If the temperature of the system decreased dramatically, could this process become non-thermodynamically favored? Justify your answer.

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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34 f and H
Calculate the standard free energy change (kJ/mol) for the reaction shown at a temperature of 298.15 K using the information provided. Reaction AHrxn (kJ/mol) ASrxn (J/mol-K) N2(g) + 2 02(g) → N204(g) 11.1 -297.6
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)
3. - the free energy under the biochemical standard states. Select all that apply. O AG O AG O AG O AG 4. is the free energy of the transition state. O AGt CAG OAG OAG"
Which of the following combinations of values for AH and AS for a given process, indicate that the process is spontaneous at all temperatures? A. O Both AH and AS are positive. B. O Both AH and AS are negative. C. O AH is positive and AS is negative. D. O AH is negative and AS is positive.
A cvg.cengagenow.com Flipgrid | 50ffc. GRLContent Netflix Favorites My Home 3-Day General.. Netflix Content [Review Topics] [References] 2req Use the References to access important values if needed for this question. 2req The free energy change for the following reaction at 25 °C, when [H*] = 7.21×10³ M and [Hg²*]=1.17 M, is 178 kJ: 2req 2H*(7.21×10-3 M) + Hg(1)→ H,(g) + Hg²*(1.17 M) AG= 178 kJ What is the cell potential for the reaction as written under these conditions? s 2req Answer: V ts 2req Would this reaction be spontaneous in the forward or the reverse direction? ots OM) pts 2reg Submit Answer Retry Entire Group 9 more group attempts remaining pts M) pts
At 25 ?C the reaction from Part A has a composition as shown in the table below. Substance Pressure (atm) 3.75 C2H2(g) H2(g) C2H6(g) 5.25x10?2 What is the free energy change, ?G, in kilojoules for the reaction under these conditions? 4.75
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
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4. Select all that is considered spontaneous a. Cleaning your room b. A piece of bread molding after being left out in the sun c. A bomb exploding d. Pushing a ball up a ramp e. Ice melting f. Frying an egg g. Putting together a puzzle
chapter 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) –241.8