[Review Topics][References]Use the References to access important values if needed for this question.The free energy change for the following reaction at 25 °C, when [Co2+] = 1.14 M and [Cr*] = 8.46×10-³ M, is -279 kJ:3C02*(1.14 M) + 2Cr(s)3Co(s) + 2Cr**(8.46x103 M) AG = -279 kJWhat is the cell potential for the reaction as written under these conditions?Answer:Would this reaction be spontaneous in the forward or the reverse direction?9 more group attempts remainingSubmit AnswerRetry Entire Group

The negative value of free energy change indicates that the reaction is proceeding spontaneously…

Answered: [Review Topics] [References] Use the…

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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Consider the reaction H2(g) + Cl2(g)- →2HCI(g) Use the standard thermodynamic data in the tables linked above. Calculate AG for this reaction at 298.15K if the pressure of HCl(g) is reduced to 14.82 mm Hg, while the pressures of H2(g) and Cl2(g) remain at 1 atm. ANSWER: kJ/mol
Predicting and FULLY explain if the following reaction will be spontaneous proceed to products, or non-spontaneous, or will reach equilibrium?
TReferences] Use the References to access important values if needed for this question. The free energy change for the following reaction at 25 °C, when [Cr= 6.98x10 M and (Ni) = 1.15 M, is 296 kJ: %3! 2Cr"(6.98x10 M) + 3Ni(s)- 2Cr(s) + 3NI*(1.15 M) AG = 296 kJ What is the cell potential for the reaction as written under these conditions? Answer: Would this reaction be spontaneous in the forward or the reverse direction forward reverse
For the reaction 2HBr (9) + Cl₂ (9) - 4 2HCl(g) + Br₂ (9) =-1.2 J/K AH-81.1 kJ and AS = - The standard free energy change for the reaction of 1.52 moles of HBr (g) at 318 K, 1 atm would be [ This reaction is favored under standard conditions at 318 K. Assume that AH and AS are independent of temperature. Submit Answer Retry Entire Group 3 more group attempts remaining kj.
Calculate the standard free-energy changes for the following reactions at 25°C. (a) CH4(g) + 20ztg) → CO2(g) + 2H20(1) (b) 2Mg0(s) → 2Mg(s) + Oz(g)
99+ [References] Use the References to access important values if needed for this question. Consider the reaction H₂(g) + Cl₂(g) →→→→2HCI(g) Use the standard thermodynamic data in the tables linked above. Calculate AG for this reaction at 298.15K if the pressure of HCI(g) is reduced to 13.25 mm Hg, while the pressures of H₂(g) and Cl₂(g) remain at 1 atm. ANSWER: Submit Answer B kJ/mol Try Another Version 1 item attempt remaining Previous Next 3:18 AM 11/22/2022
Consider the reaction CO(g) + Cl₂(g) →COCI₂(g) Use the standard thermodynamic data in the tables linked above. Calculate AG for this reaction at 298.15K if the pressure of COCl₂(g) is reduced to 17.43 mm Hg, while the pressures of CO(g) and Cl₂(g) remain at 1 atm. ANSWER: kJ/mol
[Review Topics] [References] Use the References to access important values if needed for this question. A student determines the value of the equilibrium constant to be 1.21x1012 for the following reaction. CO(g) + Cl2(g)- COC12(g) Based on this value of Keg AG° for this reaction is expected to be (greater,less) than zero. Calculate the free energy change for the reaction of 1.65 moles of CO(g) at standard conditions at 298K. AG rxn kJ
[Review Topics] [References] Use the References to access important values if needed for this question. Consider the reaction: H,S(g) + 2H,O()→3H2(g) + SO,(g) Using standard thermodynamic data at 298K, calculate the free energy change when 2.44 moles of H,S(g) react at standard conditions. AG°xn kJ Submit Answer Retry Entire Group 9 more group attempts remaining Previous Next Save a P W étv MacBook Air DII DD F11 F10 F9 F7 F8 F5 F6 F4 * & $ 7 8 9. 4 { R Y
Consider the reaction N₂(g) + 20₂(g)- >2NO₂(g) Use the standard thermodynamic data in the tables linked above. Calculate AG for this reaction at 298.15K if the pressure of NO₂(g) is reduced to 16.22 mm Hg, while the pressures of N₂(g) and O₂(g) remain at 1 atm. ANSWER: I kJ/mol
Calculate AG° for the reaction shown below using the provided thermodynamic properties information. H2O2 (1) → 2 H2O () + O2 (g) Substance AH°; (kJ/mol) AS° (J/(mol•K)) H2O2 (1) - 187.8 232.9 H20 (1) -285.83 69.91 O2 (g) 205.0 -396.4 kJ/mol -350.5 kJ/mol -33.70 kJ/mol -1105 kJ/mol -417.2 kJ/mol
In the reaction N2O4 = 2NO2, it is given that the AH298 and AS298 are +55.3kJ and +176J/K, respectively. Calculate AG at room temperature and discuss the spontaneity of this reaction at different temperature ranges.

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