10. Using the values below, calculate AG°rxn for the reaction below at 25 °C. Hg²*(aq) + 2C1 (aq) → HgCl2(s) AH°r (kJ/mol) | S° (J/K•mol) Hg²*(aq) CI (aq) HgCl2(s) +171.1 -32.2 56.5 -167.2 146 -224.0

10. Using the values below, calculate AG°rxn for the reaction below at 25 °C. Hg²(aq) + 2C1 (aq) → HgCl2(s) AH°r (kJ/mol) | S° (J/K•mol) Hg²(aq) CI (aq) HgCl2(s) +171.1 -32.2 56.5 -167.2 146 -224.0

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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6C(s) + 6H₂(g) + 30₂(g) → CH₁₂O6 (s) 2Al(s) + Fe₂O₂ (s) → ALO₂ (s) + 2Fe(s) AH = - 1237. kJ AS = -3280. AG = kJ Which is spontaneous? this reaction O the reverse reaction neither AH = -852. kJ AS = J K J K AG 19. kJ Which is spontaneous? this reaction the reverse reaction neither
#8 Round each of your answers to the nearest kJ - as it states in the directions.
A chemical engineer is studying the two reactions shown in the table below. In each case, he fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 105.0 °C and constant total pressure. Then, he measures the reaction enthalpy AH and reaction entropy AS of the first reaction, and the reaction enthalpy AH and reaction free energy AG of the second reaction. The results of his measurements are shown in the table. Complete the table. That is, calculate AG for the first reaction and AS for the second. (Round your answer to zero decimal places.) Then, decide whether, under the conditions the engineer has set up, the reaction is spontaneous, the reverse reaction is spontaneous, or neither forward nor reverse reaction is spontaneous because the system is at equilibrium.
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9 =+ For the reaction below AG° = + 33.0 kJ, AH° = + 92.2 kJ, and AS° =+ 198.7 J/K. Estimate the temperature at which this reaction occurs. 2 NH3(g) →N2(g) + 3H2(g) A) 0.464 K B) 166 K C) 298 K D) 464 K A B C
Consider the dissolution of nitrous acid: HNO₂(aq) For this reaction under standard conditions, AG° = 19.1 kJ/mol. Calculate A Gat 298 K, when [H*] = 5.0×10-² M, [NO₂¯] = 2.0×10−³ M and [HNO₂] = 0.10 M. (A) 2.0 kJ/mol (B) 12.5 kJ/mol (C) 16.6 kJ/mol (D) 19.1 kJ/mol (E) 36.2 kJ/mol - H+ (aq) + NO₂ (aq).
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The standard reaction free energy AG° = 29. kJ for this reaction: Fe2O3(g) + 2H2 (g) --> 2 Fe(s) + 3H2O(l) Use this information to complete the table below. Round each of your answers to the nearest kJ.
One of the reactions that destroys ozone in the upper atmosphere is NO(g) + O3(g) ⇒ NO2 (g) + O2(g) Substance and State AGf (kJ/mol) NO(g) 87 NO₂(g) 52 0₂ (9) 0 03 (9) 163 a Calculate ΔG° (at 298 K) for this reaction. AG = -198 kJ b Calculate K (at 298 K) for this reaction. K =
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