4. a. Consider the data below for the reaction H2Ou) = H2O() - Plot a graph and determine AH and AS for the reaction. Describe how they influence the spontaneity of the reaction as a function of temperature. T (°C) P (torr) 0.0 4.579 10.0 9.209 20.0 17.53 25.0 23.76 30.0 31.82 40.0 55.32 60.0 149.4 70.0 233.7 000

4. a. Consider the data below for the reaction H2Ou) = H2O() - Plot a graph and determine AH and AS for the reaction. Describe how they influence the spontaneity of the reaction as a function of temperature. T (°C) P (torr) 0.0 4.579 10.0 9.209 20.0 17.53 25.0 23.76 30.0 31.82 40.0 55.32 60.0 149.4 70.0 233.7 000

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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Using enthalpies of formation, calculate AH° for the following reaction at 25°C. Also calculate AS" for this reaction from standard entropies at 25°C. Use these values to calculate AG for the reaction at this temperature. Species AH; (kJ/mol) S" (J/mol·K) COCL, (9) -220.1 283.9 H20(1) -285.8 69.95 CO2 (9) -393.5 213.7 HCI(9) -92.31 186.8 COCI, (9) + H20(1) + CO, (9) + 2HCI(9) ΔΗ' kJ AS J/K AG° = kJ
Consider the following reaction with equilibrium constant 0.02532 at 25 oC. 2 A (g) + B (g) -------- 3 C(g) Determine free energy change for a mixture of 0.75 mol A, 1.20 mol C and 3.40 mol B in a 5.0-L vessel at 25 oC considering the above reaction in forward direction.
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
Compound NH4HCO3(s) NH3(g) CO2(g) H20(E) AG°; (kJ/mol) -665.9 -16.45 -394.4 -237.1 Consider the given reaction: NH3(g) + CO2(g) + H20(4) = NH4HCO3(s) Calculate AG at 298K for this reaction when the pressures of NH3 and CO2 are 0.52 atm and 0.31 atm, respectively. 22.5 kJ -26.7 kJ -13.4 kJ O 13.4 kJ O -22.5 kJ
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Compound NH4HCO3(s) NH3(g) CO2(g) H20(1) AG°; (kJ/mol) -665.9 -16.45 -394.4 -237.1 Consider the given reaction: NH3(g) + CO2(g) + H2O(1) = NH4HCO3(s) Calculate AG at 298K for this reaction when the pressures of NH3 and CO, are 0.52 atm and 0.31 atm, respectively. 22.5 kJ -13.4 kJ 13.4 kJ -26.7 kJ O -22.5 kJ
Acetic acid, HC2H3O2 (Ka = 1.8 x 10 5), dissociates in water as follows: HC2H3O2 = H* + C2H3O2. Use the K, value to calculate AG°298 (in kJ). O + 27.1 O + 11.8 O - 27.1 O - 11.8 O - 4.46 x 10-5
Determine the value of AG for the reaction at 309 K. Assume standard concentration 2NH;(g) = N,H,(g) + H, (g) Given AH (kJ/mol) S°J/{mol · K)) Substance NH3(3) -46.1 192.5 95.35 N2H4(g) H2(3) 238.5 0.0 130.6 O-87.0 kJ -182.5 kJ O -192.6 kJ O 87.0 kJ O 192.6 kJ
Use the data below to calculate the value of the equilibrium constant for the following reaction at 298 K. Please give your answer with 2 significant figures. 3 NO2(g) + H2O(e) → 2 HNO3(e) + NO(g) AfG [H2O(l)] = -237.2 kJ mol-1 ; AFG°[HNO3(e)] = -79.9 kJ mol-1 ; AfG [NO(g)] = 86.7 kJ mol-1; AfG°[NO2(g)] = 51.8kJ mol-1
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Given the following, determine K at 298K for the reaction, AgI(s) → Ag"(aq) +I (aq) Substance AG°£(kJ/mol) at 298 K I (aq) 51.59
Consider the following reaction: Use the data to find AHn for the reaction. 2 NO2 (g) = 2 NO(g) + O2(g) Express your answer in kilojoules per mole. The data in the table show the equilibrium constant for this reaction measured at several different temperatures. • View Available Hint(s) Temperature Kp 170 K 3.8 x 10-3 ? 180 K 0.34 190 K 18.4 AHon = kJ/mol 200 K 681 Submit Part B Use the data to find ASn for the reaction. Express your answer in joules per mole. ? ASin = J/K Submit Request Answer