Using standard heats of formation, calculate the standard enthalpy change for the following reaction. 2H₂S(g) + 302(g) → 2H₂O(g) + 2SO2(g) AH (H₂S(g)) = - AH (O₂(g)) = 0.0 kJ/mol AH (H₂O(g)) = AH° rxn = AH (SO₂ (9)) = ANSWER: Species AH (kl/mol) H₂(g) SO₂(9) H₂S(g) Using standard heats of formation, calculate the standard enthalpy change for the following reaction. C(s,graphite) + O₂(g) CO₂(g) 0.0 -296.8 -20.6 = -20.6 kJ/mol kJ kJ = -241.8 kJ/mol A scientist measures the standard enthalpy change for the following reaction to be 316.2 kJ: H₂S(g) + 2H₂O(1)→ 3H₂(g) + SO₂(g) Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of H₂O(l) is -824.2 0.0 0.0 Substance AH (kJ/mol) Fe₂O3 (8) H₂(g) Fe(s) = -296.8 kJ/mol A scientist measures the standard enthalpy change for the following reaction to be 76.3 kJ: Fe₂O3 (8) + 3H₂(g) → 2Fe(s) + 3H₂O(g) Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of H₂O(g) is kJ/mol. kJ/mol.

Using standard heats of formation, calculate the standard enthalpy change for the following reaction. 2H₂S(g) + 302(g) → 2H₂O(g) + 2SO2(g) AH (H₂S(g)) = - AH (O₂(g)) = 0.0 kJ/mol AH (H₂O(g)) = AH° rxn = AH (SO₂ (9)) = ANSWER: Species AH (kl/mol) H₂(g) SO₂(9) H₂S(g) Using standard heats of formation, calculate the standard enthalpy change for the following reaction. C(s,graphite) + O₂(g) CO₂(g) 0.0 -296.8 -20.6 = -20.6 kJ/mol kJ kJ = -241.8 kJ/mol A scientist measures the standard enthalpy change for the following reaction to be 316.2 kJ: H₂S(g) + 2H₂O(1)→ 3H₂(g) + SO₂(g) Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of H₂O(l) is -824.2 0.0 0.0 Substance AH (kJ/mol) Fe₂O3 (8) H₂(g) Fe(s) = -296.8 kJ/mol A scientist measures the standard enthalpy change for the following reaction to be 76.3 kJ: Fe₂O3 (8) + 3H₂(g) → 2Fe(s) + 3H₂O(g) Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of H₂O(g) is kJ/mol. kJ/mol.

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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1) Use Hess's Law to determine AH for the following target reaction. 3 CO₂(g) + 4 H₂O(g) b) C3Hg(g) + 5 O₂(g) C(s) + O₂(g) -CO₂(g) 2 H₂(g) + O₂(g) 3 C(s) + 4 H₂(g) →→→ 2 H₂O(g) C3H8(g) AH = AH = ΔΗ ΔΗ = ??? -2043 kJ -393.5 kJ -483.6 kJ
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How would you solve c? Transcribed Image Text:Temperature (°C) AN A student conducts an experiment to determine the value of for the dissolution of Na₂C₂H₂O₂ (s). The student dissolves 10.0 g of Na₂C₂H₂O₂ (s) in room-temperature water in a beaker and measures the temperature over time. The data are given in the graph above. 24- 22- 20 18 16 14 12- 10 Time (a) The student touches the side of the beaker after the dissolution has occurred and observes that it is cold. What experimental evidence is consistent with the student's observation? (b) Is the dissolution of endothermic or exothermic? Justify your answer in terms of the flow of energy between the system and surroundings. in kJ/mol. (c) The student calculated the energy change for the dissolution to be 4600 J. Based on this value, calculate AH soln
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