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19.) Consider the following reaction, determine the temperature at which it is spontaneous? SO3 (g) + H20 (1) H2SO4 (aq) So 0/ K mol) 256.76 Specie SO3 (g) H20 (U) H2SO4 (aq) AH° (kJ/mol) -395.72 -285.83 69.91 -909.27 20.1 A. 470 °C В. 742 0C С. 1346 0С D. 1073°C E. -271°C

19.) Consider the following reaction, determine the temperature at which it is spontaneous? SO3 (g) + H20 (1) H2SO4 (aq) So 0/ K mol) 256.76 Specie SO3 (g) H20 (U) H2SO4 (aq) AH° (kJ/mol) -395.72 -285.83 69.91 -909.27 20.1 A. 470 °C В. 742 0C С. 1346 0С D. 1073°C E. -271°C

Chemistry
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
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Please answer 19-20.
19.) Consider the following reaction, determine the temperature at which it is spontaneous? SO3 (g) + H20 (1) H2SO4 (aq) So (1/ K mol) 256.76 Specie SO3 (g) H20 (1) H2SO4 (aq) AHº (kJ/mol) -395.72 -285.83 69.91 -909.27 20.1 A. 470 °C B. 742 °C C. 1346 °C D. 1073°C E. -271°C 20.) Ferric oxide is one of the product of rusting. The reaction for the formation of rust is given by: 4Fe + 30z 2FE203 Calculate the Gibbs energy of the reaction, if the Gibbs energy of formation of Fez03 (s) is -742.2 kJ/mol. A. -742.2 kJ/mol B. +742.2 kJ/mol C. -1484 kJ/mol D. +1484 kJ/mol E. -371 kJ/mol
Transcribed Image Text:19.) Consider the following reaction, determine the temperature at which it is spontaneous? SO3 (g) + H20 (1) H2SO4 (aq) So (1/ K mol) 256.76 Specie SO3 (g) H20 (1) H2SO4 (aq) AHº (kJ/mol) -395.72 -285.83 69.91 -909.27 20.1 A. 470 °C B. 742 °C C. 1346 °C D. 1073°C E. -271°C 20.) Ferric oxide is one of the product of rusting. The reaction for the formation of rust is given by: 4Fe + 30z 2FE203 Calculate the Gibbs energy of the reaction, if the Gibbs energy of formation of Fez03 (s) is -742.2 kJ/mol. A. -742.2 kJ/mol B. +742.2 kJ/mol C. -1484 kJ/mol D. +1484 kJ/mol E. -371 kJ/mol
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