Calculate ΔS^0reaction in J/mol at 298.15 K given Fe2O3(s)+3H2(g)→2Fe(s)+3H2O(l) ΔS^0reaction=ΣnS^0Products−ΣnS^0Reactants Substance ΔG^0/f (kJ/mol) ΔH^0/f (kJ/mol) S^0 298K (J/mol K) Fe2O3(s) -742.2 -824.2 87.40 H2(g) 0 0 130.7 Fe(s) 0 0 27.3 H2O(l) -237.1 -285.83 70.0 ANSWER CHOICES: a) 16.7 b) -214.9 c) none of these d) 24.8
Calculate ΔS^0reaction in J/mol at 298.15 K given Fe2O3(s)+3H2(g)→2Fe(s)+3H2O(l) ΔS^0reaction=ΣnS^0Products−ΣnS^0Reactants Substance ΔG^0/f (kJ/mol) ΔH^0/f (kJ/mol) S^0 298K (J/mol K) Fe2O3(s) -742.2 -824.2 87.40 H2(g) 0 0 130.7 Fe(s) 0 0 27.3 H2O(l) -237.1 -285.83 70.0 ANSWER CHOICES: a) 16.7 b) -214.9 c) none of these d) 24.8
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter17: Chemcial Thermodynamics
Section: Chapter Questions
Problem 17.38QE
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Question
Calculate ΔS^0reaction in J/mol at 298.15 K given
Fe2O3(s)+3H2(g)→2Fe(s)+3H2O(l)
ΔS^0reaction=ΣnS^0Products−ΣnS^0Reactants
| Substance | ΔG^0/f (kJ/mol) | ΔH^0/f (kJ/mol) | S^0 298K (J/mol K) |
| Fe2O3(s) | -742.2 | -824.2 | 87.40 |
| H2(g) | 0 | 0 | 130.7 |
| Fe(s) | 0 | 0 | 27.3 |
| H2O(l) | -237.1 | -285.83 | 70.0 |
ANSWER CHOICES:
a) 16.7
b) -214.9
c) none of these
d) 24.8
e) -134.38
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