Calculate ΔG0reaction in kJ/mol at 298.15 K given Fe2O3(s)+3H2(g)→2Fe(s)+3H2O(l) ΔG^0reaction=ΣnΔG0Products−ΣnΔG0Reactants Substance ΔG0f (kJ/mol) ΔH0f(kJ/mol) S0298K (J/mol K) Fe2O3(s)Fe2O3(s) -742.2 -824.2 87.40 H2(g)H2(g) 0 0 130.7 Fe(s)Fe(s) 0 0 27.3 H2O(l)H2O(l) -237.1 -285.83 70.0 answer choices: a) 30.9 b)175.2 c)none of these d)158.7 e)-622.58
Calculate ΔG0reaction in kJ/mol at 298.15 K given Fe2O3(s)+3H2(g)→2Fe(s)+3H2O(l) ΔG^0reaction=ΣnΔG0Products−ΣnΔG0Reactants Substance ΔG0f (kJ/mol) ΔH0f(kJ/mol) S0298K (J/mol K) Fe2O3(s)Fe2O3(s) -742.2 -824.2 87.40 H2(g)H2(g) 0 0 130.7 Fe(s)Fe(s) 0 0 27.3 H2O(l)H2O(l) -237.1 -285.83 70.0 answer choices: a) 30.9 b)175.2 c)none of these d)158.7 e)-622.58
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 17.47QE
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Question
Calculate ΔG0reaction in kJ/mol at 298.15 K given
Fe2O3(s)+3H2(g)→2Fe(s)+3H2O(l)
ΔG^0reaction=ΣnΔG0Products−ΣnΔG0Reactants
| Substance | ΔG0f (kJ/mol) | ΔH0f(kJ/mol) | S0298K (J/mol K) |
| Fe2O3(s)Fe2O3(s) | -742.2 | -824.2 | 87.40 |
| H2(g)H2(g) | 0 | 0 | 130.7 |
| Fe(s)Fe(s) | 0 | 0 | 27.3 |
| H2O(l)H2O(l) | -237.1 | -285.83 | 70.0 |
answer choices:
a) 30.9
b)175.2
c)none of these
d)158.7
e)-622.58
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