6) The reaction below shows how coal (carbon) can be converted to methane (natural gas): C(s) + 2 H2(g) --------> CH4(g) Using the data provided, compute ∆G° at 25°C and then find the equilibrium constant K for the reaction; Is the reaction spontaneous or non-spontaneous? Compound ∆Hf ∆Sf CH4 –74.848 kJ/mole 186.2 J/mole K H2 0 130.6 J/K mol K C(s) 0 5.69 J/K mole K Find the temperature at which the reaction changes Find ∆G and Keq at 1000 K.
6) The reaction below shows how coal (carbon) can be converted to methane (natural gas): C(s) + 2 H2(g) --------> CH4(g) Using the data provided, compute ∆G° at 25°C and then find the equilibrium constant K for the reaction; Is the reaction spontaneous or non-spontaneous? Compound ∆Hf ∆Sf CH4 –74.848 kJ/mole 186.2 J/mole K H2 0 130.6 J/K mol K C(s) 0 5.69 J/K mole K Find the temperature at which the reaction changes Find ∆G and Keq at 1000 K.
Chemistry & Chemical Reactivity
9th Edition
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter18: Principles Of Chemical Reactivity: Entropy And Free Energy
Section: Chapter Questions
Problem 32PS
Related questions
Question
6) The reaction below shows how coal (carbon) can be converted to methane (natural gas): C(s) + 2 H2(g) --------> CH4(g)
Using the data provided, compute ∆G° at 25°C and then find the equilibrium constant K for the reaction; Is the reaction spontaneous or non-spontaneous?
Compound |
∆Hf |
∆Sf |
CH4 |
–74.848 kJ/mole |
186.2 J/mole K |
H2 |
0 |
130.6 J/K mol K |
C(s) |
0 |
5.69 J/K mole K |
- Find the temperature at which the reaction changes
-
Find ∆G and Keq at 1000 K.
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