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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
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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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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