Ask Question
1 June, 21:21

The most important commercial process for generating hydrogen gas is the water-gas shift reaction:. CH4 (g) + H2O (g) → CO (g) + 3H2 (g). Use tabulated thermodynamic data to find ΔG° for this reaction at the standard temperature of 25°C. i found this to be. = 1.423*102 kJ. Now calculate ΔG°1200 for this process when it occurs at 1200 K

+5
Answers (2)
  1. 1 June, 21:30
    0
    The Gibb's free energy at a certain temperature is calculated by using the equation,

    ΔG = - RT (ln K)

    where K is the constant. We calculate this value by using the first conditions,

    1.423x10^2 = - (8.314) (25 + 273) x (ln K)

    Solving for K,

    K = 0.94418

    Use the equation for the second set of conditions,

    ΔG = - (8.314) (1200) x (ln 0.94418)

    ΔG° at 1200 K is approximately 573.05 kJ
  2. 1 June, 21:37
    0
    The Gibb's free energy at a certain temperature is calculated through the equation,

    ΔG = - RT (ln K)

    where K is constant. Substituting the values from the first set of the given,

    1.423x10^2 = - (8.314) (25 + 273) x (ln K)

    Solving for the value of K gives us an answer of, K = 0.94418

    Use the same equation to get the value of ΔG°1200

    ΔG = - (8.314) (1200) x (ln 0.94418)

    The value of ΔG°1200 is approximately 573.05 kJ
Know the Answer?
Not Sure About the Answer?
Find an answer to your question 👍 “The most important commercial process for generating hydrogen gas is the water-gas shift reaction:. CH4 (g) + H2O (g) → CO (g) + 3H2 (g). ...” in 📗 Chemistry if the answers seem to be not correct or there’s no answer. Try a smart search to find answers to similar questions.
Search for Other Answers