Consider the reaction: Co(g) + 3H2(g)–CH4(g) + H20(g) Using standard thermodynamic data at 298K, calculate the free energy change when 1.53 moles of CO(g) react at standard conditions. AG°rxn = kJ

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Chapter1: Chemical Foundations
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a)

b)

Consider the reaction:
Co(g) + 3H2(g)
CH4(g) + H20(g)
Using standard thermodynamic data at 298K, calculate the free energy change when 1.53 moles of CO(g) react at standard conditions.
AG°,
kJ
rxn
Transcribed Image Text:Consider the reaction: Co(g) + 3H2(g) CH4(g) + H20(g) Using standard thermodynamic data at 298K, calculate the free energy change when 1.53 moles of CO(g) react at standard conditions. AG°, kJ rxn
A student determines the value of the equilibrium constant to be 6.29x104 for the following reaction.
S(s,rhombic) + 2CO(g)-
SO2(g) + 2C(s,graphite)
Based on this value of Keg:
AG° for this reaction is expected to be (greater, less)
than zero.
Calculate the free energy change for the reaction of 1.53 moles of S(s,rhombic) at standard conditions at 298K.
AG°xn =
kJ
Transcribed Image Text:A student determines the value of the equilibrium constant to be 6.29x104 for the following reaction. S(s,rhombic) + 2CO(g)- SO2(g) + 2C(s,graphite) Based on this value of Keg: AG° for this reaction is expected to be (greater, less) than zero. Calculate the free energy change for the reaction of 1.53 moles of S(s,rhombic) at standard conditions at 298K. AG°xn = kJ
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