Relationship between free energy and the equilibrium constant

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The relationship between free energy and the equilibrium constant is defined by the equation ΔG° = -RT ln K. Experimental data shows that the Kb for NH3(aq) varies with temperature, with specific values provided for 283 K, 293 K, and 303 K. For moderate temperature ranges, ΔS° and ΔH° can be considered approximately temperature independent. A user attempts to derive a linear equation relating ln Kb to ΔH and ΔS, but seeks clarification on the correct axes for their plot. The discussion emphasizes the need for proper categorization of questions and understanding of thermodynamic relationships.
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The relationship between free energy and the equilibrium constant is

Go = -RT ln K

By measuring the pH at various temperatures, the Kb for NH3(aq) was found to be temperature dependent, yielding the following values:

temperature (K) Kb
283 1.34 X 10-5
293 1.42 X 10-5
303 1.50 X 10-5

Over moderate temperature ranges (ranges less than 100 K degrees) both deltaSo and deltaHo can be considered approximately temperature independent. By plotting the available information appropriately, obtain estimates for deltaSo and delayHo for the reaction:


ok so i figured out that my y=mx+b equation should loook lik:

lnKb=delta H/R(gas constnt) - delta S/r

bbut what is my x-axis and y axis?
 
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1. This question belongs in the Coursework & Homework section of the forums. Henceforth, please post such questions there (and use a more descriptive title).

2.
ok so i figured out that my y=mx+b equation should loook lik:

lnKb=delta H/R(gas constnt) - delta S/r
That's not right. What is the relationship between \Delta G_0~,~~\Delta H_0 and \Delta S_0 ?
 
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