delta G is delta G. The catalyst lowers the activation energy of the reaction so that it provides an alternative path for the reaction to take place and that allows it to proceed faster but the delta G value remains the same. (The reaction reaches equilibrium faster).
For the second part, what is the equation for delta G?
Delta G = delta H - T*delta S. Now how do you think T will affect delta G?
Some reactions that are predicted by their sign deltaG to be spontaneous at room temperature do not proceed at a measurable rate at room temperature.
A suitable catalyst increases the rate of such a reaction. What effect does the catalyst have on deltaG for the reaction?
AND
For a reaction, how is the value of the standard free energy change, deltaG, affected by an increase in temperature? Explain.
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Would the temperature increase increase the value of delta G then?
Since delta G = delta H - T*delta S, for constant delta S, increasing T will make the right term more negative and that will make delta G more negative. I don't know what you mean by "increasing" delta G, especially when dealing with negative numbers. The safe way to answer this type question is to say that delta G becomes more negative.
okay i see what you're saying. thanks so much for all your help.
7 answers