Scienuk Posted April 7, 2017 Report Share Posted April 7, 2017 The answer is A, can someone explain how you got to the answer and the relation between temperature and equilibrium using the given equation? It doesn't seem to be mentioned in my book. Reply Link to post Share on other sites More sharing options...
kw0573 Posted April 7, 2017 Report Share Posted April 7, 2017 For a reaction going to near completion, the equilibrium constant is much greater than 1. That narrows answer to A or C. More spontaneous reactions have more negative Gibbs energy and that happens with higher T. Reply Link to post Share on other sites More sharing options...
Scienuk Posted April 7, 2017 Author Report Share Posted April 7, 2017 1 hour ago, kw0573 said: For a reaction going to near completion, the equilibrium constant is much greater than 1. That narrows answer to A or C. More spontaneous reactions have more negative Gibbs energy and that happens with higher T. By completion you mean favouring the forward reaction, I gather, correct me if I'm wrong. Also, where in the question is spontaneity mentioned? how exactly may it be related, I have an idea but am not sure, if you would elaborate on that please. Thanks! Reply Link to post Share on other sites More sharing options...
kw0573 Posted April 7, 2017 Report Share Posted April 7, 2017 Completion usually refers to the forward reaction. So spontaneity measures the readiness of how a reaction proceeds. Typically reactions that goes to completion have high spontaneity and that means a very negative Gibbs energy. Reply Link to post Share on other sites More sharing options...
Scienuk Posted April 7, 2017 Author Report Share Posted April 7, 2017 27 minutes ago, kw0573 said: Completion usually refers to the forward reaction. So spontaneity measures the readiness of how a reaction proceeds. Typically reactions that goes to completion have high spontaneity and that means a very negative Gibbs energy. My thoughts exactly, thanks! Reply Link to post Share on other sites More sharing options...
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