Please can someone explain to me what happens when Gibb's free energy value gives positive value in study of stability constants of complex at high temperature.
Gibbs energy is a measure of the spontaneous course of the process, then between the ΔG sign for any reaction and its spontaneous course (at constant temperature and pressure) there are such dependencies: If ΔG is negative (ΔG 0), then the reaction cannot occur spontaneously in the forward direction. However, the reverse reaction is spontaneous
Hi,
The Gibbs free energy is one of the most important thermodynamic functions for the characterization of a system. It is a factor in determining outcomes such as the voltage of an electrochemical cell, and the equilibrium constant for a reversible reaction.
The sign of ΔG will change from positive to negative (or vice versa) where T = ΔH/ΔS. In cases where ΔG is: negative, the process is spontaneous and may proceed in the forward direction as written. positive, the process is non-spontaneous as written, but it may proceed spontaneously in the reverse direction.
thanks Gomathy and Khomenko for your contribuction. actually ΔG move from -400.75 at 313K to +9.02 at 318K in the study of stability constants of Cr (III) ion with methyl amine. What could be the possible reason. Thanks
What you're describing can't happen. Since something did happen, you're not describing it correctly. You can't directly measure Gibbs free energy, so you must be calculating it. Your calculation is not correct, as that would be a violation of the 2LoT. You may be missing some terms or perhaps products or reactants participating in one or more reactions. The properties may also be incorrect. I have seen a lot of errors in properties listed on the web. For example, tables that say kJ/kg that should MJ/kg or kJ/g and also g when they mean gram-mole, not gram or a similar incorrect label for kg-moles. You may be on the right track but one number is off.
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