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The δgo of a reaction:
a. will change if the temperature of the reaction is changed.
b. will change if the concentration of reactants and products are changed.
c. can be used to calculate whether a reaction is thermodynamically favorable under defined non-standard conditions.
d. can predict whether a reaction will be thermodynamically favorable under standard conditions.
e. is not related to the equilibrium constant.

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E. Is The Right Answer

The δgo of a reaction is not related to the equilibrium constant.

What is δgo of a reaction?

  • The sign of the standard free energy change [tex]\Delta G^{\circ}[/tex] of a chemical reaction determines whether the reaction will tend to proceed in the forward or reverse direction.
  • A more advanced treatment of thermodynamics yields the following equation: [tex]\Delta G^{\circ}[/tex]=-RT ln(Keq) The variable R is the ideal gas constant (8.314 J/K•mol), T is the Kelvin temperature, and ln(Keq) is the natural logarithm of the equilibrium constant.
  • δgo and K. This equation allows us to calculate the equilibrium constant for any reaction from the standard-state free energy of reaction, or vice versa.
  • Gibbs free energy was originally defined graphically. In 1873, American scientist Willard Gibbs published his first thermodynamics paper, "Graphical Methods in the Thermodynamics of Fluids", in which Gibbs used the two coordinates of entropy and volume to represent the state of the body.

To learn more about δgo(Gibbs free energy ) refer to: https://brainly.com/subject/chemistry

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