Why is DeltaGo Temperature Dependent in Standard State?

In summary, the concept of standard state in thermodynamics does not consider the temperature of the system, which may cause confusion when comparing it to STP (standard temperature and pressure). This means that the value of deltaGo may vary at different temperatures, as it depends on both the standard enthalpy and standard entropy of the reaction.
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I see why, numerically speaking, deltaGo, defined as deltaGo = - RT ln K or deltaGo = deltaHo - TdeltaSo would be temperature dependent. But why is deltaGo temperature dependent, when it is simply Gibbs Free Energy at Standard State?

Is this essentially saying that the definition of standard state differs per temperature given? As in deltaGo=A for the "standard" state of 298K and 1 bar, but deltaGo=B for the "standard" state of 312K and 1 bar?

Thank you.
 
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Standard state does not take into account the temperature of a system. This is confusing because you read and hear about STP (standard temperature and pressure) which is not the same as saying standard state from the perspective of thermodynamics.

Ref: http://goldbook.iupac.org/S05925.html
 
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FAQ: Why is DeltaGo Temperature Dependent in Standard State?

What is the "Temperature Dependence of Go"?

The "Temperature Dependence of Go" is a scientific concept that describes the change in the Gibbs free energy (Go) of a system with respect to temperature. It is used to understand the relationship between temperature and the spontaneity of a chemical reaction or physical process.

How is the "Temperature Dependence of Go" calculated?

The "Temperature Dependence of Go" is calculated using the equation: ΔGo = ΔHo - TΔSo, where ΔHo is the change in the enthalpy of the system and ΔSo is the change in the entropy of the system. This equation is based on the Gibbs-Helmholtz equation, which relates the temperature dependence of Go to the temperature dependence of the equilibrium constant.

What is the significance of the "Temperature Dependence of Go" in chemistry?

The "Temperature Dependence of Go" is significant in chemistry because it helps us understand the spontaneity of a chemical reaction or process at different temperatures. Based on the calculated value of ΔGo, we can predict whether a reaction or process will be spontaneous or non-spontaneous at a particular temperature.

How does the "Temperature Dependence of Go" affect equilibrium?

The "Temperature Dependence of Go" affects equilibrium by determining the direction in which a reaction will proceed at a given temperature. If the value of ΔGo is negative, the reaction will be spontaneous and proceed in the forward direction. If the value of ΔGo is positive, the reaction will be non-spontaneous and proceed in the reverse direction. At equilibrium, ΔGo is equal to zero.

What factors can influence the "Temperature Dependence of Go"?

The "Temperature Dependence of Go" can be influenced by several factors, including the nature of the reactants and products, the temperature range, and the pressure. Changes in any of these factors can alter the value of ΔGo and affect the spontaneity of a reaction or process.

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