Question

Consider a process for which ΔH = 211 kJ and ΔS = -57 J/K. How will raising the temperature

affect ΔG for this process?

a) ΔG will increase

b) ΔG will decrease

c) ΔG will not change

d) The effect on ΔG cannot be predicted from the information given​

Answer 1

Answer :

The correct answer is b) ΔG will decrease. The change in Gibbs free energy, ΔG, is a measure of the overall change in energy and entropy during a process, and can be calculated as ΔG = ΔH - TΔS. In this case, ΔH is positive, meaning the process releases heat energy, while ΔS is negative, meaning the process becomes less random and more ordered. Raising the temperature will increase TΔS, causing ΔG to decrease, meaning the process becomes less energetically favorable at higher temperatures.

Explanation :

The Gibbs free energy, ΔG, is a thermodynamic quantity that describes the potential for a system to undergo spontaneous change. It depends on two other thermodynamic quantities: enthalpy (ΔH) and entropy (ΔS).

In the case of a process with ΔH = 211 kJ and ΔS = -57 J/K, it is not possible to predict the effect of raising the temperature on ΔG solely from this information. ΔG can be calculated using the equation ΔG = ΔH - TΔS, where T is the temperature in kelvin.

In general, ΔG can be used to determine whether a process will be spontaneous or not. If ΔG is negative, the process is spontaneous and will proceed as written. If ΔG is positive, the process is non-spontaneous and will not occur on its own. If ΔG is equal to zero, the system is at equilibrium and there is no net change.

So, in order to determine the effect of raising the temperature on ΔG, we need to calculate ΔG at the initial temperature and then calculate ΔG at the new temperature and compare the two values.

To know more about the concept please go through the links :

https://brainly.in/question/23849246

https://brainly.in/question/5363217

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