Can you show me a picture of your work, puedes enseñar me una photo de tu trabajo... luego luego ti ayudo :)
The Gibbs free energy ΔG for the vaporisation of 2-methylbutane, in KJ/mol is 8.24 KJ/mol
<h3>Data obtained from the question </h3>
- Enthalpy change (ΔH) = 25. 22 KJ/mol
- Change in entropy (ΔS) = 84.48 J/Kmol = 84.48 / 1000 = 8.448×10¯² KJ/Kmol
- Temperature (T) = 201 K
- Gibbs free energy (ΔG) =?
<h3>How to determine the Gibbs free energy </h3>
The Gibbs free energy for the reaction can be obtained as follow:
ΔG = ΔH – TΔS
ΔG = 25.22 – (201 × 8.448×10¯²)
ΔG = 25.22 – 169.8048
ΔG = 8.24 KJ/mol
Thus, the ΔG for the reaction is 8.24 KJ/mol
Learn more about Gibbs free energy:
brainly.com/question/9552459
It produces a hydrazone in which the carbon is attached with the nitrogen atom with the means of a double bond.
I think the answer to this question is A: to use prior knowledge to understand historical passages because when you are given multiple choice questions as an example use the process of elimination such as which answers you think are wrong and which you think are right.
