Answer:
The first reaction is spontaneous
The second reaction is also spontaneous
Explanation:
The question is incomplete or the data part are missing, nonetheless, here is the complete question with the data table ; For each part below , use the data below to calculate ΔG at 215 K for each of the following reactions . Then use the data in the chart to determine whether each reaction is spontaneous at 215 K.
The Gibb's free energy also referred to as the Gibb's function represented with letter G. it is the amount of useful work obtained from a system at constant temperature and pressure. The standard Gibb's free energy on the other hand is a state function represented as ΔG, as it depends on the initial and final states of the system. The spontaneity of a reaction is explained by the standard Gibb's free energy.
If ΔG = -ve ( the reaction is spontaneous)
if ΔG = +ve ( the reaction is non-spontaneous)
if ΔG= 0 ( the reaction is at equilibrium)
Use this hints for any reaction involving the Gibb's free, Enthalpy and entropy.
The step by step calculation with the data table is attached.
More than 2 compounds reactant and transformed into one or more unique substances, known as products. A reaction's calculation can be defined as follows:
[tex]2SO_2 + O_2 \longrightarrow 2SO_3[/tex]
For
DH0rxn = (2×-395.7)-(2×-296.8 +0)
= -197.8 kj
DS0rxn = (2×256.8)-(2×248.2+205.0)
= -187.8 j/mol.k
[tex]\to[/tex] DG = DH0-TDS0
= (-197.8)-(215×-187.8 ×10⁻³)
= -157.42 kj
Similar to DG which is negative, the process is spontaneous.
[tex]SO_3\ (g) + H_2O\ (l) \longrightarrow H_2SO_4\ (l)\\\\[/tex]
DH0rxn = (-814.0)-(-395.7+(-285.8))
= -132.5 kj
DS0rxn = (156.9)-(256.8+70.0)
= -169.9 j/mol.k
DG = DH0-TDS0
= (-132.5)-(215×-169.9 ×10⁻³)
= -96 kj
Like the DG is negative, the process is spontaneous.
Note:
Please find the complete question in the attached file.
Find out more about the reaction here:
brainly.com/question/17434463
