Answer: K = 284
Explanation:
Gibbs free energy (DG) = RT(InK)
Where :
R = Gas constant = 8.314J/K/mol = 0.008314KJmol/K
T = temperature in Kelvin = 298K
K = dissociation rate
DG = 14
DG = RT(InK)
14 = 0.008314 × 298 × (InK)
14 = 2.477572 × InK
Ink = (14 ÷ 2.477542)
InK = 5.6507619
K = 284
The thermodynamic standard reaction Gibbs energy has been 284 kJ/mol.
The standard Gibbs free energy has been the energy required for changing the state of 1 mole of substance from its standard state.
The Gibbs free energy ([tex]\rm \Delta G^\circ[/tex]) has been given by:
[tex]\rm \Delta G^\circ\;=\;RT\;In K[/tex]
Where,
[tex]\rm \Delta G^\circ\;=\;14\; kJ/mol[/tex]
R = constant = 0.008314 kJ.mol/K
T = temperature = 298 K
In K = natural log of K
Substituting the values for the calculation of K:
[tex]\rm 14\;kJ/mol=0.008314\;kJ.mol/K\;\times\;298\;K\;\times\;In\;K\\In\;K=\;\dfrac{14\;kJ/mol}{0.008314\;kJ.mol/K\;\times\;298\;K}\\In K=5.650[/tex]
Taking the anti log on both the side:
K = 284 kJ/mol
The thermodynamic standard reaction Gibbs energy has been 284 kJ/mol.
For more information about the Gibbs energy, refer to the link:
https://brainly.com/question/9552459
