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The chemical equation for a reaction is shown below.

2 NO2(g) → N2O4(g)

What is the standard free energy change (ΔGo) in this reaction at 298 K? (NOTE: At 298 K, ΔGfo for NO2 is 51.84 kJ/mol, and for N2O4 is 98.28 kJ/mol.)

Sagot :

The standard free energy change (∆Gº') is the energy released when the products are created from the reactants. The (∆Gº') at 298 K is -5.40kJ.

What is standard free energy change?

The standard free energy change is given by the sum of the standard free energies of the products subtracted from the sum of the standard free energies of the reactants, given as,

ΔG = ∑nΔG°products − ∑mΔG°reactants

Given,

ΔG°(NO₂) = 51.84 kJ/mol

ΔG°(N₂O₄) = 98.28 kJ/mol

Substituting values:

ΔG = ∑nΔG°products − ∑mΔG°reactants

= ΔG°(N₂O₄) − 2ΔG°(NO₂)

= 98.28 − 2(51.84)

= - 5.4

Therefore, -5.40 kJ is the standard free energy.

Learn more about standard free energy here:

https://brainly.com/question/20351258

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