Calculating Kp for these two reactions

Question

Calculate the equilibrium constant, Kp, for these two reaction at 298.15 K

a. 2 HCl (g) <===> H2 (g) Cl2 (g)

b. N2 (g) O2 (g) <====> 2 NO (g)

Answer 1

a. 2 HCl (g) &lt;===&gt; H2 (g) Cl2 (g)

dG = dGf&#039;s products - reactants

dG = (0 &amp; 0) - [(2)(-92.3kJ)

dG = +184.6 kJ

dG = -RTlnK

+184,600 Joules = - (8.314Joules per)(298.15)LnK

lnK = - 74.47

e^x both sides

first answer:  K = 4.55e-33

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b. N2 (g) O2 (g) &lt;====&gt; 2 NO (g

dG = dGf&#039;s products - reactants

dG = [(2) (90.37)] - [(0 &amp; 0)]

dG = +180.74 kJ

dG = -RTlnK

+180,740 Joules = - (8.314Joules per)(298.15)LnK

lnK = - 72.91

e^x both sides

second answer:  K = 2.16e-33