use the following thermodynamic data at 298K to determine the equilibrium consta

Question

use the following thermodynamic data at 298K to determine the equilibrium constant at this temperature for the reaction of iron in steam to form hydrogen and iron (III) oxide QUESTION 13 0.3333 points Save Answer Use the following thermodynamic data at 298 K to determine the equilibrium constant at this temperature for the reaction of iron in steam to form hydrogen and iron(III) oxide 2Fe(s) + 3H20(g) 3H2(g) + Fe2O3(s) Fe)Fe:06 H20(g)H2(8) 242 229 189 Substance Fe(s) Fe2Os(s) -824 -742 87 AH'r(kJ/mol) o -0 -0 131 S(J/K mol) 27 0 4.36 x 109 1.8 x 10-3 O 1.58 x 1022 O 4.36 x 10-9

Explanation / Answer

Delta G of reaction = delta G of products - Delta G of reactants

Delta G of reaction = [Delta G Fe2O3 + 3XDelta G of H2] - [ Delta G Fe + 3X Delta G H2O]

Delta G of reaction = -742 - ( -3X229) = -55 KJ /mole

Now the Delta G and rate constant are related as

Delta G = -RTlnK

R = gas costant = 8.314 J / K-1 mol-1

So we will convert Delta G also in joules by multiplyin with 1000.

-55X1000 = - 8.314 X 298 x ln K

so ln K = 22.19

Taking antilog on both side

K = 4.35X 10^9 Or approx 4.36 X 10^9 ( option 1)

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