A reaction has a K = 1.0 times 10^-3 at 35 degree C and 2.5 times 10^-2 at 25 de

Question

A reaction has a K = 1.0 times 10^-3 at 35 degree C and 2.5 times 10^-2 at 25 degree C. The reaction is Gaseous Cannot tel Exothermic Endothermic A particular reaction had K = 0.0100 at 5 degree C. Calculate Delta G degree in kJ A reaction has a DG degree at 22.3 kJ(or kH/mol)at 26 degree C. Calculate K For a particular K = 0.00133 t 25 degree C and K = 25 degree K = 0.0133 at 125 degree C. Calculate Delta H degree as kJ(or kJ/mol) If a reaction has K = 0.100 at 500 degree K and a Delta H degree = 25.2 kJ(or kJ/mol), what would K be at 600. K degree K.

Explanation / Answer

1. with K increasing with decreasing temperature, the reaction is,

exothermic

2. Using,

dGo = -RTlnK

K = 0.01

so,

dGo = -8.314 x 298 ln(0.01)

       = 11.41 kJ/mol

3. with,

dGo = 22.3 kJ/mol

22300 = -8.314 x 298 lnK

K = 1.23 x 10^-4

4. using,

ln(k2/k1) = dHo/R[1/T1 - 1/T2]

T1 = 25 + 273 = 298 K

T2 = 125 + 273 = 398 K

we get,

ln(0.0133/0.00133) = dHo/8/.314[1/298 - 1/398]

dHo = 22.708 kJ/mol

5. using the same formula as in 4.

ln(k2/0.1) = -25200/8.314[1/500 - 1/600]

k2 = 0.0365

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