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The equilibrium constant for a certain reaction increases by a factor of 2.84 when the temperature is increase?
The equilibrium constant for a certain reaction increases by a factor of 2.84 when the temperature is increased from 300.0 K to 350.0 K. Calculate the standard change in enthalpy for this reaction (assuming H is temperature independent).
1 Answer
- ?Lv 79 years agoFavorite Answer
hello again ...thanks for giving Best answer on the previous question ...
using Vant hoff equation ...
http://en.wikipedia.org/wiki/Van_'t_Hoff_equation
ln ( K2/K1) = -delta H/R [ 1/T2 - 1/T1 ]
where K1 = K
K2 = 2.84K
T1 = 300 K
T2 = 350 K
R = 8.314 J/K/mole
putting the values...
ln (2.84K/K) = -delta H/8.314 [ 1/350 - 1/300 ]
ln 2.84 = -delta H/8.314 [ 2.857 X 10^-3 - 3.333 X 10^-3 ]
1.044 = ( -delta H/8.314 ) X (-0.476) X 10^-3
1.044 = delta H X 5.725 X 10^-5
delta H = 1.044 / 5.725 X 10^-5 = 18235.808 J/mole = 18.235 kJ/mole
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