the rate of a reaction doubles when it's temperature change from 300 k to 310 k. activation energy of such a reaction will be
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Using Arrhenius Equation
ln(k2/k1) = (Ea/R)(1/T1-1/T2)
We get,
2.303 log2 = -(Ea/8.314)(1/300-1/310)
Ea = 5359.59 Jmol-1= 53.6 kJ mol-1
ln(k2/k1) = (Ea/R)(1/T1-1/T2)
We get,
2.303 log2 = -(Ea/8.314)(1/300-1/310)
Ea = 5359.59 Jmol-1= 53.6 kJ mol-1
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