Answer to Question #177137 in Physical Chemistry for Miriama Tamaivena

Question #177137

The activation energy of a reaction is 22.5 k Cal mol-1 and the value of rate constant at 40°C is 1.8 ×10−5 s−1. Calculate the frequency factor, A.


1
Expert's answer
2021-04-01T02:34:59-0400

Ea=22.5kcalmol1=22500calmol1Ea = 22.5 kcal mol^{-1}= 22500 cal mol^{-1}


T=40°C=40+273=313KT= 40°C = 40 + 273 = 313 K


k=1.8×105sec1k = 1.8 ×10^{-5}sec ^{-1}


Substituting the values in the equation


logA=logk+(Ea2.303RT)log A = log k + (\frac{E_a}{2.303RT})


logA=log(l.8×105)+(Ea2.303×1.987×313)log A = log (l.8×10^{-5}) + (\frac{E_a}{2.303×1.987×313})


logA=log(l.8)5+(15.7089)log A = log (l.8) – 5 + (15.7089)


logA=(10.9642)log A = (10.9642)


A=antilog(10.9642)A = antilog ( 10.9642)


A=9.208×1010A = 9.208 × 10^{10} collisions s1s^{-1}


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