Question

given, ( quad k_{1}=503 times 10^{-2} mathrm{mol}^{-1} mathrm{lit}^{2} / mathrm{sc} )
( t_{2}=6.71 mathrm{v} mathrm{mel}^{-1} 1.7^{2} / mathrm{ccc} )
[
begin{array}{l}
T_{1}=209 k
T_{2}=333 mathrm{k}
end{array}
]
( rightarrow ) To jind Activation enurgy ( ( F a ) )
We inow, Arvinionius ( e q^{4} ) "
9
( log left(frac{k}{r}right)=frac{F a}{2 cdot 103 R}left[frac{1}{T_{1}}-frac{1}{T}right] )
( therefore log left(frac{6 cdot 7}{5 times 10^{-1}}right)=frac{epsilon_{0}}{2 cdot 303 times 00621}left[frac{1}{280}-frac{1}{333}right] )
( 2-13=frac{E_{a}}{0.19} times[0.000+5] )
( therefore E_{a} geqslant frac{4 cdot 0.47}{4 cdot 57 times 10^{-4}}+0.885 times 10^{4} mathrm{J} )
( log _{2} 7 frac{6 cdot operatorname{ls} x 10^{3}}{2 cdot 30^{3} times 0 cdot 0001} times frac{1}{305} )
( log k .9 quad 0.153 times 10^{3} Rightarrow 153 )
( therefore quad k=2 cdot 18 mathrm{mo} )
( 2 / x )

# For the reaction C2H51 + OH → C2H5OH + . The rate constant was found to be 5.03 x 102 mol lit sec at 289 K and 6.71 mollit sec at 333K. What is the activation energy of the reaction? What is rate constant at 305 K?

Solution