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  • The rate of a reaction triples when temperature changes from  n

The rate of a reaction triples when temperature changes from  \mathrm{20^{\circ}C}  to \mathrm{50^{\circ}C}. The energy of activation for the reaction is:

 

Option: 1

2.8 \mathrm{~kJ}


Option: 2

12.5 \mathrm{~kJ} \mathrm{~mol}^{-1}


Option: 3

28.8 \mathrm{~kJ} \mathrm{~mol}^{-1}


Option: 4

61.2 \mathrm{~kJ} \mathrm{~mol}^{-1}


Answers (1)

best_answer

Expression for rate constant at two different temperature is given by
\mathrm{\log _{10} \frac{k_2}{k_2}=\frac{E_a}{R \times 2.303}\left[\frac{T_2-T_1}{T_1 T_2}\right] }
Given:  \mathrm{\frac{k_2}{k_1}=3 ; R=8.314 \mathrm{~J} \mathrm{~K}^{-1} \mathrm{~mol}^{-1} ; T_1=20+273=293 \mathrm{~K}} and   \mathrm{T_2=50+273=323 \mathrm{~K}} Substituting the given values in the equation,
\mathrm{ \log _{10} 3=\frac{E_a}{8.314 \times 2.303}\left[\frac{323-293}{323 \times 293}\right] }
\mathrm{ E_a=\frac{2.303 \times 8.314 \times 323 \times 293 \times 0.477}{30} }
\mathrm{ =28811.8 \mathrm{~J} \mathrm{~mol}^{-1} }
\mathrm{ =28.8118 \mathrm{~kJ} \mathrm{~mol}^{-1} }.

 

Posted by

Ritika Jonwal

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