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The first order rate constant for the de...

The first order rate constant for the decomposition of `C_(2)H_(5)I` by the reaction.
`C_(2)H_(5)I(g)rarrC_(2)H_(4)(g)+HI(g)`
at `600 K is 1.60xx10^(-5)s^(-1)`. Its energy of activation is `209 kJ mol^(-1)`. Calculate the rate constant at `700 K`

Text Solution

AI Generated Solution

To solve the problem, we will use the Arrhenius equation and the relationship between the rate constants at two different temperatures. The equation we will use is: \[ \log \left( \frac{K_2}{K_1} \right) = \frac{E_a}{2.303 \cdot R} \left( \frac{1}{T_1} - \frac{1}{T_2} \right) \] Where: - \( K_1 \) is the rate constant at temperature \( T_1 \) (600 K). ...
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