1.

The activation energies for the two reactions are Ea and Ea^(') with E_(a)gtE_(a)^('). If the temperature of the reaction system is increased from T_(1) to T_(2). Predict which alternative is correct. (k^(')) are the rate constants at highest temperature.

Answer»

`(k_(1)^('))/(k+(1)) = (k_(2)^('))/(k_(2))`
`k_(1) lt k_(2)` and `k_(2)^(') lt k_(1)^(')`
`k_(1) lt k_(2)`
`(k_(1)^(')/k_(1)) lt (2k_(2)^('))/(k_(2))`

SOLUTION :b) We know that
`k=Ae^((-Ea)/(RT))`
This means that more is the activation energy, lesser is the RATE constant.
Since `E_(a) gt E_(a)^(')`
`THEREFORE k_(1) lt k_(2)` and `k_(1)^(')` and `k_(2)^(')`


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