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In the Arrhenius for a certain reaction, the value of A and E_(a) (activation energy) are 4 xx 10^(13) sec^(-1) and 98.6 "kJ mol"^(-1), respectively. If the reaction is of first order, the temperature at which its half-life period is 10 minutes is |
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Answer» `280 K` We know that `k = (2.303)/(t) "LOG"((a)/(a-x))` `(t_(1//2)=10xx60 SEC)=1.1558xx10^(-3)` According to ARREHENIUS equation, `log k = log A - (Ea)/(2.303 RT)` Substituting the various values in the above equation `log 1.155 xx 10^(-3) = log 4 xx 10^(13) - (98.6)/(2.303 xx 8.314 xx 10^(-3) xx T)` On usual calculation, `T = 311.35 K` |
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