1.

The decomposition of A into product has value of k as as 4.5 xx10^3s^(-1)" at "10^@C and energy of activation 60"kJ mol"^(-1). At what temperature would k be 1.5xx10^4s^(-1) ?

Answer»

SOLUTION :`k_1=4.5xx10^3s^(-1)`
`T_1 = 10 + 273 K = 283 K`
`k_2=1.5x10^4s^(-1)`
`T_2=? , E_a=60" kJ MOL"^(-1)`

According to Arrhenius equation,
`LOG.k_2/k_1=E_a/(2.303R)[(T_2-T_1)/(T_1T_2)]`
or `log.(1.5xx10^4)/(4.5xx10^(3))=(60000"Jmol"^(-1))/(2.303xx8.314"JK"^(-1) mol^(-1))xx[(T_2-283)/(283T_2)]`
or , `log3.3333333=3133.63[(T_2-283)/(283T_2)]`
or `0.0472T_2=T_2-283`
or `0.9528T_2=283`
or `T_2=283/90.9528=297K=(297-273^@C)=24^@C`


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