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

Explanation

According to Arrhenius equation
`log ""(k_(2))/(k_(1))=(E_(a))/(2.303R)xx(T_(2)-T_(1))/(T_(1)T_(2))`
`k_(1)=4.5xx10^(3)s^(-1)`
`k_(2) =1.5 xx10^(4)s^(-1)`
`T_(1)=10^(@)C=283K`
`log ""(1.5 xx10^(4))/(4.5xx10^(3))=((6000Jmol ^(-1)))/(2.303 xx(8.314J mol ^(-1)))=((T_(2)-283)/(283T_(2)))`
`log 3.333 =3133.62 (T_(2)-283)/(283T_(2))`
`1-(283)/(T_(2))=0.04776`
`or T_(2)=(283)/(1-0.04776)=(283)/(0.9524)`
` T_(2) =297.19 K =(297.19-273.0)=24.19^(@)C`
Temperature `=24.19^(@)C`