For a first order reaction the rate constant is #1 xx 10^(-5) "s"^(-1)# having #E_a = "1800 kJ/mol"#. Then value of #ln A# at #T = "600 K"# is?

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Answer 1 · 2017-12-26T06:26:27

THe answer is #=3588.5s^-1#

Apply the Arrhenius Equation

#k=Ae^(-E_a/(RT))#

Here, we have

The rate constant is #k=1.0*10^-5s^-1#

The activation energy is #E_a=1800kJ "mole"^-1#

#lnk=lnA-E_a/(RT)#

The temperature is #T=600K#

The gas constant #R=8.314J"(moleK)"^-1#

Therefore,

#lnA=lnk+E_a/(RT)#

#=ln(1*10^-5)+(1.810^6)/(8.314*600)#

#=-11.51+3.610^2#

#=3588.5s^-1#