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For a first order reaction ArarrP , the ...

For a first order reaction `ArarrP` , the temperature (T) dependent rate constant `(K)` was found to follow the equation log `k=-(2000)(1)/(T)+6.0` . The pre- exponential factor A and the activation energy `E_(a)` , respectively, are :

A

`1.0xx10^(6)s^(-1)` and `9.2 kJ mol^(-1)`

B

`6.0 s^(-1)` and `16.6 kJ mol^(-1)`

C

`1.0xx10^(6)s^(-1)` and `16.6 kJ mol^(-1)`

D

`1.0xx10^(6) s^(-1)` and `38.3 kJ mol^(-1)`

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The correct Answer is:
D
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For a first order reaction A rarr P , the temperature (T) dependent rate constant (k) was found to follow the equation log k = -2000(1//T) + 6.0 . The pre-exponential factor A and the activation energy E_(a) , respective, are

The rate of reaction increases isgnificantly with increase in temperature. Generally, rate of reactions are doubled for every 10^(@)C rise in temperature. Temperature coefficient gives us an idea about the change in the rate of a reaction for every 10^(@)C change in temperature. "Temperature coefficient" (mu) = ("Rate constant of" (T + 10)^(@)C)/("Rate constant at" T^(@)C) Arrhenius gave an equation which describes aret constant k as a function of temperature k = Ae^(-E_(a)//RT) where k is the rate constant, A is the frequency factor or pre-exponential factor, E_(a) is the activation energy, T is the temperature in kelvin, R is the universal gas constant. Equation when expressed in logarithmic form becomes log k = log A - (E_(a))/(2.303 RT) Activation energies of two reaction are E_(a) and E_(a)' with E_(a) gt E'_(a) . If the temperature of the reacting systems is increased form T_(1) to T_(2) ( k' is rate constant at higher temperature).

The rate of reaction increases isgnificantly with increase in temperature. Generally, rate of reactions are doubled for every 10^(@)C rise in temperature. Temperature coefficient gives us an idea about the change in the rate of a reaction for every 10^(@)C change in temperature. "Temperature coefficient" (mu) = ("Rate constant of" (T + 10)^(@)C)/("Rate constant at" T^(@)C) Arrhenius gave an equation which describes aret constant k as a function of temperature k = Ae^(-E_(a)//RT) where k is the rate constant, A is the frequency factor or pre-exponential factor, E_(a) is the activation energy, T is the temperature in kelvin, R is the universal gas constant. Equation when expressed in logarithmic form becomes log k = log A - (E_(a))/(2.303 RT) For the given reactions, following data is given {:(PrarrQ,,,,k_(1) =10^(15)exp((-2000)/(T))),(CrarrD,,,,k_(2) = 10^(14)exp((-1000)/(T))):} Temperature at which k_(1) = k_(2) is

The rate of reaction increases isgnificantly with increase in temperature. Generally, rate of reactions are doubled for every 10^(@)C rise in temperature. Temperature coefficient gives us an idea about the change in the rate of a reaction for every 10^(@)C change in temperature. "Temperature coefficient" (mu) = ("Rate constant of" (T + 10)^(@)C)/("Rate constant at" T^(@)C) Arrhenius gave an equation which describes aret constant k as a function of temperature k = Ae^(-E_(a)//RT) where k is the rate constant, A is the frequency factor or pre-exponential factor, E_(a) is the activation energy, T is the temperature in kelvin, R is the universal gas constant. Equation when expressed in logarithmic form becomes log k = log A - (E_(a))/(2.303 RT) For a reaction E_(a) = 0 and k = 3.2 xx 10^(8)s^(-1) at 325 K . The value of k at 335 K would be

The rate of reaction increases isgnificantly with increase in temperature. Generally, rate of reactions are doubled for every 10^(@)C rise in temperature. Temperature coefficient gives us an idea about the change in the rate of a reaction for every 10^(@)C change in temperature. "Temperature coefficient" (mu) = ("Rate constant of" (T + 10)^(@)C)/("Rate constant at" T^(@)C) Arrhenius gave an equation which describes aret constant k as a function of temperature k = Ae^(-E_(a)//RT) where k is the rate constant, A is the frequency factor or pre-exponential factor, E_(a) is the activation energy, T is the temperature in kelvin, R is the universal gas constant. Equation when expressed in logarithmic form becomes log k = log A - (E_(a))/(2.303 RT) For which of the following reactions k_(310)//k_(300) would be maximum?

The temperature dependence of rate constant (k) of a chemical reaction is written in terms of Arrhenius equation, k=Ae^(-E_(a)//RT)) Activation energy (E_(a)) of the reaction can be calculate by plotting

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