For a gaseous reaction, following data is given:
`ArarrB, k_(1)= 10^(15)e-^(2000//T)`
`C rarrD, k_(2) = 10^(14)e^(-1000//T)`
The temperature at which `k_(1) = k_(2)` is

For a gaseous reaction , following date is given : A rarr B , k_1=10^(15)e^(-2000//T) C rarrD , K _2 = 10^(14) e^(-1000//T) The temperature at which k_1 = k_2 is

A rarr B, k_(A)=10^(15) e^(-2000//T) C rarr D, k_(c)=10^(14) e^(-1000//T) Temperature at which k_(A)=k_(c) is

For the two gaseous reactions, following data are given A rarr B, k_(1) =10^(10) e^(-20,000//T), C rarr D, k_(2) =10^(12) e^(-24,606//T) the temperature at which k_(1) becomes equal to k_(2) is :

For the reaction, following data is given: AtoB,K_(1)=10^(15)"exp"^(((-2000)/T)),CtoD,K_(2)=10^(14)"exp"^(((-1000)/T)) The temperature at which K_(1)=K_(2) is

{:(A rarr B, k_(A)=10^(15)e^(-2000//T),),(C rarr D, k_(C )=10^(14)e^(-1000//T)):} Temperature T K at which (k_(A)=k_(C )) 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 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 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

For the two gaseous reactions , following data are given AtoB,k_(1)=10^(10)e^(-20,000//T) CtoD,k_(2)=10^(12)e^(-24606//T) the temperature at which k_(1) becomes equal to k_(2) is

For the reaction, following data is given AtoB:K_(1)=10^(15) exp ((-2000)/T)" "CtoD,K_(2)=10^(14) exp ((-1000)/T) The temperature at whilch K_(1)=K_(2) is