Home
Class 12
CHEMISTRY
The rate of reaction increases isgnifica...

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

Doubtnut Promotions Banner Mobile Dark

Text Solution

Verified by Experts

The correct Answer is:
A
`(k_(325))/(k_(335)) = (Ae^(-E_(a)//Rxx325))/(Ae^(-E_(a)//Rxx335))`
or `(3.2 xx 10^(8)s^(-1))/(k_(335)) = (e^(-0//Rxx325))/(e^(-0//Rxx335)) or e^(0) = 1`
`:. k_(335) = 3.2 xx 10^(-8) s^(-1)`
|

Topper's Solved these Questions

  • CHEMICAL KINETICS

    CENGAGE CHEMISTRY|Exercise Exercises Multiple Correct|34 Videos

  • CHEMICAL KINETICS

    CENGAGE CHEMISTRY|Exercise Exercises Single Correct|177 Videos

  • CHEMICAL KINETICS

    CENGAGE CHEMISTRY|Exercise Ex4.4 Objective|10 Videos

  • CARBOXYLIC ACIDS AND THEIR DERIVATIVES

    CENGAGE CHEMISTRY|Exercise Exercises Archives (Analytical And Descriptive)|34 Videos

  • COORDINATION COMPOUNDS

    CENGAGE CHEMISTRY|Exercise Archives Subjective|18 Videos

Similar Questions

Explore conceptually related problems

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 a reaction is doubled for every 10^(@)C rise in temperature . The increase in reaction rate as a result of temperature rise from 10^(@) C to 100^(@)C is

The rate of a chemical reaction doubles for every 10^(@)C rise in temperature .If the temperature is increased by 60^(@)C the rate of reaction increases by about

The rate of a chemical reaction doubles for every `10^@C` rise in temperature. If the rate is increased by `60^@C`, the rate of reaction increases by:

The rate of a chemical reaction doubles for every 10^@C rise in temperature. If .the rate is increased by 60^@C , the rate of reaction increases by:

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?

In a zero-order reaction for every `10^(@)` rise of temperature, the rate is doubled. If the temperature is increased from `10^(@)C` to `100^(@)C`, the rate of the reaction will become

In a zero-order reaction for every 10^(@) C rise of temperature, the rate is doubled. If the temperature is increased from 10^(@) C to 100^(@) C, the rate of the reaction will become:

Home
Profile