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Rate constant k of a reactionn is depend...

Rate constant k of a reactionn is dependent on temperature `k=Ae^(-E_(a)//RT)`, k has the least value at

A

high T and high `E_(a)`

B

high T and small `E_(a)`

C

low T and low `E_(a)`

D

low T and high `E_(a)`

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The correct Answer is:
D
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Rate constant k of a reaction is dependent on temperatur: k=Ae^(Ea//RT) K has the least value at

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 which of the following reactions k_(310)//k_(300) would be maximum?

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 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

Arrhenius studies the effect of temperature on the rate of a reaction and postulted that rate constant varies with temperature exponentially as k=Ae^(E_(a)//RT) . Thuis method is generally used for finding the activation energy of a reaction. Keeping temperature constant, the effect of catalyst on the activation energy has also been studied. If the rate of reaction doubles for 10^(@)C rise of temperature form 290K to 300K, the activation energy of the reaction will be approximately :

A colliison between reactant molecules must occur with a certain minimum energy before it is effective in yielding Product molecules. This minimum energy is called activation energy E_(a) Large the value of activation energy, smaller the value of rate constant k . Larger is the value of activation energy, greater is the effect of temperature rise on rate constant k . E_(f) = Activation energy of forward reaction E_(b) = Activation energy of backward reaction Delta H = E_(f) - E_(b) E_(f) = threshold energy The rate constant of a certain reaction is given by k = Ae^(-E_(a)//RT) (where A = Arrhenius constant). Which factor should be lowered so that the rate of reaction may increase?

The rate of chemical reaction are strongly affected by temperature . Arrhenius (1889) gave following relation between rate contant and temperature . k=Ae^(-E_(a)//RT)" ".....(i) This equation is called Arrhenius equation. The constant 'A' is caleld Arrhenius of pre-exponential factor. Logarithm of equation (i) given : log_(10)k=log_(10)A(E_(a))/(2.3030RT)" ".....(ii) The rate constant for a reaction is . log_(10)"sec"^(-1)=14-(1.25xx10^(4)K)/(T) " ".....(iii) At what temperature, rate constant of the reaction is equal to the pre-exponenntial factor ?

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