Home
Class 12
CHEMISTRY
Compare Ea (activation energy) for a, b,...

Compare `E_a` (activation energy) for a, b, c and d.

A

`E_b gt E_c gt E_d gt E_a`

B

`E_a gt E_d gt E_c gt E_b`

C

`E_c gt E_b gt E_a gt E_d`

D

`E_d gt E_a gt E_b gt E_c`

Text Solution

Verified by Experts

The correct Answer is:
A

NA
Promotional Banner

Similar Questions

Explore conceptually related problems

For A + B to C + D, DeltaH = -20 kJ "mole"^(-1) . The activation energy for the forward reaction is 85 kJ. Then the activation energy for the backward reaction is ___

A : For exothermic reaction, DeltaH=E_a (forward) -E_a (backward) R : The value of activation energy for forward direction is less than activation energy for backward reaction.

For the first order reaction A rarr B +C , carried out at 27^(@) C . If 3.8 xx 10^(-16)% of the reactant molecules exists in the activated state , the E_(a) (activation energy) of the reaction is:

Adjoining diagram, represents the energy profile for the reaction : A + B rarr C +D . What is the valye of the activation energy for the reaction ? C +D rarr A +B ?

Given the following diagram for the reaction A+B rarr C+D The enthalpy change and activation energy for the reverse reaction, C+ D rarrA+ B are respectively.

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 activation eneries for forward and backward reactions in a chemical reaction are 30.5 and 45.4 kJ mol^(-1) respectively. The reaction is

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 If a reaction A + B rarr C is exothermic to the extent 30 kJ mol^(-1) and the forward reaction has an activation energy of 249 kJ mol^(-1) the activation energy for reverse reaction in kJ mol^(-1) is

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?