Consider the endothermic reaction XrarrY...

Consider the endothermic reaction `XrarrY` with the activation energies `E_(b) and E_(f)` for backward and forward reaction respectively . In general.

`E_(b)ltE_(f)`

`E_(b)gtE_(f)`

`E_(b)=E_(f)`

there is no definite relation between `E_(f) and E_(b)`

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Consider an eendothermic reaction XrarrY with the activation energies E_(b) and E_(f) for the backward and forward reaction, respectively. In general

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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 In a hypothetical reaction A rarr B , the activation energies for the forward and backward reactions are 15 and 9 kJ mol^(-1) , respectively. The potential energy of A is 10 kJ mol^(-1) . Which of the following is wrong?

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