Question
Which of the following statements is incorrect?
A.
Activation energy for the forward reaction is equals to activation energy for the reverse reaction
B.
For a reversible reaction, an increase in temperature increases the reaction rate for
both the forward and the backward reaction
C.
The larger the initial reactant concentration for a second order reaction, the shorter is
its half-life.
D.
When $$\Delta t$$ is infinitesimally small, the average rate equals the instantaneous rate
Answer :
Activation energy for the forward reaction is equals to activation energy for the reverse reaction
Solution :
$${E_a}\left( {F.R.} \right) \ne {E_a}\left( {B.R.} \right){E_a}$$ can be calculated.