Arrhenius equation follows k=A

Rate is directly proportional to the rate constant

The rate of reaction increase with the increase in the rate constant and the rate constant increases with increase in temperature as the exponential value () decreases and the numerator (A) remains constant so, the L.H.S value increases hence option (i) is correct.

A decrease in value of activation energy increases exponential value so rate constant increases as the rate are directly proportional to the rate constant its own value also increases simultaneously hence option (ii) is correct.

Option (iii) is incorrect as of the rate constant value increases exponentially with an increase in temperature as the denominator term () decreases with increase in temperature so L.H.S value increases as the numerator is a constant.

Option (iv) is incorrect as the rate of reaction increases with the decrease in activation energy value as clarified in option (ii).

The important fact the rate of reaction is proportion directly to rate constant k.