The activation energy of a reaction is 94.14 KJ/mol and the value of rate constant at 40º C is 1.8 x 10-1 sec-1.

From the expression,  ∆Gθ = –2.303 RT logKeq  ∆Gθ for the reaction, = (2.303) (8.314 JK–1 mol–1 ) (300 K) log10  = –5744.14 Jmol–1  = –5.744 kJ mol–1 

The answer is.... Zero order

Unit of k explain that it is zero order reaction.

Given, Ea = 94.14 x103 J mol-1 , T = 40 + 273 = 313 K, K = 1.8 x 10-1 sec-1  By using,  A = antilog (10.9635) = 9.194 x1010 sec-l

your the answer 24º C

3.6 x 10-3 Ms-1 , 5.4 x 10-3 Ms-1

Second order

(a) : ΔHR = Ef - Eb = 180 - 200 = - 20 kJ mol–1. The correct answer for this question should be –20kJ mol– 1. But no option given is...

An experimentally determined expression which relates the rate of reaction with the concentration of reactants is called rate law while the rate of reaction when concentration of each reactant is...

The energy required to form the intermediate called activated complex is known as activation energy. Activation energy = Threshold energy – Average energy of the reactants