Define average rate and instantaneous rate.

Define rate law and rate constant.

Derive integrated rate law for a zero order reaction A\(\longrightarrow \) product.

What is the order with respect to each of the reactant and overall order of the following reactions?
a) 5Br^-_(aq)+BrO₃^-_(aq)+6H⁺_(aq) ➝3Br_2(l)+3H₂O_(l)
The experimental rate law is Rate = k [Br⁻][BrO₃⁻][H⁺]²
b) CH₃CHO_(g)\(\overset { \Delta }{ \longrightarrow } \) CH_4(g)+CO_(g) the experimental rate law is
Rate =K[CH₃CHO]^{\(\frac{3}{2}\)}

The rate of the reaction X + 2y→ product is 4 x 10^-3 mol L^-1S^-1, if [X] = [Y] = 0.2M and rate constant at 400K is 2 x 10^-2s^-1, What is the overall order of the reaction.