1.

From the rate expression for the following reactions, determine their order of reaction and the dimensions of the rate constants.(i) 3NO(g) → N2O(g) + NO2(g); Rate = k [NO]2(ii) H2O2(ap) + 3I–(aq) + 2H+ → 2H2O(l) + \({ I }_{ 3 }^{ - }\); Rate = k[H2O2] [I–](iii) CH3CHO(g) + CH4(g) + CO(g);  Rate = k [CH3CHO]\(\frac { 3 }{ 2 }\)(iv) C2H5Cl(g) → C2H4(g) + HCl(g); Rate = k[C2H5Cl]

Answer»

(i) Rate = k [NO]2
Order of reaction = 2
Unit of rate constant = (mol L-1)1-n x s-1
n = order of reaction = (mol L-1)1-2 x s-1 = L mol-1 s-1
Hence order of above reaction is 2 and its unit is L mol-1 s-1.
(ii) Rate = k [H2Og][I–]
Order of reaction = 1 + 1 = 2
Unit of rate constant = (mol L-1)1 – n x s-1
= (mol L-1)1 – 2 x s-1
= (mol L-1) x s-1 = L mol-1 x s-1
For the reaction order is 2 and unit of rate constant is L mol-1 s-1
(iii) Rate = k (CH3CHO)\(\frac { 3 }{ 2 }\)
Order of reaction= \(\frac { 3 }{ 2 }\)
Unit of rate constant = (mol L-1)1 – 15 x s-1 = mol-1/2 L1/2 s-1
(iv) Rate = k [C2H5CI]
Order of reaction = 1
Unit of rate constant = (mol L-1)1 – n x s-1 = s-1
Order is 1 and unit is s-1


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