Short Answer TypeA reaction is second order in A and first order in B.
(i) Write the differential rate equation.
(ii) How is the rate affected on increasing the concentration of A three times?
(iii) How is the rate affected when the concentrations of both A and B are doubled?
A reaction is second order in A and first order in B.
Differential rate equation:-
(ii) On increasing the concentration of A three times i.e. 3A:
Rate = k[3A]2[B]=9k[A]2[B]=9(Rate) , i.e. 9 times the initial rate.
(iii) On increasing the concentration of A and B as 2A and 2B:
Rate1= k[2A]2[2B]=k(4x2)[A]2[B]=8k[A]2[B]=8 (Rate) , i.e. 8 times the initial rate.
A first order reaction takes 40 minutes for 30% decomposition. Calculate t1/2 for this reaction.
(Given log 1.428 = 0.1548)
For a first order reaction, show that time required for 99% completion is twice the time required for the completion of 90% of reaction.
Give reasons for the following:
(i) Bond enthalpy of F2 is lower than that of Cl2.
(ii) PH3 has lower boiling point than NH3Account for the following:
(i) Helium is used in diving apparatus.
(ii) Fluorine does not exhibit positive oxidation state.
(iii) Oxygen shows catenation behaviour less than sulphur
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