A 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 first order reaction takes 40 minutes for 30% decomposition. Calculate t1/2 for this reaction.
(Given log 1.428 = 0.1548)
A --> P
T=0 a 0
T=t (a-x) x
Now, it takes 40 min for 30% decomposition i.e. reactant left after 40 min is 70% of its initial concentration.
So,
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