A reaction is first order in A and second order in B : How is the rate affected when the concentrations of both A and B are doubled?

A reaction is first order in A and second order in B . How is rate affected when concentration of B is tripled?

A reaction is first order in A and second order in B (i) Write the differential rate equation. (ii) How is the rate affected on increasing the concentation of B three times ? (iii) How is the rate affected when the concentration of both A and B are doubled ?

For the raction A+Brarr products, it is found that order of A is 2 and the order of B is 3. In the rate expression when the concentration of both A and B are doubled the rate will increases by a factor

A reaction is first order in A and second order in B i) Write differential rate equation. ii) How is rate affected when the concentration of B is tripled? iii) How is rate affected when the concentration of both A and B are doubled?

A reaction is first order in A secod order in B : (i) write differential rate equation. (ii) How is the rate affected when the concentration of B is tripled ? (iii) How is the rate affected when the concentration of both A and B is doubled?

(a) 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 concentration of both A and B doubled? (b) A first order reaction takes 40 minutes for 30% decomposition. Calculate t_(1//2) for this reaction. (Given log 1.428 = 0.1548)

A reaction is first order in A and of second order in B. Write the differential rate equation for the reaction.