Q. The reaction $2A + B + C \rightarrow D + E$is found to be first order in A, second in B and zero order in C. What is the effect on the rate of increasing concentration of A, B and C two times?
A) 72 times
B) 8 times
C) 24 times
D) 36 times
Explanation
(b)
The rate law for the reaction is as
r=$\frac{dx}{dt}$=k(A)$(B)^{2}(C)^{0}$=$k(A)(B)^{2}$
on increasing the concentration of A,B and C two times.
r’=$\frac{dx}{dt}$=k(2A)$(2B)^{2}(2C)^{0}$
=8k(A)$(B)^{2}$
Thus, the rate increases eight times.
Reviewed by Dr. Abubacker
Physics Educator & NEET/JEE Specialist
Ph.D. in Physics with 19+ years of teaching experience.