The rate law for the reaction below is given by the expression $$k\left[ A \right]\left[ B \right]$$
$$A + B \to {\text{Product}}$$
If the concentration of $$B$$ is increased from $$0.1$$ to $$0.3\,mole,$$ keeping the value of $$A$$ at $$0.1\,mole,$$ the rate constant will be :
A.
$$3k$$
B.
$$9k$$
C.
$$\frac{k}{3}$$
D.
$$k$$
Answer :
$$k$$
Solution :
Rate constant is independent of concentration.
Releted MCQ Question on Physical Chemistry >> Chemical Kinetics
Releted Question 1
If uranium (mass number 238 and atomic number 92) emits an $$\alpha $$ -particle, the product has mass no. and atomic no.