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The number of reacting species (atoms, ions or molecules) taking part in an elementary reaction, which must collide simultaneously in order to bring about a chemical reaction is called molecularity of a reaction. In the rate equation Rate \(=k[\mathrm{~A}]^x[\mathrm{~B}]^y\)
\(x\) and \(y\) indicate how sensitive the rate is to the change in concentration of A and B, respectively. Sum of these exponents, i.e., \(x +y\) gives the overall order of a reaction where \(x\) and \(y\) represent the order with respect to the reactants A and B respectively. Hence, the sum of powers of the concentration of the reactants in the rate law expression is called the order of that chemical reaction. For a first order reaction, the concentration of the reactant varies as \([\mathrm{R}]=[\mathrm{R}]_0 e^{-k t}\)
The units of first and zero order rate constant of reactions are respectively:

Question

Accepted Answer

(C) M, s^{-1}

Answer

(A) s^{-1}, M s^{-1}

Answer

(B) M s^{-1}, s^{-1}

Answer

(D) s^{-1}, M

List-I (Function f(x))	List-II (Interval)
(A) \(f(x)=x\|x\|\)	(I) Decreases on \((0, \infty)\)
(B) \(f(x)=x^2+2 x-5\)	(II) Increases on \((3, \infty)\)
(C) \(f(x)=x^2-6 x+9\)	(III) Decreases on \((-\infty,-1)\)
(D) \(f(x)=-x^2\)	(IV) Increases on \((-\infty, \infty)\)

Answer & Solution

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X	0	1	2
P(X)	k	2k	3k