Answer:
The correct option is: B.) M^-1 s^-1
Explanation:
According to the rate law, the rate of a given chemical reaction is equal to the product of the reactant concentrations. Where, the exponents a and b are the partial orders for the concentration of X and Y, respectively.
The rate equation for the chemical reaction is:
Rate = k [X]ᵃ[Y]ᵇ
Here, k is the rate constant.
The concentration of X and Y reactants is given in mol.L⁻¹ or M (molarity).
The unit of rate of a chemical reaction is mol.L⁻¹.s⁻¹ or molarity per second M.s⁻¹
Given: rate = k [X][Y]
In the given rate equation, the exponents of concentrations of reactants X and Y is 1. Thus the overall order of the reaction is 2.
Therefore, it is a second order reaction.
Since the unit of rate is M.s⁻¹ and units of [X] and [Y] is M.
∴ [tex]Rate (M.s^{-1}) = k [X (M)] [Y (M)][/tex]
⇒ [tex]k = \frac{Rate (M.s^{-1})}{[X (M)] [Y (M)]} [/tex]
⇒ the unit of k in the given rate law equation = M⁻¹.s⁻¹
