Answer: [tex]mol^{-1}Ls^{-1}[/tex]
Explanation:
Rate law says that rate of a reaction is directly proportional to the concentration of the reactants each raised to a stoichiometric coefficient determined experimentally called as order.
[tex]Rate=k[A]^x[B]^y[/tex]
k= rate constant
x = order with respect to A
y = order with respect to A
Given : [tex]Rate=k[A]^1[B]^1[/tex]
[tex]k=\frac{rate}{[A]^1[B]^1}[/tex]
Putting the units of various quantities:
[tex]k=\frac{rate}{[A]^1[B]^1}[/tex]
[tex]k=\frac{molL^{-1}s^{-1}}{[molL^{-1}]^1[molL^{-1}]^1}[/tex]
[tex]k=mol^{-1}Ls^{-1}[/tex]
Thus units of rate constant are [tex]mol^{-1}Ls^{-1}[/tex]
