Answer: \(mol^{-1}Ls^{-1}\)
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.
\(Rate=k[A]^x[B]^y\)
k= rate constant
x = order with respect to A
y = order with respect to A
Given : \(Rate=k[A]^1[B]^1\)
\(k=\frac{rate}{[A]^1[B]^1}\)
Putting the units of various quantities:
\(k=\frac{rate}{[A]^1[B]^1}\)
\(k=\frac{molL^{-1}s^{-1}}{[molL^{-1}]^1[molL^{-1}]^1}\)
\(k=mol^{-1}Ls^{-1}\)
Thus units of rate constant are \(mol^{-1}Ls^{-1}\)
