BRAINLIEST AND 50 POINTS FOR CORRECT ANSWER!! :DD


The decomposition of hydrogen iodide and its rate law are shown below. The concentration of HI is 0.045 M.


2HI(g) → \(H_{2}\)(g) + \(l_{2}\)(g)


\(R=k[HI]^{2}\)


At a given temperature, the rate constant is \(1.6*10^{-3} M^{-1} s^{-1}\). What is the rate at this temperature for the given concentrations?


A.) \(1.6*10^{-3} Ms^{-1}\)


B.) \(3.2*10^{-6} Ms^{-1}\)


C.) \(3.6*10^{-2} Ms^{-1}\)


D.) \(7.2*10^{-5} Ms^{-1}\)