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

Verified Answer :

QueenNaae

Rate= 16 x 10 (-3)  answer B

Edufirst

The rate equation is R = k [HI]^2

Where R is the rate constant and [HI] is the molar concentration of HI.

Here k = 1.6 10 ^-3 M^-1 s^-1 and [HI] is 0.045 M.

Then you just need to replace the two values in the rate equation:

R = 1.6 10^-3 M^-1 s^-1 (0.045 M)^2 = 3.24 10^-6 M/s

Which using two significant figures is 3.2 * 10^-6 M/s

Then, the answer is the option B.

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