isaacholton7
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Brainliest and 20 points for the correct answer.

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

2HI(g) → [tex] H_{2} [/tex](g) + [tex] l_{2} [/tex](g)

[tex] R=k[HI]^{2} [/tex]

At a given temperature, the rate constant is [tex] 1.6*10^{-3} M^{-1} s^{-1} [/tex]. What is the rate at this temperature for the given concentrations?

A.) [tex] 1.6*10^{-3} Ms^{-1}[/tex]

B.) [tex] 3.2*10^{-6} Ms^{-1}[/tex]

C.) [tex] 3.6*10^{-2} Ms^{-1}[/tex]

D.) [tex] 7.2*10^{-5} Ms^{-1}[/tex]

Respuesta :

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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