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The gas phase decomposition of hydrogen iodide at 700 K HI(g)½ H2(g) + ½ I2(g) is second order in HI with a rate constant of 1.20×10-3 M-1 s-1. If the initial concentration of HI is 1.09 M, the concentration of HI will be M after 2.36×103 seconds have passed.

Respuesta :

Answer:

C HI = 0.2667 M

Explanation:

  • HI(g) → 1/2H2(g) + 1/2I2(g)

decomposition rate HI(g):

∴ a: HI(g)

  • - ra = (K)*(Ca)∧α

∴ K = 1.20 E-3 M/s.........rate constant

∴ α = 2.....second order

∴ Cao = 1.09 M.........initial concentration of HI(g)

⇒ Ca = ? .....t = 2.36 E3 s

⇒ - ra = δCa/δt = K Ca²

⇒ - ∫δCa/Ca² = K∫δt

⇒ [ 1/Ca - 1/Cao ] = K*t

⇒ 1/Ca = (K*t) + 1/Cao

⇒ 1/Ca = ((1.20 E-3/M.s)(2.36 E3 s)) + (1/1.09 M)

⇒ 1/Ca = 2.832/M + 0.9174/M

⇒ 1/Ca = 3.749/M

⇒ Ca = 0.2667 M

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