[NOBr]_0 = 0.900 M half-life 2.00 s

The rate law for the reaction

2NOBr(g) → 2NO(g) + Br2(g)

at some temperature is

Rate = –Δ[NOBr] / Δt = k [NOBr]^2

a. If the half-life for this reaction is 2.00 s

when [NOBr]_0 = 0.900 M,

calculate the value of k for this reaction.

b. How much time is required for

the concentration of NOBr to decrease to 0.100 M?

Rate = k [NOBr]^2 에서,

[NOBr]^2 이므로,

---> 2차 반응

2차 반응의 반감기

t_1/2 = 1 / (k [A]_0)

( 참고 https://ywpop.tistory.com/25 )

k = 1 / (t_1/2 × [A]_0)

= 1 / (2.00 s × 0.900 M)

= 0.556 /M•s

2차 반응 속도식

(1 / C_t) = k•t + (1 / C_0)

t = [(1 / C_t) - (1 / C_0)] / k

= [(1 / 0.100) - (1 / 0.900)] / 0.556

= 15.987 s

= 16.0 s

[키워드] 2차 반응 기준

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