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rate law for second order reaction

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The rate constant for the second-order reaction given below is 0.80/M·s at 10°C.

2 NOBr(g) ----> 2 NO(g) + Br2(g)

(a) Starting with a concentration of 0.080 M, calculate the concentration of NOBr after 13 s.

(b) Calculate the half-life when [NOBr]0 = 0.090 M.

(c) Find the half-life when [NOBr]0 = 0.044 M

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The solution is comprised of detailed explanations of rate law for second order reaction.

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The rate law for second order reaction is
- d[NOBr] / dt = k[NOBr]^2
After the integration, the concentration of NOBr at time t is
1/ [NOBr] =1/ [NOBr]_0 + kt
You should be able ...

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