Order of a reaction is an experimental quantity.(1) Calculate the over

1.	Order of a reaction is an experimental quantity.(1) Calculate the overall order of a reaction which has the rate expression :(a) Rate = k[A]1/2 [B]3/2(b) Rate = k[A]3/2 [B]-1(2) The initial concentration of N2O5 in the following first order reaction N2O6(g) → 2NO2(g) + 1/2 O2(g) was 1.24 × 10-2 mol/L at 318 K.The concentration of N2O5, after 60 min was 0.20 × 10-2 mol/L. Calculate the rate constant of the reaction at 318 K.
Answer» (1). (a) Order = \(\frac{1}{2}+\frac{3}{2}\) = 2 (b) Order = \(\frac{3}{2}+(-1)\) = \(\frac{1}{2}\) (2). For a 1^st order reaction, k = \(\frac{2.303}{t}log\frac{[R]_0}{[R]}\) = \(\frac{2.303}{60}log\frac{1.24\,\times\,10^{-2}}{0.20\,\times\,10^{-2}}\) = \(\frac{2.303}{60}log\,6.2\,min^{-1}\) k = 0.0304 min^-1

Order of a reaction is an experimental quantity.(1) Calculate the overall order of a reaction which has the rate expression :(a) Rate = k[A]1/2 [B]3/2(b) Rate = k[A]3/2 [B]-1(2) The initial concentration of N2O5 in the following first order reaction N2O6(g) → 2NO2(g) + 1/2 O2(g) was 1.24 × 10-2 mol/L at 318 K.The concentration of N2O5, after 60 min was 0.20 × 10-2 mol/L. Calculate the rate constant of the reaction at 318 K.

Answer»

(1). (a) Order = \(\frac{1}{2}+\frac{3}{2}\) = 2

(b) Order = \(\frac{3}{2}+(-1)\) = \(\frac{1}{2}\)

(2). For a 1^st order reaction,

k = \(\frac{2.303}{t}log\frac{[R]_0}{[R]}\)

= \(\frac{2.303}{60}log\frac{1.24\,\times\,10^{-2}}{0.20\,\times\,10^{-2}}\)

= \(\frac{2.303}{60}log\,6.2\,min^{-1}\)

k = 0.0304 min^-1

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