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Following data is obtained for the reaction, N_(2)O_(5) to 2NO + 1/2O_(2) a) Show that the reaction is of first order b) Calculate the half life period. |
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Answer» Solution :a) For first ORDER reaction `k=2.303/t log a/(a-x)` `k_(1) = 2.303/(300s) (log) ([1.6 xx 10^(-12)])/([0.8 xx 10^(-2)])= (2.303)/(300s) xx LOG2 = 2.303/(300s)xx (0.3010) = 2.3 xx 10^(-3)`s `k_(2)= (2.303)/(600s)(0.6021) = 2.3 xx 10^(-3)`s Since the magnitude of the RATE constant reamains the same, the reaction is of first order. b) `t_(1//2) = 0.693/k = 0.693/(2.3 xx 10^(-3)s) = 301.30`S |
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