150 8. Molecular iodine dissociates at 625 K with a first-order rate constant of

Question

150 8. Molecular iodine dissociates at 625 K with a first-order rate constant of 0.271s. What is the half-life of this reaction? 9. The reaction NOx) + COr) CO2 g) + NO has a rate constant of 2.57 M ,S-1 at 201 K and 567M-1'5-1 at So5K. Find the activation energy in ku mol ( in-1), 10. Ir 24 x 10 g o NOBr decomposes in a 20 x 10 ml fak in 0 minutes, find the average a T, )) rate of Br production: 2 NOBng-2 NOO-Bro 11. Ozone naturally decomposes to oxygen by this reaction: 2 Os(g)-3 Odg) The experimentally observed rate law for this reaction is: Rate kioto2l-1 Show that this proposed mechanism is consistent with the experimentally observed rae law. Slow 12. Calculate the value of Ap cr K, for each of the following at 27 C (a) 2 so,(g) +0,(g) 2 So,(g) K,-8x102, (b) NAs) + 20,(g) 2N02(g) ,-3x10-17 13. Write the equilibrium constant expressions, K, and predict the position of equilibrium for the following -4.6 x 10 2lag) 2 1.0 x 10 (b) Ca(NO,); aq + H,so.aq Caso, + 2HNO3

Explanation / Answer

Half-life of a First order kinetics is given by the realtionship, t1/2 = 0.693/k

Here, Rate constant, k = 0.271 s-1

Therefore,  t1/2 = 0.693/k = 0.693/0.271 = 2.55 s

Half life of dissociation of molecular Iodine is  2.55 s

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