Answer to Question #220740 in General Chemistry for max

Question

The rate of decomposition of dinitrogen oxide gas, NO_{2 (g)}, was studied at 650 K by evacuating 0.3 moles of the said gas in a 1-L container. After 30 minutes it was found out that 30.0% of NO₂ decompose to NO _(g) and O_{2 (g)}. Base on the rate law the order of reaction is second order. (a) What is the rate constant? (b) Calculate the half-life of the reaction (c) Determine the time required for the reaction to precede 75.0% to completion. (d) How many moles of NO₂ will remain after 40.0 minutes elapsed?

Answer 1

rate = k[NO]²[Cl₂]¹

5.1 x 10^-3 = k[0.5]²[0.5]

k = 0.0408 s^-1 atm^-2