Nitrogen dioxide undergoes thermal decomposition according to the second-order reaction 2 NO2(g) → 2 NO(g) + O2(g). When 0.700 M NO2 is allowed to react for 90.0 seconds, its concentration falls to 0.0463 M. What is the rate constant for the reaction?

K = 0.2241 M-1 s-1

Explanation:

∴ a: NO2

∴ α = 2 second order

⇒ - δCa/δt = K Ca²

⇒ - ∫δCa/Ca² = K*∫δt

⇒ [ 1/Ca - 1/Cao ] = K*t

∴ Ca = 0.0463 M

∴ Cao = 0.700 M

∴ t = 90.0 s

rate constant (K):

⇒ - [ 1/0.0463 - 1/0.700 ] = K*(90.0 s)

⇒ 20.1697 M-1 = K*(90.0 s)

⇒ K = 0.2241 M-1 s-1

- aluminum and copper chloride.

- the chloride ion to separate the aluminum from the oxygen so that the aluminum can react with the copper ions (and the water molecules).

its first and third is your answer i did the qustion the fourth isnt right