2. (10 pts) Consider the following second-order reaction: 2NO2(g) + 2NO(g)+O2(g) The rate constant is 0.54...

Question

Question

2. (10 pts) Consider the following second-order reaction: 2NO2(g) + 2NO(g)+O2(g) The rate constant is 0.54 M-15-1, at 300 °C.

Answer 1

Answer #1

Q2. The second order integrate rate law is given as :

1/[A] - 1/[A]_o = (k) * (t)

where [A]_o = initial reactant concentration = 0.62 M

[A] = final reactant concentration = 0.28 M

k = rate constant = 0.54 M^-1s^-1

t = time

Substituting the values,

1/(0.28 M) - 1/(0.62 M) = (0.54 M^-1s^-1) * (t)

1.96 M^-1 = (0.54 M^-1s^-1) * (t)

t = (1.96 M^-1) / (0.54 M^-1s^-1)

t = 3.6 s

It would take 3.6 seconds to reduce the concentration from 0.62 M to 0.28 M

Answer 2

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