igormacedorrn
Answered

In a study to determine the rate of the following reaction:
2NO(g)+O2​(g) = 2NO2​(g)


the concentration of NO was 0.0400 M at t = 5.0 s and 0.0225 M at t = 650.0 s. What is the average rate of the reaction during this time period?

Answer :

Answer:

The rate of reaction is - 2.868 * 10^-4 M/S

Explanation:

In the following reaction: 2 NO + O2 → 2NO2

NO will be consumed, when adding O2.

This means it will disappear. This is confirmed by the concentration at 5 seconds and 650 seconds.

A = -Δ[A] / ΔT   = [A2] - [A1] / T2 - T1

(0.225 - 0.04) / (650 - 5) = 0.185 / 645 = 2.868 * 10^-4 M/S

Since it will disappear, this number will be negative : - 2.868 * 10^-4 M/S

The rate of reaction is - 2.868 * 10^-4 M/S

okpalawalter8

Answer:

  • The average rate of the reaction during this time period = [tex]1.357*10^{-5} M/s[/tex]

Explanation:

Given :-

At t = 5s , [NO] = 0.0400M

At t = 650s , [NO] = 0.0225M

Reaction:

[tex]2NO(g) + O_2(g) ---> 2NO_2(g)[/tex]

Average rate of the reaction = [tex]-\frac{1}{2}*\frac{\delta [NO]}{\delta t}[/tex]

The negative sign is used as concentration of reactant decreases with time

Therefore,

Average rate of reaction = [tex]-\frac{1}{2} (\frac{0.0225 - 0.04}{650 - 5})[/tex]

Average rate of reaction = [tex]1.357*10^{-5} M/s[/tex]

For more information on rate of reaction, visit

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