Consider the following reaction: 2 H2(g) + 2 NO(g) → 2 H2O(g) + N2(g) If the concentration of NO changed from 0.100 M to 0.025 M in the first 15 minutes of the reaction, what is the average rate of the reaction during this time interval?

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Alleei Alleei · Answer 1 · 2020-03-03T11:43:00+01:00

Answer: The average rate of the reaction during this time interval is, 0.005 M/s

Explanation:

The given chemical reaction is:

[tex]2H_2(g)+2NO(g)\rightarrow 2H_2O(g)+N_2(g)[/tex]

The expression will be:

[tex]\text{Average rate of reaction}=\frac{C_2-C_1}{t_2-t_1}[/tex]

where,

[tex]C_2[/tex] = final concentration of [tex]NO[/tex] = 0.025 M

[tex]C_1[/tex] = initial concentration of [tex]NO[/tex] = 0.100 M

[tex]t_2[/tex] = final time = 15 minutes

[tex]t_1[/tex] = initial time = 0 minutes

Putting values in above equation, we get:

[tex]\text{Average rate of reaction}=\frac{0.025-0.100}{15-0}[/tex]

[tex]\text{Average rate of reaction}=0.005M/s[/tex]

Hence, the average rate of the reaction during this time interval is, 0.005 M/s