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13 January, 21:50

Consider the following reaction: 2{/rm{ N}}_2 {/rm{O (}}g) /; / rightarrow /; 2{/rm{ N}}_2 (g) /; + /; {/rm{O}}_2 (g)

a. In the first 12.0 s of the reaction, 1.7*10-2 mol of {/rm{O}}_2 is produced in a reaction vessel with a volume of 0.240 L. What is the average rate of the reaction over this time interval?

b. Predict the rate of change in the concentration of {/rm{N}}_2 {/rm{O}} over this time interval. In other words, what is {/Delta [{/rm{N}}_2 {/rm{O}}]}/{/Delta t}?

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  1. 13 January, 22:18
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    a. 5.9 * 10⁻³ M/s

    b. 0.012 M/s

    Explanation:

    Let's consider the following reaction.

    2 N₂O (g) → 2 N₂ (g) + O₂ (g)

    a.

    Time (t) : 12.0 s

    Δn (O₂) : 1.7 * 10⁻² mol

    Volume (V) : 0.240 L

    We can find the average rate of the reaction over this time interval using the following expression.

    r = Δn (O₂) / V * t

    r = 1.7 * 10⁻² mol / 0.240 L * 12.0 s

    r = 5.9 * 10⁻³ M/s

    b. The molar ratio of N₂O to O₂ is 2:1. The rate of change of N₂O is:

    5.9 * 10⁻³ mol O₂/L. s * (2 mol N₂O/1 mol O₂) = 0.012 M/s
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