Question

1. Consider the reaction 2N₂O(g) -> 2N₂(g) + O₂(g)

A. (2) Express the reaction in terms of the change in the concentration of each of the reactants and products.

B. (2) In the first 15 seconds of the reaction, 0.015 mol of O₂ is produced. What is the average rate of the reaction during this time interval?

Answer 1

2N2O(g) -> 2N2(g) + O2(g)

mols of O2 produced in 15 sec= 0.015 mols
Average rate of reaction =
- 1/2{d(N2O)/dt} = 1/2{d(N2)/dt} = d(O2)/dt [note negative sign indicate disappearance of reactant as time passes]

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b) Suppose the container is of 1 Liter [If volume is specified you need to use that number in liters]

the concentration of O2 produced = moles of O2/volume
= 0.015 mols/1L= 0.015 mols/L

Average rate= 0.015 mols/L/15 sec = 0.001 M/s
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