Chemistry 30

In the following decomposition reaction,

 2 N₂O₅ → 4 NO₂ + O₂

oxygen gas is produced at the average rate of 9.1 × 10^-4 mol · L^-1 · s^-1. Over the same period, what is the average rate of the following:

• the production of nitrogen dioxide
• the loss of nitrogen pentoxide

Solution:

• From the equation we see that for every 1 mole of oxygen formed, four moles of nitrogen dioxide are produced. Thus, the rate of production of nitrogen dioxide is four times that of oxygen:

• Nitrogen pentoxide is consumed at twice the rate that oxygen is produced:

Consider the following reaction:

N₂(g) + 3 H₂(g) → 2 NH₃(g)

If the rate of loss of hydrogen gas is 0.03 mol · L^-1· s^-1, what is the rate of production of ammonia?

Solution:

From the balanced equation we see that there are 2 moles NH₃ produced for every 3 moles H₂ used. Thus: