2NO + O2 yield 2NO2
Suppose that a particular moment during the reaction nitrogen monoxide (NO) is reacting at the rate of 0.074 M/s -1. At what rate is NO2 being formed?
The equation tells you that
2 moles of NO react to form 2 moles of NO2
This is a 1:1 ratio
This means that NO2 will form at the same rate that NO reacts, because as 1 mole of NO reacts to form 1 mole of NO2 .
Thus rate NO2 is formed at will be 0.058 M/s
To determine the rate at which NO2 is being formed, we need to analyze the stoichiometry of the reaction.
The balanced equation for the reaction is:
2NO + O2 -> 2NO2
From the balanced equation, we can see that for every 2 moles of nitrogen monoxide (NO) reacting, 2 moles of nitrogen dioxide (NO2) are being formed. This means that the rate of formation of NO2 is directly proportional to the rate of consumption of NO.
Given that the rate of consumption of NO is 0.074 M/s, we can use the stoichiometry of the reaction to determine the rate at which NO2 is being formed.
Since the stoichiometric ratio of NO to NO2 is 1:1, the rate at which NO2 is being formed is also 0.074 M/s.
Therefore, the rate at which NO2 is being formed is 0.074 M/s.