in a reaction,2 NO2(g), <=> N2O4 the rate of disappearance of N2O4 is 2.95 mol/min. What is the rate of disappearance of NO2?
For each mole of N2O4 that disappears, two moles of NO2 are formed.
2.95 x 2 = ?
If they really want the rate of DISappearance of NO2, then you have to have a minus sign in front of the answer. Both species cannot be disappearing at the same time.
To find the rate of disappearance of NO2, you first need to determine the relationship between the rate of disappearance of N2O4 and NO2, which can be established from the balanced chemical equation.
The balanced chemical equation for the given reaction is:
2 NO2(g) <=> N2O4
From the equation, you can see that every 2 moles of NO2 react to form 1 mole of N2O4. This means the stoichiometric ratio between NO2 and N2O4 is 2:1.
Therefore, the rate of disappearance of N2O4 can be related to the rate of disappearance of NO2 using the stoichiometric ratio.
Rate of disappearance of NO2 = (Rate of disappearance of N2O4) * (1 / Stoichiometric coefficient of NO2)
In this case, the rate of disappearance of N2O4 is given as 2.95 mol/min, and the stoichiometric coefficient of NO2 is 2.
Rate of disappearance of NO2 = 2.95 mol/min * (1 / 2) = 1.475 mol/min
So, the rate of disappearance of NO2 is 1.475 mol/min.