Consider the chemical reaction below equated
2N2O5 (g) -> 4NO2 (g) + O2 (g)
knowing that a certain period of time, N2O5 consumption rate is 0.10 mole / s, determine for the same time interval:
a) the average rate of formation of NO2
b) the average speed O2 formation
I have re-balanced your equation.
2N2O5 (g) -> 4NO2 (g) + 5O2 (g)
a)0.1 mol/s x (4 mols NO2/2 mols N2O5)
b) same process.
To determine the average rate of formation of NO2 and the average speed of O2 formation, we need to use the stoichiometry of the chemical reaction and the given consumption rate of N2O5.
a) Average rate of formation of NO2:
From the balanced chemical equation, we see that for every 2 moles of N2O5 consumed, 4 moles of NO2 are formed. Therefore, the mole ratio is 2:4.
Given that the consumption rate of N2O5 is 0.10 mole/s, we can use this information to find the average rate of formation of NO2.
Since the mole ratio of N2O5 to NO2 is 2:4, the average rate of formation of NO2 will be twice the consumption rate of N2O5.
Therefore, the average rate of formation of NO2 is:
2 * N2O5 consumption rate = 2 * 0.10 mole/s = 0.20 mole/s
b) Average speed of O2 formation:
From the balanced chemical equation, we see that for every 2 moles of N2O5 consumed, 1 mole of O2 is formed. Therefore, the mole ratio is 2:1.
Using the same consumption rate of N2O5, we can determine the average speed of O2 formation.
Since the mole ratio of N2O5 to O2 is 2:1, the average speed of O2 formation will be half the consumption rate of N2O5.
Therefore, the average speed of O2 formation is:
1/2 * N2O5 consumption rate = 1/2 * 0.10 mole/s = 0.05 mole/s
So, the average rate of formation of NO2 is 0.20 mole/s and the average speed of O2 formation is 0.05 mole/s.
To determine the average rate of formation of NO2 and the average rate of formation of O2, we need to compare the stoichiometric coefficients of the given balanced chemical equation.
a) Average rate of formation of NO2:
From the balanced chemical equation, we can see that the molar ratio between N2O5 and NO2 is 2:4, which simplifies to 1:2. This means that for every 1 mole of N2O5 consumed, 2 moles of NO2 are formed.
Given that the N2O5 consumption rate is 0.10 mol/s, we can calculate the average rate of formation of NO2 by multiplying the consumption rate by the stoichiometric ratio:
Average rate of formation of NO2 = 0.10 mol/s * (2 mol NO2 / 1 mol N2O5) = 0.20 mol/s
Therefore, the average rate of formation of NO2 is 0.20 mole/s.
b) Average rate of formation of O2:
From the balanced chemical equation, we can see that the molar ratio between N2O5 and O2 is 2:1. This means that for every 2 moles of N2O5 consumed, 1 mole of O2 is formed.
To find the average rate of formation of O2, we can use the same approach as in part a):
Average rate of formation of O2 = 0.10 mol/s * (1 mol O2 / 2 mol N2O5) = 0.05 mol/s
Therefore, the average rate of formation of O2 is 0.05 mole/s.