At 25∘C, 0.11 mol of N2O4 reacts to form 0.10 mol of N2O4 and 0.02 mol of NO2. At 90∘C, 0.11 mol of N2O4 forms 0.050 mol of N2O4 and 0.12 mol of NO2. From these data, it can be concluded that
A. N2O4 molecules react by a second order rate law.
B. N2O4 molecules react by a first order rate law.
C. N2O4 molecules react faster at 25∘C than at 90∘C.
D. the equilibrium constant for the reaction above increases with an increase in temperature.
D. Determining first or second order isn't done with different temperatures so neither A nor B are right.
C isn't right because increaing T increases the rate of reaction (usually).
So D must the the correct answer. Calculate Keq and see it K increases with T. .........N2O4 --> 2NO2
@25C I..........0.11........0
............E.........0.10.....0.02
K@25 C = (NO2)^2/(N2O4) = (0.02)^2/0.10 = ?
@90C I..............0.11........0
............E............0.05........0.12
K@90C = (0.12)^2/0.05 = ?
Compare the two K values at the two temperatures.
Thank you SOO much!
To answer this question, we first need to understand the reaction that is taking place between N2O4 and NO2. The balanced chemical equation for the reaction can be written as follows:
N2O4 ⇌ 2NO2
Now, let's analyze the given data at 25∘C:
- 0.11 mol of N2O4 reacts to form 0.10 mol of N2O4 and 0.02 mol of NO2
And at 90∘C:
- 0.11 mol of N2O4 forms 0.050 mol of N2O4 and 0.12 mol of NO2
By comparing these two sets of data, we can observe that the amount of N2O4 decreases while the amount of NO2 increases as the temperature increases. This indicates that the forward reaction (from N2O4 to NO2) is favored at higher temperatures.
Now, let's analyze the options:
A. N2O4 molecules react by a second order rate law.
We cannot conclude anything about the order of the reaction based on the given data. We haven't been provided with any information about the rate of the reaction.
B. N2O4 molecules react by a first order rate law.
Similar to option A, the given data doesn't provide any information about the rate law of the reaction. Therefore, this option cannot be concluded.
C. N2O4 molecules react faster at 25∘C than at 90∘C.
This conclusion is incorrect based on the given data. The reaction produces more NO2 at higher temperatures, indicating that the reaction occurs faster at 90∘C.
D. The equilibrium constant for the reaction above increases with an increase in temperature.
Based on the analysis of the given data, we can conclude that the equilibrium constant for the reaction increases with an increase in temperature. At higher temperatures, more NO2 is produced, suggesting that the forward reaction is favored.
Therefore, the correct answer is D. The equilibrium constant for the reaction above increases with an increase in temperature.