The following decomposition reaction SO2Cl2-->SO2 + Cl2 was run in a laboratory. Following data collected:
Time(s) Pressure SO2Cl2 (ATM)
0 1
2500 .947
5000 .895
7500 . 848
10000 .803
What is the overall order of reaction?
Good
To determine the overall order of the reaction, we need to analyze the data given and examine how the pressure of SO2Cl2 changes over time.
The overall order of a reaction can be determined by calculating the reaction rate constant (k) using the rate law equation:
Rate = k[A]^m[B]^n
In this reaction, since SO2Cl2 is the only reactant, the rate law equation can be simplified to:
Rate = k[SO2Cl2]^x
To determine the overall order of the reaction, we need to find the value of x.
One way to do this is by calculating the reaction rate at different time intervals using the given pressure values and then comparing them.
Let's calculate the reaction rates at different time intervals:
Rate at 0 to 2500 s: (1 - 0.947) / (2500 - 0) = 0.0001832 atm/s
Rate at 2500 to 5000 s: (0.947 - 0.895) / (5000 - 2500) = 0.000104 atm/s
Rate at 5000 to 7500 s: (0.895 - 0.848) / (7500 - 5000) = 0.000094 atm/s
Rate at 7500 to 10000 s: (0.848 - 0.803) / (10000 - 7500) = 0.000095 atm/s
Looking at the calculated rates, we observe that the rate does not remain constant and decreases over time. This indicates that the reaction is slowing down as the reaction progresses.
Since the rate of reaction is dependent only on the concentration of SO2Cl2, and the rate is decreasing over time, we can conclude that the reaction is first order with respect to SO2Cl2. In other words, x = 1.
Therefore, the overall order of the reaction is 1st order.