Reaction: N2O (g) -> 2N2 (g) + O2 (g) Performed at a temperature of 575 ° C across platinum in a zero-order reaction. In the gas phase, the following findings were obtained: Experiment [N2O] M Initial Rate, M/min 1 0.312 0.007418 2 1.248 0.1187 3 2.184 0.3635 1. write the rate law for the gas phase response from the findings in the table and find the rate constant.
Reaction: N2O (g) -> 2N2 (g) + O2 (g)
Performed at a temperature of 575 ° C across platinum in a zero-order reaction.
In the gas phase, the following findings were obtained:
|
Experiment |
[N2O] M |
Initial Rate, M/min |
|
1 |
0.312 |
0.007418 |
|
2 |
1.248 |
0.1187 |
|
3 |
2.184 |
0.3635 |
1. write the rate law for the gas phase response from the findings in the table and find the rate constant.
2. The following mechanism was proposed for this response:
Fast equilibrium: 2N2O (g) <--> N4O2
Slow process: N4O2 (g) ---> 2N2 (g) + O2 (g)
Get the rate law out of the mechanism. Is it suitable for the experimental results?
3. Suggest a suitable drawing to determine the order of the reaction and determine the speed of the reaction and explain the calculations:
-
- For the reaction on platinum
- For the reaction in the gas phase.
Explain your answer
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