Consider the gas-phase reaction between nitric oxide and bromine
at 273 ∘C
2NO(g)+Br2(g)→2NOBr(g).
The following data for the initial rate of appearance of NOBr were
obtained:
Experiment | [NO](M) | [Br2](M) | Initial Rate of Appearance of NOBr(M/s) |
1 | 0.10 | 0.20 | 24 |
2 | 0.25 | 0.20 | 150 |
3 | 0.10 | 0.50 | 60 |
4 | 0.35 | 0.50 | 735 |
What is the rate of disappearance of Br2 when [NO]= 8.1×10−2 M and [Br2]= 0.22 M ?
Express your answer using two significant figures.
The rate equation of this reaction can be written as:
Where k is the rate constant and n and m are the reaction orders. We can take experiments 1 and 2 (they have the same concentration of bromine, which cancel out) and calculate:
So, we have
Which means that n = 2.
Analogously, If we take experiments 1 and 3, we have the same concentration of NO, so we can use this:
So now we have:
So m = 1.
Knowing n and m, we can calculate the constant k using experiment 4 and the rate equation:
So,
We can now calculate the rate of appearence of NOBr with the given concentrations:
BUT we have to bear in mind that per each 2 moles of NOBr that dissappear, one mole of Br2 is consumed, so its rate of disappearance will be half this value, and with a negative value, since bromine is a reactant.: -8.7 M/s
Consider the gas-phase reaction between nitric oxide and bromine at 273 ∘C 2NO(g)+Br2(g)→2NOBr(g). The following data...
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