By Dickinson R.G.

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**Extra resources for The Combination of Hydrogen and Oxygen in the Presence of Activated Mercury**

**Sample text**

5 is equal to the experimental rate constant. One way of determining this rate constant, therefore, would be to calculate the average value of this ratio using all of the available data. 3. A general approach This is an approach for the determination of partial order that does not involve any checking of data and which can be used to determine partial orders of any value, integral or otherwise. It is well suited to computer-based analysis, If we continue with our example of the thermal decomposition of NO2 at 300 "C (and put to one side our knowledge that it is second-order) then, as already discussed, a plausible rate equation is J =k~[N02]~ ( 5 3) The quantity of interest in this equation is a and it appears as an exponent.

3. The partial order with respect to NO2 is 2 and, overall, the reaction is second-order. 5 is equal to the experimental rate constant. One way of determining this rate constant, therefore, would be to calculate the average value of this ratio using all of the available data. 3. A general approach This is an approach for the determination of partial order that does not involve any checking of data and which can be used to determine partial orders of any value, integral or otherwise. It is well suited to computer-based analysis, If we continue with our example of the thermal decomposition of NO2 at 300 "C (and put to one side our knowledge that it is second-order) then, as already discussed, a plausible rate equation is J =k~[N02]~ ( 5 3) The quantity of interest in this equation is a and it appears as an exponent.

This effect, however, is relatively small and for increases of temperature over a range of, say, 100 O C , it would be difficult to detect experimentally. 1 with an energy barrier to reaction that was very close to zero? In these circumstances most collisions will lead to chemical reaction; in other words, the fraction of successful collisions will be effectively constant and independent of temperature. Thus, experimentally, it would be difficult to detect any change in the rate of reaction with increasing temperature.