From concentration data

But for a reaction with volume change, the rate is obtained from the following modified form  

In determining m, variation in A is not influenced by variation in B. For this, a large excess of B should be employed. The converse should be applied when determining n. When a large excess of one of the reactants was employed, the kinetics reduces from (m x n)th order to pseudo nth order and Equation 7.5 reduces to Equation 7.2. 

A factorized design can be performed to minimize the number of experiments as briefly explained in Example 7.1 and in the preceding section. 

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Cr at two field sites where other studies had inferred Cr(Vl) reduction from concentration data (Table 8). We are adding here unpublished data from one of those sites and three analyses from a third site where conditions are strongly oxidizing and Cr(Vl) reduction should not occur. All of the groundwater samples are enriched in the heavy isotope relative to SRM-979, indicating that Cr(VI) reduction has taken place. 

In previous chapters, we discussed two different ways to determine the value of an equilibrium constant K from concentration data (Section 13.2) and from thermochemical data (Section 17.11). In this section, we ve added a third way from electrochemical data. The following are the key relationships needed for each approach ... 

Obtaining reaction rates from concentration data... 

The form of the ANOVA table for multiple regression is shown in Table 4. The completed table for the linear model fitted to the fluorescence data is given in Table 5. This analysis of variance serves to test whether a regression line is helpful in predicting the values of intensity from concentration data. For the linear model we wish to test whether the fine of slope b adds a significant contribution to the zero-order model. The null hypothesis being tested is. 

Calculation of the Chemical Equilibrium Constant for an Ionic Dissociation Reaction From Concentration Data... 

I Calculate equilibrium constants from concentration data. 

At the beginning of this section, we gave data from the results of two experiments. Experiments 1 and 2, involving catalytic methanation. By substituting the molar concentrations from these two experiments into the equilibrium-constant expression for the reaction, you can show that you get the same value for both experiments, as you expect from the law of mass action. This value equals for methanation at 1200 K. Thus, besides verifying the validity of the law of mass action in this case, you can also see how an equilibrium constant can be obtained from concentration data. ... 

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