Equilibrium H2SO4 making

The after intermediate H2SO4 making equilibrium curve equation is ... 

O = equilibrium percentage of after-H2SO4-making input SO2 that is oxidized in... 

The important point is that, at any one particular temperature, the equilibrium constant is just that—constant. This gives us a means of forcing the equilibrium to favour the products (or reactants) since the ratio of the two must remain constant. Therefore, if we increase the concentration of the reactants (or even that of just one of the reactants), more products must be produced to keep the equilibrium constant. One way to make esters in the laboratory is to use a large excess of the alcohol and remove water continually from the system as it is formed, for example by distilling it out. This means that in the equilibrium mixture there is a tiny quantity of water, lots of the ester, lots of the alcohol, and very little of the carboxylic acid in other words, we have converted the carboxylic acid into the ester. We must still use an acid catalyst, but the acid must be anhydrous since we do not want any water present—commonly used acids are toluene sulfonic acid (tosic acid, TsOH), concentrated sulfuric acid (H2SO4), or gaseous HC1. The acid catalyst does not alter the position of the equilibrium it simply speeds up the rate of the reaction, allowing equilibrium to be reached more quickly. 

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