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The values found for the equilibrium constant in each test tube are fairly constant. Although some values are off by a bit, this is probably due to human error, or the limitations of the measuring devices that were used. This is shown by the fact that the values found for the equilibrium in each test tube are in the range from 145 M-1 to 155 M-1. However the uncertainty of the results is approximately 10 M-1 proving the accuracy of the results.
For this experiment, acidified nitrate solution was used for both reactants.. The solution contained NO3 because neither Fe3+ ions nor SCN- ions exist by themselves. Since NO3 is soluble in nearly all solutions, it does not interfere with the reaction, and can therefore be used to isolate the Fe3+ and SCN- ions. The H+ however, acts a catalyst. It speeds up the reaction, by reducing the activation energy, but does not affect either the equilibrium or the equilibrium constant.
Conclusion:
The equilibrium constant for the reaction between Iron (III) and thiocyanate to form thiocyanoiron (III) was found to be approximately 1..