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In order for a chemical reaction to occur, particles of the reactants involved must collide with one another at the correct angle and with the correct amount of energy.
The factors, which affect the rate of a reaction, are the surface area, nature of the reactants, concentration, temperature, and catalysts.
It woul be more likely that the reaction proceeds in a series of elementary reactions. As it was expected, an increase in temperature led to a faster rate for a chemical reaction.
In this lab, the order of the reaction will be determined with respect to the iodate ions. Rate of the reaction at 38 o C is 239.16 times faster then the reaction at room temperature.
In this experiment, two solutions will be mixed, and the completion of the reaction will be marked by a color change. The other contains the hydrogen sulfite ion (HSO3-) and soluble starch.
The net ionic equation is as follows: 5 HSO3- 2 IO3- I2 5 SO4-2 H2O 3 H It should be expected that the rate of this reaction will depend on the concentration of the biosulfite ion and the iodate ion. The difference between concentration 2 and 1 is two times smaller then the difference between rate 2 and 1.
However, is the reaction fifth order with respect to the biosulfite ion? Doubling the concentration of KIO3 increases the rate by factor of 4, so reaction is a second order.
It seems unlikely that five biosulfite ions would be able to simultaneously collide with two iodate ions. The second objective was to determine a difference on the rate of the reaction when the solution is 10o C higher than a room temperature.
The reactant chemical(s) are given on the left-hand side and the product chemical(s) on the right-hand side.
The two are connected with an arrow leading from the left to the right, symbolizing the reaction.