The Rate and Order of a Reaction
Autor: Aaron Cotton-Betteridge • March 21, 2016 • Lab Report • 488 Words (2 Pages) • 894 Views
Lab 3 -The Rate and Order of a Reaction
DATA TABLE
Trial | [FeCl3] | [KI] | Initial rate (s–1)1 |
1 | 0.01 M | 0.01 M | 0.0018931 |
2 | 0.01 M | 0.005 M | 0.0041108 |
3 | 0.005 M | 0.01 M | 0.0016864 |
4 | 0.0075 M | 0.005 M | 0.0050817 |
5 | 0.005 M | 0.0075 M | 0.004307 |
DATA ANALYSIS
To start our experiment we calculated our molar concentration of FeCI3 and KI for each reaction by dividing volume by our concentration of 0.02 M for both FeCI3 and KI and then dividing by the total volume of solution in the reaction, 0.04 L. For example, to calculate the molar concentrations for our first reaction we divided the 0.02 L of FeCI3 solution in the reaction by its molarity (which is equal to moles over liters) of 0.2 M / 1 L which gave us the moles of FeCl3 in that reaction. As previously stated we divided each reaction by the total volume of solution in the reaction which was 0.04 L. By doing this we calculated that the molar concentration of Iron Chloride III in our first reaction was 0.01 M.
Because both FeCI3 and KI had the same molarity, and there were only three volumes (collectively between FeCI3 and KI), and the same number of total volume we only need to calculate for three molar concentrations between each of the 5 reactions.
To calculate the order of the reaction in FeCI3 and Kl I followed the standard convention to derive a reactants order, but didn’t find conclusive results. I started by dividing the reactants of reaction one together and dividing them by the product of reaction two. I chose reaction one and two because they shared the same concentration of (0.005) n for their first reactants limiting the reaction to only one unknown variable for which I could now solve. Dividing the now only other concentration from reaction 1 by reaction two yielded a number raised to the unknown power which is equal to reaction ones initial rate by reaction two initial rate. The calculated relationship between reaction one and twos unknown exponent and initial rate allows us to solve for the unknown exponent by using the properties of log.
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