I did 3 Experiments and got 3 rate as the following:
Exp1: (S2O8)2-:0.05M; I-:0.05M rate:1.7x10^-5 M/s
Exp2: (S2O8)2-:0.10M; I-:0.05M rate:3.4x10^-5 M/s
Exp3:(S2O8)2-:0.05M; I-:0.10M rate:3.6x10^-5 M/s
what effect does doubling [(S208)2-] have on the rate? By what factor does the rate increase?
what effect does doubling [I-] have on the rate? By what factor does the rate increase?
How do I calculate x, y for the rate law: Rate=K[(S208)2-]^x times [I-]^y? Do I substitute the value of[(S208)2-]and [I-] from each Exp?
How do I calculate the value of the rate constant K for each Exp and the average value?
To analyze the effect of doubling [(S2O8)2-] on the rate, we can compare the rates between Experiments 1 and 3. In Experiment 1, [(S2O8)2-] is 0.05 M and the rate is 1.7x10^-5 M/s. In Experiment 3, [(S2O8)2-] is doubled to 0.10 M, and the rate increases to 3.6x10^-5 M/s. Thus, we can see that doubling [(S2O8)2-] leads to an increase in the rate.
To determine the factor by which the rate increases when [(S2O8)2-] is doubled, we can take the ratio of the rates from Experiment 3 and Experiment 1:
(3.6x10^-5 M/s) / (1.7x10^-5 M/s) ≈ 2.12
This indicates that when [(S2O8)2-] is doubled, the rate increases by a factor of approximately 2.12.
Similarly, to analyze the effect of doubling [I-] on the rate, we can compare the rates between Experiments 1 and 2. In Experiment 1, [I-] is 0.05 M and the rate is 1.7x10^-5 M/s. In Experiment 2, [I-] is doubled to 0.10 M, and the rate increases to 3.4x10^-5 M/s. This demonstrates that doubling [I-] also leads to an increase in the rate.
To determine the factor by which the rate increases when [I-] is doubled, we can take the ratio of the rates from Experiment 2 and Experiment 1:
(3.4x10^-5 M/s) / (1.7x10^-5 M/s) ≈ 2
This indicates that when [I-] is doubled, the rate increases by a factor of approximately 2.
To calculate the values of x and y in the rate law equation Rate = K[(S2O8)2-]^x times [I-]^y, we need to use the experimental data. Comparing the rates from Experiments 1, 2, and 3, we can set up three equations:
Equation 1: (1.7x10^-5 M/s) = K[(0.05 M)^x][(0.05 M)^y]
Equation 2: (3.4x10^-5 M/s) = K[(0.10 M)^x][(0.05 M)^y]
Equation 3: (3.6x10^-5 M/s) = K[(0.05 M)^x][(0.10 M)^y]
By solving this system of equations, you can obtain the values of x and y, which represent the reaction orders with respect to [(S2O8)2-] and [I-], respectively.
To calculate the value of the rate constant K for each experiment, you can rearrange the rate law equation to solve for K:
K = Rate / [(S2O8)2-]^x times [I-]^y
Substitute the rate value and the corresponding concentrations of [(S2O8)2-] and [I-] from each experiment into this equation. This will give you the rate constant for each experiment. To calculate the average value of the rate constant, you can take the average of the individual rate constants obtained from the experiments.