Can someone help me with these calculations? I am very confusedwith how to do them. If you can help, please email me [email protected] so I can text you my data. Also, comment onthis of course so I can give you the points after the help.
Graph of absorbance versus concentration using the average absorbance values, (see manual introduction for graph requirements and Excel Tutorial posted on Sakai for assistance on making a graph.) Conversion of absorbance readings to concentration values for kinetics trials. Graph of [CV] versus time for first three kinetic trials. (Put all three trials on the same axes.) Graph of ln[CV] versus time for first three kinetic trials. (Put all three trials on the same axes.) Graph of 1/[CV] versus time for first three kinetic trials. (Put all three trials on the same axes.) Comparison of linear fit of the reaction orders to one another to determine order of reaction with respect to crystal violet. Graph of appropriate relationship between [CV] and time for last three kinetic trials. (Put all three trials on the same axes. See Excel Tutorial on Sakai site for directions.) Determination of the concentration of OH' in the reaction tube immediately after mixing with crystal violet in Parts 2 and 3 of the experiment. Determination of order of reaction with respect to [OH']o using the ratio of the slope for best fit of first three kinetic trials to the slope for the best fit of the last three kinetic trials, as shown here (slopes may be positive or negative whereas k is always positive): Recall that k' = k[OH] - you are solving for "n". Calculate the rate constant "k" for each kinetic trial, the average rate constant, and the standard deviation for rate constant. Include each of the values you will address in the Discussion. written in paragraph-form, describe each of the following: Does the rate of the reaction change as the reaction progresses? Support your conclusion. What is the order of the reaction with respect to each of the reactants (both crystal violet and sodium hydroxide)? Support your conclusions. What was the percent error in the order of reaction with respect to NaOH from your results? Is it significant (large or small compared to the value)? Support your conclusion. Write the rate law for the reaction and identify the value for the constant. How do you quantify error for each part in this experiment? To what sources do you attribute error for each part of your experiment? Explain how the suspected sources could contribute to the magnitude and direction of the error.
PROCESSING THE DATA 1. Write the Kc expression for the reaction in the Data and Calculation table. 2. Calculate the initial concentration of Fe3+, based on the dilution that results from addingKSCN solution and water to the original 0.0020 M Fe(NO3)3 solution. See Step 2 of theprocedure for the volume of each substance used in Trials 1-4. Calculate [Fe3+]i using theequation:
[Fe3+]i =
Fe(NO3)3 mLtotal mL X (0.0020 M)
This should be the same for all four test tubes. 3. Calculate the initial concentration of SCNâ, based on its dilution by Fe(NO3)3 and water:
[SCNâ]i =
KSCN mLtotal mL X (0.0020 M)
In beaker 1, [SCNâ]i = (2 mL / 100 mL)(.0020 M) = .000040 M. Calculate this for the otherthree beakers. 4. [FeSCN2+]eq is calculated using the formula:
[FeSCN2+]eq =
AeqAstd
X [FeSCN2+]std
where Aeq and Astd are the absorbance values for the equilibrium and standard solutions, respectively, and [FeSCN2+]std = (1/100)(0.0020) = 0.000020 M. Calculate [FeSCN2+]eq foreach of the four trials. 5. [Fe3+]eq: Calculate the concentration of Fe3+ at equilibrium for Trials 1-4 using the equation:
[Fe3+]eq = [Fe3+]i â [FeSCN2+]eq
6. [SCNâ]eq: Calculate the concentration of SCN- at equilibrium for Trials 1-4 using theequation:
[SCNâ]eq = [SCNâ]i â [FeSCN2+]eq
7. Calculate Kc for Trials 1-4. Be sure to show the Kc expression and the values substituted infor each of these calculations. 8. Using your four calculated Kc values, determine an average value for Kc.
