Hi, So I collected the data and just need answers for these questions. not sure where to start and don't understand them. Please, answer all or don't answer. Thanks in advance and I appreicate it. I'll rate it if you do answer all, and I appreciate your help!Conclusions:
1. Create a data table that displays the voltage of each trial (Ecell) and the temperature of each trial. Then, calculate and display as a calculated column ?G for the cell at each of the temperatures, using ?G = -n F E.
2. Calculate a ?G0 value for each temperature, given that ?G = ?G0 + RT ? ln Q, and include a calculated column for this in your data table.
3. Calculate and include a column for an E0 value for 25 0C, given your E0 value and the relationship ?G0 = -nFE0 . Using the standard reduction potential table, calculate an accepted E0 value at 250C. Then, calculate your percentage of error. Offer explanation for why these values are different!
4. Determine the equilibrium constant K for this reaction from your value of ?G0 at 250C, given that ?G0 = - RT ? ln K. Include a calculated column in your data table for K. Assume 250C for the standard free energy in order to determine the equilibrium constant.
5. What is the relationship between temperature and cell potential, E?
6. What is the relationship between cell potential, E, and ?G? Explain why this makes sense!
7. Define the Faraday constant, F.
8. Are most oxidation/reduction reactions exothermic, endothermic, or both, do you think? Explain why you think this?
9. Should your reaction be exothermic or endothermic? Explain in terms of your calculated energy and/or voltage values!
10. From your value of ?G0 at 250C, and an accepted value of ?S0 , calculate the ?H0 for this reaction at standard temperature conditions. Is this consistent with your answer to number 9? Explain!
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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.
