Reaction Ecal (Meas) Quotient, Q OM) Cu 0.937V OM) | Cu 0.90 5V OM) Cu 0.23V OM) Cu415Y Ecall (Calc) Ece(Calc) Zn | Zn+2 (1.0 M) || Cu+2 (1.0 M) | Cu 0.937 V Zn | Zn+2 (1.0 M) || Cu+2 (0.10 M) | Cu 0.90 5V Zn | Zn+2 (0.10 M) || Cu+2 (1.0 M) | Cu 0.923V Zn | Zn+2 (0.10 M) || Cu+2 (0.10 M) | Cu 0.915 V Mg | Mg+2 (1.0 M) || Zn+2 (1.0 M) | Zn 0.848V Mg | Mg+2 (1.0 M) || Zn +2 (0.10 M) | Zn 0.887v Me Mg+2 (0.10 M) || Zn+2 (1.0 M) | Zn 0.858V Mg Mg+2 (0.10 M) || Zn+2 (0.10 M) | Zn 0.818 V Mg | Mg+2 (1.0 M) || Cu+2 (1.0 M) | Cu 809V. Mg | Mg 2 (1.0 M) || Cu+2 (0.10 M) | Cu 16V Mg Mg+2 (0.10 M) || Cu+2 (1.0 M) | Cu 1.750 V Mg | Mg+2 (0.10 M) || Cu+2 (0.10 M) | Cu789

Beaker Volume of KSCN No solution 1 0.50 mL 9.50 mL Part I: Data for Calibration Graph Accurate Concentration of potassium thiocyanate, KSCN stock solution: 0.001 M 0.2 M Fe(NO3)3- Iron(III)nitrate solution: 0.5M Volume of HNO3 solution 0.2 M Volume of 0.2 M Fe(NO3)3 solution 10.00 mL Absorbance 0.037 2 1.00 mL 9.00 mL 10.00 mL 3 2.00 mL 8.00 mL 10.00 mL 4 3.00 mL 7.00 mL 10.00 mL 0.122 0.313 0.547 5 4.00 mL 6.00 mL 10.00 mL 6 5.00 mL 5.00 mL 10.00 mL 0.791 0.868

Write a balanced redox reaction for the following electrochemical cell: Pt | Cu* (aq); Cu²+ (aq) || Fe3+ (aq) | Fe What is the correct balanced reaction for the cell?

h Oxidation: Cr2+ → Cr³+ + e Reduction: Cu²+ + 2 e¯ → Cu Net: 2 Cr²+ + Cu²+ What is the standard potential, Eºnet ? Standard Reduction Potentials Eº net Reduction Half-Reaction E° (V) Co³+ + e- → Co²+ 1.82 Au³ + + 3e- → Au(s) 1.50 Pd²+ + 2 e- → Pd 0.987 Ag++ e- → Ag(s) 0.80 Fe³+ + e- → Fe²+ 0.771 → Cu(s) 0.52 → Cu(s) 0.337 → Cut 0.153 → H₂(g) 0.00 → Sn(s) -0.14 Cu++ e- Cu²++2 e- Cu²++ e- 2H+ + 2 e- Sn²+ + 2 e- Co²+ +2 e- Cr³++ e- Fe²+ +2 e- Cr³+ +3 e- Zn²++ 2 e- A1³+ + 3 e- → Cu + 2 Cr³+ = V →Co(s) -0.28 → Cr²+ -0.41 → Fe(s) -0.44 → Cr(s) -0.74 → Zn(s) -0.763 →Al(s) -1.66

4. In addition to finding the right answer can you explain what is Determinate error (I think the correct answer is the 3rd option here but not sure if right)

Please help answer this

You begin preparation of the calibration curve to measure absorbance vs concentration of FeSCN2+. To do so, you add 2.422 mL of 0.200 M Fe(NO3)3 to a cuvette and then directly add 215 µL of 0.001 M KSCN. What is the resulting concentration of FeSCN2*, assuming complete conversion of SCN' to FeSCN2+? Enter your answer in units of mM to four digits after the decimal.

how do you solve 0.2860=0.059/2log[Cu2+]

4. You prepare several dilutions of an unknown compound. You measure the absorbance of each solution at 340 nm using a 1 cm cuvette (your results are listed in the table below). What is the extinction coefficient (in (M•cm)') of the compound? (Hint: assume that each of the individual values contains some degree of experimental error.) Concentration(uM) Absorbance at 340 nm 10.0 0.011 20.0 0.023 40.0 0.066 80.0 0.119 160.0 0.189

From the data in Table 2.5, compute the concentration of the undiluted and diluted ovalbumin samples (make sure to account for the appropriate dilution factors, DF, in the computation).