Electrode systems used in cell 2n/Zn²+ Cul Cuat 2. Zn/Znat Fe²+ Fest 3. Cu/cuat AS/Agr 4.Zn/Zn²+ Ag/Agr 5. Zn/Zn2+ 1₂/I- 6. Fe2+ ke st Bra Br at 7. Br₂/Br Cia 101 Calculations Cell potential, Ecell (volts) .83 41 .41 1.3 1.0 .41 .10 Negative electrode Zn zn си 2n Zn Fe CI Oxidation reaction Exidation in volts Reduction reaction EⓇ Preduction in volts A. Noting that oxidation occurs at the negative pole in a cell, write the oxidation reaction taking place in each of the cells. The other electrode system must undergo reduction; write the reduction reaction that occurs in each cell. B. Assume that E AB = 0.00 volts (whether in reduction or oxidation). Enter that value in the table for all of the silver electrode systems you used in your cells. Since Ecell = Eoxidation +Ereduction you can calculate Eº values for all the electrode systems in which the Ag.Ag system was involved. Enter those values in the table. C. Using the values and relations in Part B and taking advantage of the fact that for any given electrode system, Eoxidation=-Eroduction complete the table of E values. The best way to do this is to use one of the E values you found in Part B in another cell with that electrode system. That potential, along with Ell, will allow you to find the potential of the other electrode. Continue this process with other cells until all the electrode potentials have been determined.

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An analytical chemist measures the amount of Elements E₁ and E₂ in four samples of an unknown Substance. sample of E1 1 2 3 mass mass of E2 4 16.0 g 9.1 g 17.1 g 9.8 g 18.5 g 10.6 g 12.0 g 6.9 g It's known that X contains no elements other than E₁ and E₂. Using this information, answer the questions in the table below. Is X a pure substance or a mixture? If you don't have enough information to decide, choose can't decide. If you said X is a pure substance, calculate the mass of Element E₁ the analytical chemist would find in a new 10.0 g sample of X. Round your answer to 2 significant digits. O pure substance O mixture O (can't decide) g

1a. Determine the volume of 1.000 g of water (Densitywater = 0.9999 g/mL). 1b. Determine the volume of 1.000 g of ice (Density ce = 0.9168 g/cm³). (1 mL = 1 cm³) %3D %3D 1c. From the volumes above, what can we conclude about 1.000 g of water when it freezes?