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?

On the diagram below sketch the regions where colour has developed and what colour each region is for each test tube. Given that the standard reduction potential for Fe (Fe2*(aq) + 2e→ Fe(s)) is -0.44 V, would any of the metals zinc, lead, or tin, be effective as a sacrificial anode to inhibit the corrosion of iron? Justify your answer and also indicate if this agrees with the given ɔbservations iron nail iron + tin iron + zinc iron + aluminium iron + copper Hint: there is no blue colour in the iron + zinc and iron + aluminium test tubes (and the pink colour is around the iron nail in these test tubes). There's blue colour here. Each test tube contains agar gel with phenolphthalein and potassium ferricyanide Use your observations to complete the following table. The first line has been completed to show you what is required.

How many hours are required to plate 12.00 g of nickel metal from 1.00 M NİSO4(aq), using a current of 3.00 A?

Calculate the cell potential for the reaction as written at 25.00 °C, given that [Cr²+] = 0.768 M and [Fe²+] = 0.0170 M. Use the standard reduction potentials in this table. Cr(s) + Fe²+ (aq) — Cr²+(aq) + Fe(s) E = V

An electrochemical cell is constructed by dipping a zinc rod in a solution of Zn(NO3)2(aq), dipping a cobalt rod in a solution of CoCl2(aq), and connecting them with a wire and a salt bridge. In the cell that is constructed, the metallic zinc is being oxidized. d. The standard cell potential for this electrochemical cell is 0.482 V and two moles of electrons are exchanged per mole of reaction. What is equilibrium constant, K, for the redox reaction described by this electrochemical cell at 298 K?

Consider the following electrochemical cell in which X is an unknown metal:       Pt (s) | Cl–(1 M) | Cl2 (1 atm) || X2+(1 M) | X (s)If the standard cell emf is 0.23 V, what is the standard reduction potential at 25○C for X2++ 2 e– → X (s)

A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 3Cu (aq) + 2A1 (s) 3Cu (s)+2A1* (aq) 2+ 3+ Suppose the cell is prepared with 2.15 M Cu“ in one half-cell and 7.31 M Al" in the other. Calculate the cell voltage under these conditions. Round your answer to 3 significant digits. AL Rights

Calculate the standard cell potential, E, for the equation Cr(s) + F,(g) → Cr**(aq) + 2F (aq) Use the table of standard reduction potentials. E• cell %3D V

A galvanic cell is powered by the following redox reaction: 2+ + 3 Cu²+ (aq) + Cr(OH)3(s) + 5OH¯(aq) → 3 Cut (aq) + Cro (aq) + 4H₂O(1) Answer the following questions about this cell. If you need any electrochemical data, be sure you get it from the ALEKS Data tab. Write a balanced equation for the half-reaction that takes place at the cathode. Write a balanced equation for the half-reaction that takes place at the anode. Calculate the cell voltage under standard conditions. Round your answer to 2 decimal places. 0 0 0 E = v V ロ→ロ X 5

Balance the following redox reaction in acidic solution Ag (s) + Cr2O72- (aq) à Ag+ (aq) + Cr3+ (aq)