Write the balanced equation of the reaction that occurs in a voltaic cell made using aluminum and tin electrodes immersed in 1.00 Msolutions of Al3* and Sn2+. Use the standard electrode potentials listed below to answer this question. Sn-* + (aq) +2e¯ → Sn(s) Esn²*/Sn= -0.136 V AF*(aq)+3e¯ → Al(s) E°A3+/AI= -1.662V Не (aq)

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25°C.  Al(s) ∣ Al3+(aq), 0.115 M||  Al3+(aq), 3.89 M)∣Al(s)

For a galvanic cell based on the following half-reactions: Fe3+(aq) + e- → Fe2+(aq)Ag+(aq) + e- → Ag(s)

A voltaic electrochemical cell is constructed using the following reaction. The half-cell components are separated by a salt bridge. 21 (aq) + Cl2(g) → 2(s) + 2CI(aq) Write the reactions that take place at the anode and at the cathode, the direction in which the electrons migrate in the external circuit, and the direction the anions in the salt bridge migrate. Use smallest possible integer coefficients. If a box is not needed, leave it blank. Enter the reaction that takes place at the anode. Include state symbols: Enter the reaction that takes place at the cathode. Include state symbols: In the external circuit, electrons migrate v the Cl2 electrode v the I electrode. Anions migrate v the salt bridge v the Cl2 compartment.