For the following spontaneous reaction, identify the half-reaction that would occur at the anode and the half-reaction that would occur at the cathode of a voltaic cell.  2Al(s) + 6H+(aq) →2Al3+(aq) + 3H2(g)

consider the following voltaic cell. Which reaction occurs at the anode ? O Sn²+ (aq) + 2e → Sn(s) Au(s) → Au3-(aq) + 3e Sn(s) → Sn²+ (aq) + 2e- Au³+ (aq) + 3e² → Au(s) O O Sn(s) | Sn²+ (aq) || Au³+ (aq) | Au(s)

A chemist designs a galvanic cell that uses these two half-reactions: 3+ 2+ Fe (aq)+e → Fe (aq) Cro (aq) + 4H₂O(1)+3e¯ Cr(OH)3(s)+5 OH(aq) Answer the following questions about this cell. Write a balanced equation for the half-reaction that happens at the cathode. Write a balanced equation for the half-reaction that happens at the anode. Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is half-reaction spontaneous as written. 0 standard reduction potential Ed=+0.771 V 'red E 'red = -0.13 V ロ→ロ × x10 5

Analyze the components of a voltaic electrochemical cell. A voltaic electrochemical cell is constructed using the following reaction. The half-cell components are separated by a salt bridge. Hg2+(aq) + Cu(s)→ Hg(I) + Cu²+(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 to v the Hg+ electrode from v the Cu electrode. In the salt bridge, anions migrate to the Cu compartment [from v) the Hg compartment.

These are the relevant reactions for a zinc/copper galvanic cell in no particular order:   a) Cu2+(aq) + 2e– → Cu(s)   b) Zn(s) + Cu2+(aq) →Cu(s) + Zn2+(aq)   c) Zn(s) → Zn2+(aq) + 2e–   Identify which is the oxidizing reaction, the reducing reaction, and the overall reaction. Briefly explain WHY.

What reactions take place at the cathode and the anode when each of the following solutions is used in an electrolytic cell? Write the half-reaction equations for the anode and cathode, and state whether the reaction would result in metal being plated onto the object. 1.0 mol/L aluminum fluoride solution, AlF3(aq)

A particular voltaic cell operates on the reaction below, giving an emf of 0.853 V. Calculate the maximum electrical work (in kJ) generated when 20.2 g of zinc metal is consumed. Zn(s) + CI2(g) → Zn2+(aq) + 2 Cl −(aq)

Calculate Ecell (volts) for the galvanic cell containing the reaction shown below where the concentration of the ion at the anode is 0.400 M and the concentration of the ion at the cathode is 1.86 M.

A voltaic cell is based on a nitrate/NO half-cell and a NiCl2/Ni half-cell. (Heads up, the chloride ions in this reaction are bystander ions.) Eo for NO-3 (aq) → NO(g) = +0.96 Eo for NiCl2 (aq) → Ni(s) = –0.28  What is the cell potential of the reaction when pH = 2.7, [NO3-] = 1.5 M, PNO = 0.010 atm and [Ni2+] = 0.21 M

What reactions take place at the cathode and the anode when each of the following solutions is used in an electrolytic cell? Write the half-reaction equations for the anode and cathode, and state whether the reaction would result in metal being plated onto the object. 1.0 mol/L manganese iodide solution, Mn12(aq)