A voltaic cell employs the following redox reaction: PbO2 (s) + NO (g) → Pb2+ (aq) + NO3− (aq)  a) Balance the above reaction in acidic solution. b) Draw a diagram of the voltaic cell. Label the PbO2, NO, Pb2+, and NO3−. Indicate the direction of electron flow and the direction of anion and cation flow from the salt bridge. c) The PbO2/ Pb2+ half-reaction has a standard reduction potential (E°) of 1.46 V and the NO3-/ NO half-reaction has a standard reduction potential (E°) of 0.96 V. Calculate the potential of the cell at 25 °C under the following conditions: PNO 0.950 atm [Pb2+] 0.0500 M [NO3−] 0.0620 M pH 4.67

A galvanic cell was formed using Avium and Beanium:[hypothetical elements] Reduction Potentials: Av3+(aq) + 3e- → Av(s) Eo = -0.48 V Bn4+(aq) + 4e- → Bn(s) Eo = +0.15 V a) Write a net ionic equation for this reaction. b) Write the cell notation for this cell. c) Which is the oxidizing agent? Explain how you know.

a) Balance the following redox reaction in basic solution: H2O2(aq) + ClO2(aq) → ClO2-(aq) + O2(g) b) Sketch the voltaic cell for the redox reaction, labeling the direction for electron flow, the anode and cathode , and the species present in each half-cell. Show all the work please!

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.

Consider a voltaic cell in which the following reaction takes place. 2Fe 2+ (aq) + H₂O2 (aq) + 2 H+ (aq) --→2Fe ³+ (aq) +2H₂O (1) calculate Eº Calculate E and Gibbs free energy when [Fe²+] = 0.00813 M, [H₂O₂] = 0.914 M, [Fe ³+] = 0.199 M, [H] = 1.32 x 10³ M

Consider a galvanic cell created from the following redox reaction: 3Zn (s) + 2Au3+ (aq) → 3Zn2+ (aq) + 2Au (s) 1) Draw out a schematic diagram (as shown in image)  2) Label each component (anode, cathode, salt bridge, solution choice, and electron flow direction) in your schematic diagram.

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.