Consider the following voltaic cell at 298K. Select only the statements that are TRUE. Cu (s) I Cu²+ (1.0 M) II A³+ (1.0 M) 1 Al (s) Al³+ (aq) + 3 e→→ Al(s) red = -1.66V Cu²+ (aq) + 2e → Cu(s) The anode is Cu(s). E E In the Nernst equation, the value of n = 5. Al³+ (aq) is reduced. red = 0.34V The reducing agent is Al³+ (aq).

For a voltaic cell based on the reaction below, what reaction happens at the cathode?Zn(s)+2H+(aq)→Zn2+(aq)+H2(g)   Zn(s)→Zn2+(aq)+2e-   2H+(aq)+2e-→H2(g)   Zn2+(aq)+2e-→Zn(s)   H2(g)→2H+(aq)+2e-

Cr(s) Cr(NO3)3 A Voltaic Cell NaCl(aq) Pb(s) Pb(NO3)2 Cr³+ (aq) + 3 eCr (s) E° = -0.41 V Pb²+ (aq) + 2 e¯¯ → Pb (s) E° = -0.12 V The concentration of the solutions in each half-cell is 1.0 mol/L. Placing some Cr(s) in a solution containing Pb2+ ions. Placing some Pb(s) in a solution containing Cr³+ ions. O Placing some Cr(s) in a solution containing Cr³+ ions. O Placing some Pb(s) in a solution containing Pb³+ ions. Based on the given reduction potentials, which of the following would lead to a reaction?

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.

3. The oxidation of methanol, as described by the equation below, has a AG value of -937.9 kJ/mol. What is the standard cell potential for a methanol fuel cell? 2CH3OH +30₂ → 2CO₂ + 4H₂O

Consider the reaction: Fe(s) + CuSO4(aq) → FeSO4(aq) + Cu(s) What is the half-cell reaction for reduction? Multiple Choice О Fe(s) -> Fe2+(aq) + 2 e- Cu2+(aq) + 2 e-→ Cu(s) О Cu(s) → Cu2+(aq) + 2e- Fe(s) + 2 e-→ Fe2(aq)

A digital watch battery draws 0.10 milliamperes of current, which is provided by a mercury battery whose net reaction is: HgO(s) + Zn(s) → ZnO(s) + Hg(l) If a partially used battery contains 1.10 g of each of these four substances, for how many hours will the watch continue to run?

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.

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)

Do the work on paper please