(b) The molar conductivity (^m) of the acetic acid is given as 5.27 x 104 S m² mol-¹ at a concentration of 100 mol m³. If the cell has a resistance of 33.01 S-1 when filled with 100 mol m³ KCl(aq) and 300.0 S-1 when filled with 100 mol m³ CH3COOH, calculate the measured conductivity (K) of 100 mol m³ KCl(aq). The conductivity (K) of water is 0.076 S m¹ at 25 °C.

The half-cells Ag+(aq. 1.0 M)|Ag(s) and H+(aq, ? M)|H2(1.0 bar) are linked by a salt bridge to create a voltaic cell. With the silver electrode as the cathode, a value of 0.902 V is recorded tor kcell at 298 K. Determine the concentration of H+ and the pH of the solution.

Galvanic cells harness spontaneous oxidationreduction reactions to produce work by producing a current. They do so by controlling the flow of electrons from the species oxidized to the species reduced. How is a galvanic cell designed? What is in the cathode compartment? The anode compartment? What purpose do electrodes serve? Which way do electrons always flow in the wire connecting the two electrodes in a galvanic cell? Why is it necessary to use a salt bridge or a porous disk in a galvanic cell? Which way do cations flow in the salt bridge? Which way do the anions flow? What is a cell potential and what is a volt?

Table 17-1 lists common half-reactions along with the standard reduction potential associated with each half-reaction. These standard reduction potentials are all relative to some standard. What is the standard (zero point)? lf is positive for a half-reaction, what does it mean? If is negative for a half-reaction, what does it mean? Which species in Table 17-1 is most easily reduced? Least easily reduced? The reverse of the half-reactions in Table 17-1 are the oxidation half-reactions. How are standard oxidation potentials determined? In Table 17-1, which species is the best reducing agent? The worst reducing agent? To determine the standard cell potential for a redox reaction, the standard reduction potential is added to the standard oxidation potential. What must be true about this sum if the cell is to be spontaneous (produce a galvanic cell)? Standard reduction and oxidation potentials are intensive. What does this mean? Summarize how line notation is used to describe galvanic cells.

A typical total phosphate concentration in a cell, [HPO42] + [H2PO4], is 2.0 102 M. What are the concentrations of HPO42 and HPO4 at pH 7.40?

Gibbs energy change, A¡G° , is related to cell potential, Eell, by the equation A;G° = –nFEel Part B where n is the number of moles of electrons transferred Calculate the standard cell potential at 25 ° C for the reaction and F = 96 500 C mol1 is the Faraday's constant. X(s) + 2Y*(ag)→+X²+(ag) +2Y(s) where A,H° = -675 kJ mol1 and A,S° = -393 J K-1 mol-1 Express your answer to three significant figures and include the appropriate units. • View Available Hint(s) ? HA Value Units %3D cell Submit Previous Answers X Incorrect; Try Again

Consider the following galvanic cell reaction at 25 oC, 4 Cr2+(aq) + O2(g) + 4 H3O+(aq) → 4 Cr3+(aq) + 6 H2O(l). Which of thefollowing statements best describes what would happen to the cell potential if the concentration of Cr2+ is increased?(a) The cell potential would become less positive.(b) The cell potential would become more positive.(c) The cell potential would remain the same.(d) It is impossible to tell.

Based on the cell notation of an electrochemical cell, Pt(s) | H2 (g, 1 atm) | H+ (aq,0.02M)|| Ag* (aq.0.15 M) Ag (s) (a) write the half-cell notation equation of the anode and cathode. (b) write the overall cell reaction equation. (c) given that the cell potential is +0.852 V, calculate the standard reduction potential of silver. (d) calculate the equilibrium constant for the reaction at 25 C.

The cell notation of an electrochemical cell is given as below. Zn(s) |Zn²*(aq, 1.0 M)|| H*(aq, 1.0 M)|H,(g, 1 atm)|Pt(s) (a) Given that the cell potential is +0.76 V at 25°C, calculate the standard electrode potential for Zn*/Zn. (b) The cell potential of the above cell is recorded as +0.67 V at 25°C when hydrochloric acid and 1.0 atm hydrogen gas is used. Calculate the pH of the hydrochloric acid.

The electromotive force of the cell Pb(s) PbSO4(s) Na2SO4.10H₂O(aq)|Hg2SO4(s) Hg() is 0.9647 V at 25 °C. The temperature coefficient is 1.74 x 10-4 V K-¹. What is the AH for the reaction in kJ mol-¹? Express your answer in four significant figures.