A certain metal M forms a soluble sulfate salt M₂SO4. Suppose the left half cell of a galvanic cell apparatus is filled with a 2.50 M solution of M₂SO4 and the right half cell with a 1.25 mM solution of the same substance. Electrodes made of M are dipped into both solutions and a voltmeter is connected between them. The temperature of the apparatus is held constant at 25.0 °C. Which electrode will be positive? What voltage will the voltmeter show? Assume its positive lead is connected to the positive electrode. Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits. O left O right 1 olo Ar BH

M(NO3)3. Suppose the left half cell of a galvanic cell apparatus is filled with a 2.00 M solution of M(NO3), and A certain metal M forms a soluble nitrate salt the right half cell with a 1.00 mM solution of the same substance. Electrodes made of M are dipped into both solutions and a voltmeter is connected between them. The temperature of the apparatus is held constant at 30.0 °C. Which electrode will be positive? left O right What voltage will the voltmeter show? Assume its positive lead is connected to the positive electrode. 0 Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits. X olla Ar

13. The cell potential of an electrochemical cell with the cell reaction Al(s) + Cr3+(aq) →Cr(s) + Al3+(aq) is 1.63 V.  What is the maximum electrical work obtainable from this cell when 0.150 g of Al is consumed?

A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 3 Cu²+ (aq) + 2Al(s) → 3Cu (s) +2A1³+ (aq) 2+ Suppose the cell is prepared with 4.04 M Cu²+ in one half-cell and 4.43 M A1³+ in the other. Calculate the cell voltage under these conditions. Round your answer to 3 significant digits. x10 X 3 8 Ś

The oxidation of methanol, as described by the equation below, has a ΔG° value of -937.9 kJ/mol. What is the standard cell potential (in V) for a methanol fuel cell? 2 CH3OH (l) + 3 O2 (g) → 2 CO2 (g) + 4 H2O (l)

Balance the following reactions. Calculate the cell potential and the Gibbs free energy of these reactions at standard conditions. Identify the reactions with K > 1 among the following redox reactions. Write the line representations for the Galvanic cells, indicating the anode and 1. cathode. a. Cl2 + Br → Ct + Br2 b. Mnoa + H* + Ce → Cet + Mn2 + H20

A certain metal M forms a soluble nitrate salt M(NO3)3. Suppose the left half cell of a galvanic cell apparatus is filled with a 3.00 M solution of M(NO3)3 and the right half cell with a 30.0 mM solution of the same substance. Electrodes made of M are dipped into both solutions and a voltmeter is connected between them. The temperature of the apparatus is held constant at 35.0 °C. Which electrode will be positive? What voltage will the voltmeter show? Assume its positive lead is connected to the positive electrode. Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits. ☐ left ☐ x10 right ☑

The oxidation of methanol, as described by the equation below, has a ΔG° value of -938 kJ/mol. What is the standard cell potential (in V) for a methanol fuel cell? 2 CH3OH (l) + 3 O2 (g) → 2 CO2 (g) + 4 H2O (l)