What is the cell potential for a voltaic cell having one electrode composed of a Zn strip dipped in a 0.034 M Zn(NO)(aq) solution and the other electrode composed of a Zn strip dipped into a 0.414 M Zn(NO)(aq) solution? Assume all other cell components are in place and the temperature is 25.0°C.   To produce 1.21 kg of solid potassium from molten KCl, how many hours must 0.721 amps be passed through the KCl?   How many hours will you have to electrolyze the forks to apply 0.500 g of Ag to each one? Your electrolysis device operates at a current of 3.75 amps.

Consider the voltaic Cell shown below. Voltaic Cell V Voltmeter Salt Ag (s)-> bridge Cd (s) Ag+ (aq) 2.75 M Cd+2 (aq) 0.0125 M • What is the value of potential for the spontaneous reaction that occurs as the cell operates at 25°C? Ecell = • As the cell operates spontaneously under these conditions, which electrode is the cathode of the cell? Cd Ag • Which Electrode loses mass as the cell operates under these conditions? Ag Cd

When a lead acid car battery is recharged by the alternator, it acts essentially as an electrolytic cell in which solid lead(II) sulfate (PBSO4) is reduced to lead at the cathode and oxidized to solid lead(II) oxide (PbO) at the anode. Suppose a current of 46.0 A is fed into a car battery for 24.0 seconds. Calculate the mass of lead deposited on the cathode of the battery. Round your answer to 3 significant digits. Also, be sure your answer contains a unit symbol.

A galvanic cell at a temperature of 25.0°C is powered by the following redox reaction: 2Cr3+(aq)+3Ca(s)--->2Cr(s)+3Ca2+(aq) Suppose the cell is prepared with 1.96 M Cr3+ in one half-cell and 6.08 M Ca2+ in the other. Calculate the cell voltage under these conditions. Round your answer to 3 significant digits.

Write the cell notation for an electrochemical cell consisting of an anode where Zn (s) is oxidized to Zn²+ (aq) and a cathode where H* (aq) is reduced to H2₂ (g) at a platinum electrode . Assume all aqueous solutions have a concentration of 1 mol/L and gases have a pressure of 1 bar.

A voltaic electrochemical cell is constructed using the following reaction. The half-cell components are separated by a salt bridge. 2cl'(aq) + F2(g)– Cl2(g) + 2F'(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 v x the Cl electrode X the F, electrode. Anions migrate X the salt bridge X the Cl' compartment.

what is the standard cell potential (in Volts) for a a galvanic cell that can do 567 kJ of work. The number of electrons tranferred in the rxn is 4.

Write the cell notation for an electrochemical cell consisting of an anode where Cr²+ (aq) is oxidized to Cr³+ (aq) at a platinum electrode and a cathode where Ag* (aq) is reduced to Ag (s). Assume all aqueous solutions have a concentration of 1 mol/L.

A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2Cr³+ (aq) + 3 Ca(s) → 2Cr(s) + 3Ca²+ (aq) Suppose the cell is prepared with 6.35 M Cr³+ in one half-cell and 0.492 M Ca²+ in the other half. Calculate the cell voltage under these conditions. Cr³+ (aq) + 3e → Cr(s) Ca²+ (aq) + 2e →→ Ca(s) There are 6 galvanic cell. Er The standard cell potential (E°) for this galvanic cell is +2.124 red = -0.744 V Ered= -2.868 V volatage is 2.15 Under these conditions, the reaction quotient is moles of electrons transferred during to operate this V V. 0.00295 In order to increase the cell voltage for this cell ✔ [ Select ] V. and the cell It is impossible to change the voltage Not enough information Q>1 Q<1 3

[Fe3+]= 2.0×10−3 M; [Mg2+]= 3.15 M   Express your answer in units of volts.