Based on the zinc / copper electrochemical cell in Table 10.1, which statement is correct? O Zinc is the anode, copper is the cathode and the overall cell voltage is negative. O Zinc is the cathode, copper is the anode and the overall cell voltage is negative. Zinc is the cathode, copper is the anode and the overall cell voltage is positive. O Zinc is the anode, copper is the cathode and the overall cell voltage is positive.

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) Ered = -0.744 V Ca2+ (aq) + 2e → Ca(s) Ered = -2.868 V The standard cell potential (E°) for this galvanic cell is [Select] V. There are [ Select] + moles of electrons transferred during to operate this galvanic cell. Under these conditions, the reaction quotient is [Select] and the cell volatage is [Select] V. In order to increase the cell voltage for this cell, [Select ]

A galvanic (voltaic) cell consists of an electrode composed of aluminum in a 1.0 M aluminum ion solution and another electrode composed of gold in a 1.0 M gold(III) ion solution, connected by a salt bridge. Calculate the standard potential for this cell at 25 °C. Refer to the list of standard reduction potentials. Excell V

A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2+ Cu2+ (aq) + Zn (s) → Cu (s) + Zn²+ (aq) 2+ Suppose the cell is prepared with 3.51 M Cu²*+ in one half-cell and 1.20 M Zn²+ in the other. Calculate the cell voltage under these conditions. Round your answer to 3 significant digits. 日 ☐ x10 ☐ μ ロ・ロ

Thomas Edison invented an electric meter that was nothing more than a simple coulometer, a device to measure the amount of electricity passing through a circuit. In this meter, a small, fixed fraction of the total current supplied to a household was passed through an electrolytic cell, plating out zinc at the cathode. Each month the cathode could then be removed and weighed to determine the amount of electricity used. If 0.25% of a household’s electricity passed through such a coulometer and the cathodeincreased in mass by 1.83 g in a month, how many coulombs of electricity were used during that month?

Calculate the cell voltage under these conditions. Round your answer to 3 significant digits.

What is the maximum voltage that can be produced by a galvanic cell with the following electrodes? Copper and Lead Zinc and Lithium

How long would it take to deposit 7.54 g of copper (molar mass 63.55 g/mol) at the cathode of an electrolytic cell, if a current of 15.9 A is passed through an aqueous solution of CuSOa? 19.4 min 32.2 min 24.0 min 33.9 min 26.8 min

7. Fig. 7.1 shows a simplified diagram of the electrolysis of sodium chloride solution, used to produce chlorine in industry. concentrated sodium chloride solution anode cathode gas 111 chlorine gas permeable membrane hydrogen Fig. 7.1 The balanced equation for the overall chemical change that occurs in the process shown in Fig. 7.1 is 2NaCl + 2H₂O → 2NaOH + Cl₂ + H₂ a. Show that the relative formula mass of sodium chloride is 58.5 sodium hydroxide solution b. Calculate the number of moles in 234g of sodium chloride. Show your working. Number of moles= Volume= c. Calculate the volume of chlorine molecules produced at room temperature and pressure, when 234g of sodium chloride are electrolysed. (1 mole of chlorine molecules has a volume of 24 dm³ at room temperature and pressure). Show your working

You are a bioengineer designing a new type of pacemaker. Which type of Galvanic cell would be best for you to use in this new device?