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Introductory Chemistry Plus Mastering Chemistry with Pearson eText -- Access Card Package (6th Edition) (New Chemistry Titles from Niva Tro)
- A voltaic cell is constructed using the reaction of chromium metal and iron(II) ions. 2 Cr(s) + 3 Fe2+(aq) 2 Cr3+(aq) + 3 Fe(s) Complete the following sentences: Electrons in the external circuit flow from the ________ electrode to the ______ electrode. Negative ions move in the salt bridge from the ________ half-cell to the ______ half-cell. The half-reaction at the anode is _______ and that at the cathode is ________.arrow_forwardYou have 1.0 M solutions of Al(NO3)3 and AgNO3 along with Al and Ag electrodes to construct a voltaic cell. The salt bridge contains a saturated solution of KCl. Complete the picture associated with this problem by a writing the symbols of the elements and ions in the appropriate areas (both solutions and electrodes). b identifying the anode and cathode. c indicating the direction of electron flow through the external circuit. d indicating the cell potential (assume standard conditions, with no current flowing). e writing the appropriate half-reaction under each of the containers. f indicating the direction of ion flow in the salt bridge. g identifying the species undergoing oxidation and reduction. h writing the balanced overall reaction for the cell.arrow_forwardConsider an electrochemical cell based on the half-reactions Ni2+(aq) + 2 e Ni(s) and Cd2+(aq) + 2e Cd(s). (a) Diagram the cell, and label each of the components (including the anode, cathode, and salt bridge). (b) Use the equations for the half-reactions to write a balanced, net ionic equation for the overall cell reaction. (c) What is the polarity of each electrode? (d) What is the value of Ecell? (e) In which direction do electrons flow in the external circuit? (f) Assume that a salt bridge containing NaNO3 connects the two half-cells. In which direction do the Na+(aq) ions move? In which direction do the NO3 (aq) ions move? (g) Calculate the equilibrium constant for the reaction. (h) If the concentration of Cd2+ is reduced to 0.010 M and [Ni2+] = 1.0 M, what is the value of Ecell? Is the net reaction still the reaction given in part (b)? (i) If 0.050 A is drawn from the battery, how long can it last if you begin with 1.0 L of each of the solutions and each was initially 1.0 M in dissolved species? Each electrode weighs 50.0 g in the beginning.arrow_forward
- One half-cell in a voltaic cell is constructed from a silver wire electrode in a AgNO3 solution of unknown concentration. The other half-cell consists of a zinc electrode in a 1.0 M solution of Zn(NO3)2. A potential of 1.48 V is measured for this cell. Use this information to calculate the concentration of Ag+(aq).arrow_forwardConsider a cell based on the following half-reactions: a. Draw this cell under standard conditions, labeling the anode, the cathode, the direction of electron flow, and the concentrations, as appropriate. b. When enough NaCl(s) is added to the compartment containing gold to make the [Cl] = 0.10 M, the cell potential is observed to be 0.31 V. Assume that Au3+ is reduced and assume that the reaction in the compartment containing gold is Au3+(aq)+4Cl(aq)AuCl4(aq) Calculate the value of K for this reaction at 25C.arrow_forwardThe zinc copper voltaic cell shown with this problem is currently running under standard conditions. How would the intensity of light from the bulb change if you were to a dissolve some additional CuSO4(s) in the CuSO4 solution? b dissolve some additional Zn(NO3)2(s) in the Zn(NO3)2 solution? c add H2O to the CuSO4 solution? d remove the salt bridge?arrow_forward
- Calculate the potential developed by a voltaic cell using the following reaction if all dissolved species are 0.015 M. 2 Fe2+(aq) + H2O2(aq) + 2 H+(aq) 2 Fe3+(aq) + 2 H2O()arrow_forwardA voltaic cell is constructed from the following half-cells: a chromium electrode in chromium(III) sulfate solution and a lead electrode in lead(II) sulfate solution. The half-reactions are Cr(s)Cr3(aq)+3ePb2+(aq)+2ePb(s) Sketch the cell, labeling the anode and cathode (and the electrode reactions), and show the direction of electron flow and the movement of cations.arrow_forwardIn principle, a battery could be made from aluminum metal and chlorine gas. (a) Write a balanced equation for the reaction thatwould occur in a battery using Al3+(aq) | Al(s) andCl2(g) | Cl(aq) half-cells. (b) Identify the half-reaction at the anode and at the cathode. Do electrons flow from the Al electrode when thecell does work? Explain. (c) Calculate the standard potential, Ecell, for the battery.arrow_forward
- For each of the following electrochemical cells, write equations for lire oxidation and reduction half-reactions and for the overall reaction (a) Pb(s)|Pb2+(aq)||Sn4+(aq),Sn2+(aq)|C(s) (b) Hg()|Hg2Cl2(s)|Cl(aq)||Ag+(aq)|Ag(s)arrow_forwardFrom the information provided, use cell notation to describe the following systems: (a) In one half-cell, a solution of Pt(NO3)2 forms Pt metal, while in the other half-Cell, Cu metal goes into a.Cu(NO3)2 solution with all solute concentrations 1 M. (b) The cathode consists of a gold electrode in a 0.55 M Au(NO3)3 solution and the anode is a magnesium electrode in 0.75 M Mg(NO3)2 solution. (c) One half-cell consists of a silver electrode in a 1 M AgNO3 solution, and in the other half-cell, a copper Electrode in 1 M Cu(NO3)2 is oxidized.arrow_forward
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