Multiple ChoiceGiven the following standard reduction potentials,Hg22+(aq) + 2 e– 2 Hg (l) E° = +0.789 V Hg2Cl2(s) + 2 e– 2 Hg (l) + 2 Cl-(aq) E° = +0.271 Vdetermine Ksp for Hg2Cl2(s) at 25 °C.793views1rank9comments
Multiple ChoiceDetermine the standard cell potential for the following cell: Ni (s)│Ni2+ (aq) ║Cu2+ (aq)│Cu (s) cell.356views
Multiple ChoiceWhich of the following correctly describes the products of the electrolysis of an aqueous solution of KI?249views
Open QuestionFor the redox reaction label: the anode, cathode, half-reactions occurring at each half-cell, direction of electron flow, and direction of neutral ions flow.Ni(s)+Zn2+(aq)→Ni2+(aq)+Zn(s)Ni\left(s\right)+Zn^{2+}\left(aq\right)\rightarrow Ni^{2+}\left(aq\right)+Zn\left(s\right)Ni(s)+Zn2+(aq)→Ni2+(aq)+Zn(s)331views
Textbook QuestionThe diagram that follows represents a molecular view of a process occurring at an electrode in a voltaic cell. (b) Is the electrode the anode or cathode? 350views
Textbook QuestionThe diagram that follows represents a molecular view of a process occurring at an electrode in a voltaic cell. (a) Does the process represent oxidation or reduction?627views
Textbook QuestionAssume that you want to construct a voltaic cell that uses the following half-reactions: A2+1aq2 + 2 e- ¡ A1s2 Ered ° = -0.10 V B2+1aq2 + 2 e- ¡ B1s2 E°red = -1.10 V You begin with the incomplete cell pictured here in which the electrodes are immersed in water. (a) What additions must you make to the cell for it to generate a standard emf?651views
Textbook QuestionThe electrodes in a silver oxide battery are silver oxide 1Ag2O2 and zinc (b) Which battery do you think has an energy density most similar to the silver oxide battery: a Li-ion battery, a nickel– cadmium battery, or a lead–acid battery? [Section 20.7]425views
Textbook QuestionIndicate whether each statement is true or false: (c) A salt bridge or permeable barrier is necessary to allow a voltaic cell to operate.341views
Textbook QuestionA voltaic cell similar to that shown in Figure 20.5 is constructed. One electrode half-cell consists of a silver strip placed in a solution of AgNO3, and the other has an iron strip placed in a solution of FeCl2. The overall cell reaction is Fe1s2 + 2 Ag+1aq2 ¡ Fe2+1aq2 + 2 Ag1s2 (f) In which directions do the cations and anions migrate through the solution?726views
Textbook Question(b) Write the half-reaction that occurs at a hydrogen electrode in acidic aqueous solution when it serves as the anode of a voltaic cell.374views
Textbook Question(c) Why is it impossible to measure the standard reduction potential of a single half-reaction?340views
Textbook QuestionA voltaic cell that uses the reaction PdCl42-1aq2 + Cd1s2 ¡ Pd1s2 + 4 Cl-1aq2 + Cd2+1aq2 has a measured standard cell potential of +1.03 V. (a) Write the two half-cell reactions.470views
Textbook QuestionA voltaic cell consists of a strip of cadmium metal in a solution of Cd1NO322 in one beaker, and in the other beaker a platinum electrode is immersed in a NaCl solution, with Cl2 gas bubbled around the electrode. A salt bridge connects the two beakers. (c) Write the equation for the overall cell reaction.1147views
Textbook QuestionSketch a voltaic cell for each redox reaction. Label the anode and cathode and indicate the half-reaction that occurs at each electrode and the species present in each solution. Also indicate the direction of electron flow. a. Ni2+(aq) + Mg(s) ¡ Ni(s) + Mg2+(aq)2306views1rank
Textbook QuestionConsider the voltaic cell: d. Indicate the direction of anion and cation flow in the salt bridge858views
Textbook QuestionWhy is the cathode of a galvanic cell considered to be the positive electrode?439views
Textbook QuestionDescribe galvanic cells that use the following reactions. In each case, write the anode and cathode half-reactions and sketch the experimental setup. Label the anode and cathode, identify the sign of each electrode, and indicate the direction of electron and ion flow. (b) 554views
Textbook QuestionDescribe galvanic cells that use the following reactions. In each case, write the anode and cathode half-reactions and sketch the experimental setup. Label the anode and cathode, identify the sign of each electrode, and indicate the direction of electron and ion flow. (b) 467views
Textbook QuestionDetermine whether or not each metal dissolves in 1 M HCl. For those metals that do dissolve, write a balanced redox reaction showing what happens when the metal dissolves. a. Al3504views6rank
Textbook QuestionDetermine whether or not each metal dissolves in 1 M HNO3. For those metals that do dissolve, write a balanced redox reaction showing what happens when the metal dissolves. a. Cu1256views1rank
Textbook QuestionDetermine whether or not each metal dissolves in 1 M HIO3. For those metals that do dissolve, write a balanced redox equation for the reaction that occurs. a. Au1241views
Textbook QuestionAn H2/H+ half-cell (anode) and an Ag+/Ag half cell (cathode) are connected by a wire and a salt bridge. (b) Write balanced equations for the electrode and overall cell reactions.1268views
Textbook QuestionWhat conditions must be met for a cell potential E to qualify as a standard cell potential E°?404views
Textbook QuestionHeart pacemakers are often powered by lithium–silver chromate 'button' batteries. The overall cell reaction is 2 Li1s2 + Ag2CrO41s2 ¡ Li2CrO41s2 + 2 Ag1s2 (a) Lithium metal is the reactant at one of the electrodes of the battery. Is it the anode or the cathode?431views
Textbook QuestionIn some applications nickel–cadmium batteries have been replaced by nickel–zinc batteries. The overall cell reaction for this relatively new battery is: 2 H2O1l2 + 2 NiO1OH21s2 + Zn1s2 ¡ 2 Ni1OH221s2 + Zn1OH221s2 (b)What is the anode half-reaction?613views
Textbook QuestionMake a sketch of a concentration cell employing two Zn/Zn2+ half-cells. The concentration of Zn2+ in one of the half-cells is 2.0 M and the concentration in the other half-cell is 1.0x10^-3 M. Label the anode and the cathode and indicate the half-reaction occuring at each electrode. Also indicate the direction of electron flow.975views
Textbook QuestionConsider the concentration cell: b. Indicate the direction of electron flow.665views
Textbook QuestionConsider the concentration cell: c. Indicate what happens to the concentration of Pb2+ in each half-cell.591views
Textbook Question(d) Lithium is not nearly as abundant as sodium. If sodium ion batteries were developed that function in the same manner as lithium ion batteries, do you think 'sodium cobalt oxide' would still work as the electrode material? Explain.499views
Textbook Question(c) Will the lithium cobalt oxide cathode expand or contract as lithium ions are inserted?527views
Textbook QuestionA friend wants you to invest in a new battery she has designed that produces 24 V in a single voltaic cell. Why should you be wary of investing in such a battery?290views
Textbook QuestionWrite a balanced equation for the overall cell reaction when a lead storage battery is being charged. Refer to Section 19.10. 232views
Textbook QuestionA storm has knocked out power to your beach house, and you would like to build a battery from household items to charge your iPhone. You have the following materials. alum in the kitchen, which can be used to make a 1.0 M Al3+ solution bleach, which is a solution that is approximately a 1.0 M in ClO-aluminum foil, a platinum necklace and bologna, which can be used as a salt bridge (a) What are the half reactions and overall reaction in the battery?198views
Textbook QuestionThe half-reactions that occur in ordinary alkaline batteries can be written as In 1999, researchers in Israel reported a new type of alkaline battery, called a 'super-iron' battery. This battery uses the same anode reaction as an ordinary alkaline battery but involves the reduction of FeO42- ion (from K2FeO4) to solid Fe(OH)3 at the cathode. (b) Write a balanced equation for the cathode half-reaction in a super-iron battery. The half-reaction occurs in a basic environment.475views
Open QuestionWhat is the reduction half-reaction for the following overall galvanic cell reaction? Co2+(aq) + 2 Ag(s) → Co(s) + 2 Ag+(aq)95views
Open QuestionWhat balances charges that may build up as reduction and oxidation occur in a voltaic cell94views