(a)
Interpretation:
An anode in the given voltaic cell should be determined.
Concept Introduction :
A redox reaction is meant to take place when the oxidation states of the atoms present in a chemical species are changed.
Electrical energy can be generated through spontaneous
When these half cells containing the strip of the metal and the metal ion solution are placed in separate beakers, flow of electrons takes place from one half cell to other and these two half cells are connected by a salt bridge. The strip of the metal in each of these half cells is known as electrode and this strip is in contact with the metal ion solution.
Oxidation takes place at the electrode known as anode whereas reduction reaction takes place at cathode. Oxidation means loss of electrons while reduction means gain of electrons. Direction of a spontaneous redox reaction is determined with the help of activity series in which the metals which lose electrons easily are placed at the top and the metals that are unable to lose electrons easily are placed at bottom of the series.
(b)
Interpretation:
A cathode in the given voltaic cell should be determined.
Concept Introduction :
A redox reaction is meant to take place when the oxidation states of the atoms present in a chemical species are changed.
Electrical energy can be generated through spontaneous oxidation-reduction reaction by making use of apparatus known as voltaic cell. It contains two half cells, at one of the half cell oxidation takes place and at other half cell reduction takes place.
When these half cells containing the strip of the metal and the metal ion solution are placed in separate beakers, flow of electrons takes place from one half cell to other and these two half cells are connected by a salt bridge. The strip of the metal in each of these half cells is known as electrode and this strip is in contact with the metal ion solution.
Oxidation takes place at the electrode known as anode whereas reduction reaction takes place at cathode. Oxidation means loss of electrons while reduction means gain of electrons. Direction of a spontaneous redox reaction is determined with the help of activity series in which the metals which lose electrons easily are placed at the top and the metals that are unable to lose electrons easily are placed at bottom of the series.
(c)
Interpretation:
The half cell reaction at anode should be written.
Concept Introduction :
A redox reaction is meant to take place when the oxidation states of the atoms present in a chemical species are changed.
Electrical energy can be generated through spontaneous oxidation-reduction reaction by making use of apparatus known as voltaic cell. It contains two half cells, at one of the half cell oxidation takes place and at other half cell reduction takes place.
When these half cells containing the strip of the metal and the metal ion solution are placed in separate beakers, flow of electrons takes place from one half cell to other and these two half cells are connected by a salt bridge. The strip of the metal in each of these half cells is known as electrode and this strip is in contact with the metal ion solution.
Oxidation takes place at the electrode known as anode whereas reduction reaction takes place at cathode. Oxidation means loss of electrons while reduction means gain of electrons. Direction of a spontaneous redox reaction is determined with the help of activity series in which the metals which lose electrons easily are placed at the top and the metals that are unable to lose electrons easily are placed at bottom of the series. Half cell reaction is a component of a given redox reaction. It is either the oxidation or reduction component of the given redox reaction.
(d)
Interpretation:
The half cell reaction at cathode should be written.
Concept Introduction :
A redox reaction is meant to take place when the oxidation states of the atoms present in a chemical species are changed.
Electrical energy can be generated through spontaneous oxidation-reduction reaction by making use of apparatus known as voltaic cell. It contains two half cells, at one of the half cell oxidation takes place and at other half cell reduction takes place.
When these half cells containing the strip of the metal and the metal ion solution are placed in separate beakers, flow of electrons takes place from one half cell to other and these two half cells are connected by a salt bridge. The strip of the metal in each of these half cells is known as electrode and this strip is in contact with the metal ion solution.
Oxidation takes place at the electrode known as anode whereas reduction reaction takes place at cathode. Oxidation means loss of electrons while reduction means gain of electrons. Direction of a spontaneous redox reaction is determined with the help of activity series in which the metals which lose electrons easily are placed at the top and the metals that are unable to lose electrons easily are placed at bottom of the series. Half cell reaction is a component of a redox reaction. It is either the oxidation or reduction component of the given redox reaction.
(e)
Interpretation:
The overall cell reaction should be written.
Concept Introduction :
A redox reaction is meant to take place when the oxidation states of the atoms present in a chemical species are changed.
Electrical energy can be generated through spontaneous oxidation-reduction reaction by making use of apparatus known as voltaic cell. It contains two half cells, at one of the half cell oxidation takes place and at other half cell reduction takes place.
When these half cells containing the strip of the metal and the metal ion solution are placed in separate beakers, flow of electrons takes place from one half cell to other and these two half cells are connected by a salt bridge. The strip of the metal in each of these half cells is known as electrode and this strip is in contact with the metal ion solution.
Oxidation takes place at the electrode known as anode whereas reduction reaction takes place at cathode. Oxidation means loss of electrons while reduction means gain of electrons. Direction of a spontaneous redox reaction is determined with the help of activity series in which the metals which lose electrons easily are placed at the top and the metals that are unable to lose electrons easily are placed at bottom of the series.
(f)
Interpretation:
The shorthand cell notation should be written.
Concept Introduction :
A redox reaction is meant to take place when the oxidation states of the atoms present in a chemical species are changed. Electrical energy can be generated through spontaneous oxidation-reduction reaction by making use of apparatus known as voltaic cell. It contains two half cells, at one of the half cell oxidation takes place and at other half cell reduction takes place cell notation is the shorthand method writing a given
Want to see the full answer?
Check out a sample textbook solutionChapter 15 Solutions
Basic Chemistry
- (7.9) Using potentials listed in the Table, the standard reduction determine whether the following reaction is spontaneous under standard conditions. Support your answer. Hg*2(aq) + 21¯(aq) → ,+2, Hga) +I2(s) From the Table: Hg*2(aq) + 2e¯ → Hga) E°red = +0.85 V I2(s) + 2e- - 21 (aq) E°red = +0.54 V Answer: Is the above reaction spontaneous? (YES or NO) Briefly support your answer (. Refer to the Table of Standard Reduction Potential below. STANDARD REDUCTION POTENTIAL AT 25 °C ETV) atteaction +0.50 2H,O + 2e-Hlg) + 20H (a Hait-Reaction (V) Ag (ag) +- Agis) Aglle(s)+- Ag)+ r (a) AgCIs) - Ag(s) -a(ap) Ag(CN), (a) eAgs)+ 2CN (a) -O83 Agi+ r(a) 0.10 HO, (a) + HO) + 2e 3OH (a) +0.22 HOa) + 2H(ag) 2e 2Ho) -0.31 He(a 2e 2 Hg) +0.45 2Hg"(a)+ 2e Hg () -0.15 He(a)+ 2e Hel) ) + 2e 21(a) -1.46 2 10, (a) + 12H(a) + 10e l) +6HO) +0.56K'(ag) K) +1.78 a79 AgCro,(s) + 2e 2 Ags) + Cro ) Agl(s) +e- Ag) (a) AgrS,0(a) + - Agis) + 25,0 (a) A" (a) + 3e - A) 92 054 1.20 HAs0,n- 2H"(a) + 2e HAOa) + H,o)…arrow_forward(7.7) A voltaic cell based on the half- reactions: In (aq) – In*3(ag) + 2e™ (aq) Br2() +2e¯→ 2Br¯(ag) The standard emf for this cell is +1.46 V. Using the data below, calculate, E'red for the reduction of In*3 to In*1. Br2() + 2e¯ → 2B1¯(ag) (cathode) E red(cathode) = E %3D Br(aq) = +1.06 V (See Table below) Choices: (A) +0.40 V (B) -0.40 V (C) + 2.50 V (D) -2.50 V Answer: E'red for the reduction of In+3 = to In*1 (in volts) STANDARD REDUCTION POTENTIALS at 25°C; Reduction Half Reaction F: (g) + 2e → 2F (aq) HO, (aq) + 2H" (aq) + 2e 2H;0 PbO(3) +4H" (ag) + So (ag) + 2e PbSO(s) + HO MnO. (aq) + 8H" (aq)+ Se+ Ma" (ag) + 4H,o Au" (aq) + 3e Au (s) Ch (g) + 2e 2C (ag) CrO (aq) + 14H" (aq) + 6e →2Cr" (aq) + TH:O MnO: (3) i 4H" (aq) 2e Ma (aq) 2H:0 O: (g) + 4H" (aq) + 4e + 2H:0 Br: () +2e + 2Br (ag) NO, (aq) + 4I" (aq) + 3e + NO (g) + 2H:0 2Hg (aq) + 2e Hg" (aq) Hgr" (aq) + 2e→ 2Hg () Ag (aq) +e Ag (s) Fe (aq) + e Fe (aq) O: (g) - 21 (aq) + 2e HO: (ag) E MnO" (aq) + 2H0 + 3e MnO: (3) + 40H…arrow_forward(7.11) A voltaic cell is constructed that uses the following reaction and operates at 298 K: Zn(s) + Cd+2, Cd*2(aq) ® + (S)uZ Zn*2(aq) + Cd(s) a) What is the emf of the cell under standard conditions? Zn*2 (ag) + 2e¯ ® Zn(s) E°cell = -0.76 V cd*2 (aq) + 2e¯ ® Cd(s) E°cell = -0.40 V Answer: The emf of the cell is V. Refer to the Table of Standard Reduction Potential below to solve Question (a). STANDARD REDUCTION POTENTIAL AT 25 °c E() Hall Reaction +0.N0 2 H,O) + ze Hg) + 2OH (a) Hal-Reaction Hall-Reaction E(V) Ag"(ng) +e- Ag(s) --0.83 Aglir(s) +e- Ag(s) + Br (ag) AgCKs) +e- Ag(s) + a"(a) Ag(CN), "(a) +e Ag(s)+ 2CN (a) Ag:Cro(s) + 2e 2 Ag(s) + Cro (ag) +0.10 HO, (a) + H,O) + 2e 3OH (ay) +0.22 H,O(ng) + 2H"(ag) + 2e 2 H;O() -0.31 Hg/ (a) + 2e 2 Hg() +0.45 2g"(ay) + 2e 1Hg (a) -0.15 Hg" (a) + 2e - Hg() +0.01 s) + 2e 21(a) +1.78 +0.79 +0.92 Agl(s) +e- Ag(s) +I(ay) +0.85 Ag(S0,) (ay) +e Ag(s) + 2 S,0 (ap) +0.54 A (ay) + 3e Al(s) HAso,(a) + 2H'(ay) + 2e - HAsOdany) + HO() Ba"(ag) + 2e -…arrow_forward
- (7.4) Describe in shorthand notation a galvanic cell for which the cell has the following reaction. Chose the BEST option by writing the CAPITAL LETTER of the best answer. Cu(s) + 2 Fe*3(aq) - Cu*?(aq) + 2 (be). Fe2 (aq) CHOICES: (A) Cu Cu*2||Fe*3|Fe*2 (B) Cu*2|Cu||Fe*3| Fe*2 (C) Cu|Cu*2||Fe*2 |Fe*3 (C) Cu*2|Cu||Fe*2| Fe*3 Answer:arrow_forwardQuestion 1.4 1.4 A metal cube has a total surface area of 690 cm2 and is to be gold-plated to a thickness of 0,5 cm. The process needs to be completed in exactly 2 hours. The electrochemical equivalent of gold is 1,118 mg/C and the density of gold is 19300 kg/m3. 1.4.1) Calculate the current required for the platingarrow_forwardComplete and balance the following redox reaction in basic solution Zn(s) → Zn(OH),*(aq) + H,(g) 4 4- 2- D2+ 3+ 4+ + 1 2 3 4 6. 7 8 9. O3 O6 O7 (s) (1) (g) (aq) + e Zn H* OH Reset • x H,0 Delete 9. 4. 3. 2.arrow_forward
- Question 10 of 25 Complete and balance the following redox reaction in acidic solution NO2(g) → NO3 (aq) + NO(g) 04- O+ 2+ 3+ O4+ 1 4 6. 7 9. O2 3 4 O5 O6 07 O8 O9 (s) (1) (g) (aq) H e N H* OH H2O H30* Reset x H2O Delete MacBook Pro 80 000 DII DD F2 F3 F4 F5 F6 F7 F8 F9 F10 %23 %24 3 5 3. 2.arrow_forwardLabeling an Electrolytic Cell The diagram below represents the electrolysis of a sodium chloride solution (brine). Match each numbered item in the diagram with the letter of the correct label from the list below. sodium ion cathode positive terminal battery chlorine gas 1. electrolyte hydrogen gas chloride ion anode negative terminal -2. 3. 4. direction of electron flow 5. 6.- 7. 69. 8. 5. 10. 9. 6. 10. 8. 11. a. Write the equation for the half-reaction that occurs at the cathode. b. Is this an example of oxidation or of reduction? 2. a. Write the equation for the half-reaction that occurs at the anode. b. Is this an example of oxidation or of reduction? 3. Write the overall ionic equation.. 4. Write the overall molecular equation.arrow_forward(7: 4 pts) Balance the following redox reaction in basic conditions. Show your work for partial credit.arrow_forward
- For each of the reaction below, identify: (0.5 marks each) substance being oxidized substance being reduced oxidizing agent reducing agent number of electrons transferred. 1. K2Cr207 + 14HCI -> 2KCI + 2CrCl + 3Cl + 7H20 2. 10 OH +4C12 + S2032 > 5H20 + 2502 + 8 CIarrow_forwardConsider an electrochemical cell with a copper metal electrode immersed in a solution of Cu2+ ions of unknown concentration, connected via a salt bridge to a 0.100 M Ce solution and a platinum electrode over which pure chlorine gas at 1 atmosphere is bubbled. 1.1 Write the complete shorthand notation for this cell. 1. 1.2 Determine the concentration of Cu2+ ions required, if the cell potential is to be 1.122 V under these conditions at 298.15K.arrow_forwardGiven the following redox pair, identify the reducing agent: NAD+/ NADH (-0.32) 2e- 202H2O (0.82) 2e- A. NADH B. NAD+ C. O₂ D. H₂Oarrow_forward
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistryChemistryISBN:9781259911156Author:Raymond Chang Dr., Jason Overby ProfessorPublisher:McGraw-Hill EducationPrinciples of Instrumental AnalysisChemistryISBN:9781305577213Author:Douglas A. Skoog, F. James Holler, Stanley R. CrouchPublisher:Cengage Learning
- Organic ChemistryChemistryISBN:9780078021558Author:Janice Gorzynski Smith Dr.Publisher:McGraw-Hill EducationChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningElementary Principles of Chemical Processes, Bind...ChemistryISBN:9781118431221Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. BullardPublisher:WILEY