Concept explainers
(a)
Interpretation:
Whether
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:
Whether
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:
Whether
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.
(d)
Interpretation:
Whether
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.
(e)
Interpretation:
Whether
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.
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EP BASIC CHEMISTRY-STANDALONE ACCESS
- (7.12) A technician plates a faucet with 0.86 g Cr metal by electrolysis of aqueous Cr2(SO4)3. If 12.5 min is allowed for the plating, what current is needed? Molar mass of Cr: 51.996 g/mol Analysis/Strategy: mass of Cr ® mol Cr mol e¯ (or Faraday) ® coulombs ® amperes Reduction half-reaction of chromium solution to chromium metal: Cr* ,+3, (aq) e¯ ® Cr(s) + chromium solution, Cr2(SO4)3, has the ions: [Cr*3 s04-²] Answer: The current needed is ampere. (2 sig fig)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_forward(7.8) A voltaic cell is based on Co*2/Co half- cell and a AgCl/Ag half-cell. a) What reaction occurs at the anode? b) What is the standard cell potential, E°cell ? (a) Choices: The reaction that occurs at the anode: (A) Co*2(aq) + 2e¯ ® Co(s) (B) Co(s) ® Co²(aq) +2, + 2e- (C) Ag*(aq) + e¯ ® Ag(s) (D) Ag(s) ® Ag* (aq) + e¯ Answer: The reaction that occurs at the anode is (CAPITAL LETTER only). b) What is the standard cell potential, E°cell ? Choices: (A) +0.52 V (C) -0.52 V (B) -1.08 V (D) +1.08 V Answer: The standard cell potential of the cell, E°cell = V. Refer to the Table of Standard Reduction Potential below. STANDARD REDUCTION POTENTIAL AT 25 °C Retie Hall eaction Ag'ay+e Agls) Agle) Ag) + r"(ag) AgCs) +- Ag) 0.0 2 H0)+ 2e Hl)+ 20H Tng 0.10 HO, (a) + HAXn + 2e 3OH(a) +0.22 HO) + 2H() + 2e-2H0 -0. Hea 2 2 Ha 0.45ag (a) + te He"( AgCN, (a+ r- Ag) + 2CN (a) Ag:CrO) 2e 2Ag) Co/ Aglis - Ag +F) +0.79 AgSOl - Ag) + 25,0 (ag) A la+ 3e - AA als) + 2e 2(a) +1.20 Ha ag + 2() + 2- HO + H,0)…arrow_forward
- (7.3) Write the half-cell reactions for each of the following cells. Choose from the given options the BEST answer. Write the CAPITAL LETTER of your cholce. (a) Ag I Ag* a H* I Hz 1 Pt Answer: Half-cell reactions: (A) ) & () (B) ) & (iv) (C) (i) & () (D) (i) & (iv) O Agʻ(aq) o Agts) + e Ci) Agts) Ag'laq) + Clii) 2 H"(aq, IM) 2e" - Hzg 1 atm) (iv) Hag 1 atm) - 2 H'taq, IM) * 2e I Brzn PE Answer: Hall-cell reactions: (w W& Cii) (B) (im & (i) (C) (1) & (iv) & (iv) (D) (i) Crz0, ng • 14 H'cag) *• 6e Ge 2 Cr*tag) + 7 H,0D (ii) 2 Br 2e O Brzn (iv) Brzo 2 Br+ 2earrow_forward15. 5. For the following combustion reactions, identify the species that is oxidized, the species that is reduced, the oxidizing agent, and the reducing agent. [5.49] a. 2 C₂H₂ + 5 O₂ - 4 CO₂ + 2 H₂O b. 2 C.Ho+13 O; → 8 CO, + 10 HẸOarrow_forward(5.9: Similar to For Practice 5.15) Identify the oxidizing agent in the reaction below. Mg(s) + 2HCl(aq) --> MgCl2(aq) + H2(g) O Mg O H₂ OHCI This is not a redox reaction. < Previousarrow_forward
- (7.2b) Complete and balance the following by ion-electron method. Reactions are taking place in alkaline solution. b) Cr(OH)a) + CIO (aq) - Cro, (aq) + Clug Analysis: Balancing under acidic condition first (adding H30 & H*) Oxidation-Half reation: Balancing atoms & charges: Cr(OH)) * H20 - Cro, ug) + Reduction-Half reation: Balancing atoms and charges: e Clap H20 Balancing electrons lost & galned Multiply oxidation-half reaction by e's Multiply reduction-half reaction by e's Final balanced equation: Continue next page.arrow_forwardAssign oxidation numbers to each element in the following compoundsarrow_forward(7.1b) Complete and balance the following by ion-electron method. Reactions are taking place in acidic solution. b) Mn*2(aq) + BiO3 (aq) Bi* (aq) + Mn04 (aq) Analysis: Oxidation-Half reation: Balancing atoms & charges: Mn*2(aq) Mn04 (aq) H20 - + H* + e Reduction-Half reation: Balancing atoms and charges: BiO3 (aq) H* + Bi* (aq) e H20 Balancing electrons lost & gained Multiply oxidation-half reaction by e's Multiply reduction-half reaction by es Final balanced equation: Continue nextarrow_forward
- (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(7.2b) Complete and balance the following by ion-electron method. Reactions are taking place in alkaline solution. b) Cr(OH)a) + CIO (nq) - Cro, (aq) Analysis: Balancing under acidic condition first (adding H30 & H") Oxidation-Half reation: Balancing atoms & charges: Cr(OH)x) * H20 - Cro, ug * H' + Reduction-Half reation: Balancing atoms and charges: 10 taq H20 Balancing electrons lost & gained Multiply oxidation-half reaction by Multiply reduction-half reaction by e's Final balanced equation: Continue next page.arrow_forwardFill in the blanks: (7.13) Using a current of 4.75 A, how many minutes does it take to plate a sculpture with 1.50 g of Cu from a CuS04 solution? (Cu 63.546 g/mol) Analysis/Strategy: mass of Cu ® mol Cu ® mol e" (or Faraday) ® coulombs ® time in minutes (given current in amperes) Reduction half-reaction of copper solution to copper metal: Cu*2(aq) · + e¯ ® Cu(s) copper solution, CUSO4, has the ions: [Cu*2_SOq] Answer: The time needed to plate out a sculpture is minutes. (3 sig fig)arrow_forward
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