11:27The Nernst equation | Applications of thermodynamics | AP Chemistry | Khan AcademyKhan Academy450views
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11:30Using the Nernst equation | Redox reactions and electrochemistry | Chemistry | Khan AcademyKhan Academy Organic Chemistry380views
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Multiple ChoiceIf [Br–] = 0.010 M and [Al3+] = 0.022 M, predict whether the following reaction would proceed spontaneously as written at 25ºC:Al (s) + Br2 (l) ⇌ Al3+ (aq) + Br– (aq)Standard Reduction PotentialsAl3+ (aq) + 3 e– → Al (s) E°red = –1.66 VBr2 (l) + 2 e– → Br– (aq) E°red = +1.09 V135views3rankHas a video solution.
Multiple ChoiceDetermine [Fe2+] for the following galvanic cell at 25ºC if given [Sn2+] = 0.072 M, [Fe3+] = 0.0219 M, and [Sn4+] = 0.00345 M. Sn2+ (aq) + 2 Fe3+ (aq) ⇌. Sn4+ (aq) + 2 Fe2+ (aq) Ecell = + 0.68 VStandard Reduction PotentialsSn4+ (aq) + 2 e– →. Sn2+ (aq) E°red = + 0.151 VFe3+ (aq) + e– → Fe2+ (aq) E°red = + 0.771 V131views1commentsHas a video solution.
Textbook QuestionConsider the following voltaic cell: (c) What is the change in the cell voltage when the ion concentrations in the cathode half-cell are increased by a factor of 10?625viewsHas a video solution.
Textbook QuestionConsider a Daniell cell with 1.0 M ion concentrations: Does the cell voltage increase, decrease, or remain the same when each of the following changes is made? Explain. (a) Write a balanced equation for each cell reaction.842viewsHas a video solution.
Textbook QuestionA voltaic cell utilizes the following reaction: Al1s2 + 3 Ag+1aq2 ¡ Al3+1aq2 + 3 Ag1s2 What is the effect on the cell emf of each of the following changes? (a) Water is added to the anode half-cell, diluting the solution.727viewsHas a video solution.
Textbook QuestionA voltaic cell is constructed that uses the following reaction and operates at 298 K: Zn1s2 + Ni2+1aq2 ¡ Zn2+1aq2 + Ni1s2 (c) What is the emf of the cell when 3Ni2+4 = 0.200 M and 3Zn2+4 = 0.900 M?746viewsHas a video solution.
Textbook QuestionA voltaic cell utilizes the following reaction: 4 Fe2+1aq2 + O21g2 + 4 H+1aq2 ¡ 4 Fe3+1aq2 + 2 H2O1l2 (b) What is the emf of this cell when 3Fe2+4 = 1.3 M, 3Fe3+4= 0.010 M, PO2 = 0.50 atm, and the pH of the solution in the cathode half-cell is 3.50?659viewsHas a video solution.
Textbook QuestionA voltaic cell utilizes the following reaction: (b) What is the emf for this cell when 3Fe3+4 = 3.50 M, PH2= 0.95 atm, 3Fe2+4 = 0.0010 M, and the pH in both half-cells is 4.00?913views1rank1commentsHas a video solution.
Textbook QuestionA voltaic cell is constructed that is based on the following reaction: Sn2+1aq2 + Pb1s2 ¡ Sn1s2 + Pb2+1aq2 (a) If the concentration of Sn2+ in the cathode half-cell is 1.00 M and the cell generates an emf of +0.22 V, what is the concentration of Pb2+ in the anode half-cell?829viewsHas a video solution.
Textbook QuestionA voltaic cell employs the following redox reaction: Sn2+(aq) + Mn(s) ¡ Sn(s) + Mn2+(aq) Calculate the cell potential at 25 °C under each set of conditions. c. [Sn2+] = 2.00 M; [Mn2+] = 0.0100 M3296views1rankHas a video solution.
Textbook QuestionAn electrochemical cell is based on these two half-reactions: Ox: Pb(s) -> Pb2+ (aq, 0.10 M) + 2 e- Red: MnO4-(aq, 1.50 M) + 4 H+(aq, 2.0 M) + 3 e- -> MnO2(s) + 2 H2O(l) Calculate the cell potential at 25 °C.3105viewsHas a video solution.
Textbook QuestionAn electrochemical cell is based on these two half-reactions: Ox: Sn(s) ¡ Sn2+(aq, 2.00 M) + 2 e- Red: ClO2(g, 0.100 atm) + e- ¡ ClO2-(aq, 2.00 M) Calculate the cell potential at 25 °C.2330viewsHas a video solution.
Textbook QuestionA voltaic cell consists of a Zn>Zn2+ half-cell and a Ni>Ni2+ half-cell at 25 °C. The initial concentrations of Ni2+ and Zn2+ are 1.50 M and 0.100 M, respectively. c. What are the concentrations of Ni2+ and Zn2+ when the cell potential falls to 0.45 V? Ec°ell for the fuel-cell breathalyzer, which employs the following1117viewsHas a video solution.
Textbook QuestionA voltaic cell consists of a Zn>Zn2+ half-cell and a Ni>Ni2+ half-cell at 25 °C. The initial concentrations of Ni2+ and Zn2+ are 1.50 M and 0.100 M, respectively. b. What is the cell potential when the concentration of Ni2+ has fallen to 0.500 M?2015viewsHas a video solution.
Textbook QuestionA voltaic cell consists of a Zn>Zn2+ half-cell and a Ni>Ni2+ half-cell at 25 °C. The initial concentrations of Ni2+ and Zn2+ are 1.50 M and 0.100 M, respectively. a. What is the initial cell potential?495viewsHas a video solution.
Textbook QuestionA voltaic cell consists of a Pb>Pb half-cell and a Cu>Cu half- cell at 25°C. The initial concentrations of Pb2+ and Cu2+ are 0.0500 M and 1.50 M, respectively. c. What are the concentrations of Pb2+ and Cu2+ when the cell potential falls to 0.35 V?720viewsHas a video solution.
Textbook QuestionA voltaic cell consists of a Pb>Pb half-cell and a Cu>Cu half- cell at 25°C. The initial concentrations of Pb2+ and Cu2+ are 0.0500 M and 1.50 M, respectively. b. What is the cell potential when the concentration of Cu2+ has fallen to 0.200 M?1429viewsHas a video solution.
Textbook QuestionA voltaic cell consists of a Pb>Pb half-cell and a Cu>Cu half- cell at 25°C. The initial concentrations of Pb2+ and Cu2+ are 0.0500 M and 1.50 M, respectively. a. What is the initial cell potential?613viewsHas a video solution.
Textbook QuestionA concentration cell consists of two Sn/Sn2+ half-cells. The cell has a potential of 0.10 V at 25°C. What is the ratio of the Sn2+ concentrations in the two half-cells?2228views2rankHas a video solution.
Textbook QuestionA Cu/Cu2+ concentration cell has a voltage of 0.22 V at 25 °C. The concentration of Cu2+ in one of the half-cells is 1.5x10^-3 M. What is the concentration of Cu2+ in the other half-cell? (Assume the concentration in the unknown cell is the lower of the two concentrations.)3631viewsHas a video solution.
Textbook QuestionConsider a galvanic cell that uses the reaction Calculate the potential at 25 °C for a cell that has the following ion concentrations: [Ag+] = 0.010M, [Ni2+] = 0.100M.1064viewsHas a video solution.
Textbook QuestionA galvanic cell has an iron electrode in contact with 0.10 M FeSO4 and a copper electrode in contact with a CuSO4 solu-tion. If the measured cell potential at 25 °C is 0.67 V, what is the concentration of Cu2+ in the CuSO4 solution?1191viewsHas a video solution.
Textbook QuestionThe Nernst equation applies to both cell reactions and half-reactions. For the conditions specified, calculate the potential for the following half-reactions at 25 °C. (b) 1141views1rankHas a video solution.
Textbook QuestionWhen suspected drunk drivers are tested with a Breathalyzer, the alcohol (ethanol) in the exhaled breath is oxidized to acetic acid with an acidic solution of potassium dichromate: The color of the solution changes because some of the orange Cr2O7 2-is converted to the green Cr3+ The Breath-alyzer measures the color change and produces a meter reading calibrated in blood alcohol content. (b) What is the value of E for the reaction when the concentrations of ethanol, acetic acid, Cr2O7 are 1.0 M and the pH is 4.00?819viewsHas a video solution.
Textbook QuestionA voltaic cell is constructed that uses the following half-cell reactions: Cu+1aq2 + e- ¡ Cu1s2 I21s2 + 2 e- ¡ 2 I-1aq2 The cell is operated at 298 K with 3Cu+4 = 0.25 M and 3I-4 = 0.035 M. (a) Determine E for the cell at these concentrations.2565views1rankHas a video solution.
Textbook QuestionAt one time on Earth, iron was present mostly as iron(II). Later, once plants had produced a significant quantity of oxygen in the atmosphere, the iron became oxidized to iron(III). Show that Fe2+(aq) can be spontaneously oxidized to Fe3+(aq) by O2(g) at 25°C assuming the following reasonable environmental conditions: 644viewsHas a video solution.
Textbook QuestionCopper reduces dilute nitric acid to nitric oxide (NO) but reduces concentrated nitric acid to nitrogen dioxide (NO2): Assuming that [Cu2+] = 0.10 M and that the partial pressures of NO and NO2 are 1.0 * 10-3 atm, calculate the potential (E) for reactions (1) and (2) at 25 °C and show which reaction has the greater thermodynamic tendency to occur when the concentration of HNO3 is (a) 1.0 M722viewsHas a video solution.
Textbook QuestionA battery relies on the oxidation of magnesium and the reduction of Cu2+. The initial concentrations of Mg2+ and Cu2+ are 1.0 * 10-4 M and 1.5 M, respectively, in 1.0-liter half-cells. a. What is the initial voltage of the battery?1345viewsHas a video solution.
Textbook QuestionA battery relies on the oxidation of magnesium and the reduction of Cu2+. The initial concentrations of Mg2+ and Cu2+ are 1.0 * 10-4 M and 1.5 M, respectively, in 1.0-liter half-cells. b. What is the voltage of the battery after delivering 5.0 A for 8.0 h?347views1rankHas a video solution.
Textbook QuestionA mercury battery uses the following electrode half-reactions: (c) What is the effect on the cell voltage of a tenfold change in the concentration of KOH in the electrolyte? Explain..349viewsHas a video solution.
Textbook QuestionHow does the pH of the solution affect the formation of rust?425viewsHas a video solution.
Textbook QuestionAn MnO2(s)/Mn2+(aq) electrode in which the pH si 10.24 is prepared. Find the [Mn2+] necessary to lower the potential of the half-cell to 0.00 V (at 25°C)769viewsHas a video solution.
Textbook QuestionTo what pH should you adjust a standard hydrogen electrode to get an electrode potential of -0.122 V? (Assume that the partial pressure of hydrogen gas remains at 1 atm.)580viewsHas a video solution.
Textbook QuestionA concentration cell has the same half-reactions at the anode and cathode, but a voltage results from different concentrations in the two electrode compartments. (b) A similar cell has 0.10 M Cu2+ in both compartments. When a stoichiometric amount of ethylenediamine (NH2CH2CH2NH2) is added to one compartment, the measured cell potential is 0.179 V. Calculate the formation constant Kf for the complex ion Cu(NH2CH2CH2CH2)22+. Assume there is no volume change.676viewsHas a video solution.
Textbook QuestionConsider the redox titration of 100.0 mL of a solution of 0.010 M Fe2+ in 1.50 M H2SO4 with a 0.010 M solution of KMnO4, yielding Fe3+ and Mn2+. The titration is carried out in an electrochemical cell equipped with a platinum electrode and a calomel reference electrode consisting of an Hg2Cl2/Hg electrode in contract with a saturated KCl solution having [Cl-] = 2.9M. Using any data in Appendixes C and D, calculate the cell potential after addition of (a) 5.0 mL, (b) 10.0mL, (c) 19.0 mL, and (d) 21.0 mL of the KMnO4 solution.332viewsHas a video solution.