Calculate the standard cell potential for each of the following electrochemical cells.
You may want to reference (Pages 854 - 861) Section 19.4 while completing this problem.
a) Cr2O72−(aq)+14H+(aq)+6I−(aq)→2Cr3+(aq)+7H2O(l)+3I2(s)
Calculate the standard cell potential for each of the following electrochemical cells. You may want to...
Consider the following balanced cell reaction: Cr2O72- + 14H+ + 6I- ⟶ 2Cr3+ + 3I2+ 7H2O In the determination of the cell potential at nonstandard conditions, the value that should be used for “n” (i.e. number of electrons transferred) in the Nernst equation is: A. 2 B. 6 C. 1 D. 4 E. 5
An electrochemical cell is based on the following two half-reactions: Part A oxidation: Sn (s) +Sn2+ (aq, 1.70 M)+2e reduction: CIO2(g, 0.265 atm )+e+C10(aq, 2.00 M) You may want to reference (Pages 865 - 869) Section 19.6 while completing this problem. Compute the cell potential at 25°C. Express the cell potential to three significant figures. ME PO ΑΣΦ ? Ecco V Submit Request Answer
use tabulated standard electrode potential to calculate the standard cell potential for the reaction occurring in an electrochemical cell at 25 C. (The equation is balanced.) 3Ni^2+(aq)+2Cr(s)--->3Ni(s)2Cr^3+(aq) Express your answer to two significant figures and include the appropriate units. em 26 E (V) -0.45 -0.50 -0.73 -0.76 -1.18 Standard reduction half-cell potentials at 25°C Half-reaction E° (V) Half-reaction Aul+ (aq) + 3e +Au(s) 1.50 Fe2+ (aq) + 2eFe(s) Ag+ (aq) +e-Ag(s) 0.80 Cr3+ (aq) + Cr²+ (aq) Fe+(aq) + 3e...
Choose the label which best describes the following: A B C D E F G H Direction which anions move through the salt bridge A B C D E F G H Pt anode The overall, balanced, spontaneous reaction occurring in this (standard) cell is: Cr2O72−(aq) + 6Cl−(aq) + 14H+(aq) → 7H2O(l) + 2Cr3+(aq) + 3Cl2(g) 7H2O(l) + 2Cr3+(aq) + 3Cl2(g) → Cr2O72−(aq) + 6Cl−(aq) + 14H+(aq) 7H2O(l) + 2Cr3+(aq) + Cl2(g) → Cr2O72−(aq) + 2Cl−(aq) + 14H+(aq) 2Cr3+(aq) + 3Cl2(g) →...
The electrochemical cell described by the balanced chemical reaction has a standard cell potential of -0.2 V. Calculate the equilibrium constant (Kc) for the reaction at 298 K. Round your answer to 3 significant figures. H2SO3(aq) + H2O(l) → H2(g) + SO42-(aq) + 2H+(aq) The electrochemical cell described by the cell notation has a standard cell potential of -0.10 V. Calculate the value (kJ) for the ΔG˚ of the cell. Round your answer to 3 significant figures. Pt(s) l Cr3+(aq),...
2. Calculate the standard cell emf (cell potential) for electrochemical cells having the following overall cell reactions and predict if they are spontaneous: a) Sn(s) + Pb2+ (aq) → Sn?" (aq) + Pb(s) Eºcell = Volts. Spontaneous? b) 2002 (aq) + Zn?"(aq) → 2Co3+ (aq) + Zn(s) Eºcell__volts; Spontaneous? c) Cl2(g) + 2Br (aq) + 2Cl(aq) + Br2(1); E° = volts; Spontaneous?
Calculate the equilibrium constant for each of the reactions at 25 °C. Part B You may want to reference (Pages 861 - 865) Section 19.5 while completing this problem. O2 (g) + 2H20 (1) + 2Cu (s) ~40H(aq) + 2Cu²+ (aq) Express your answer using two significant figures. EVO ALO ? K = Submit Previous Answers Request Answer Cr(s) + Fe2+ (aq) → Cr3+ (aq) + Fe(s) Express your answer as a chemical equation. Identify all of the phases in...
You may want to reference (Pages 910 - 914) section 19.6 while completing this problem. Part B A voltaic cell employs the following redox reaction: 2 Fe+ (aq) +3 Mg(s) +2 Fe (s) + 3 Mg?(aq) Calculate the cell potential at 25°C under each of the following conditions. Fe+] = 1.8x10-3M; Mg²+] = 2.35 M Express your answer in units of volts. VALD O ? Submit Request Answer
A voltaic cell employs the following redox reaction: 2Fe3+(aq)+3Mg(s)→2Fe(s)+3Mg2+(aq) Calculate the cell potential at 25 ∘C under each of the following conditions. You may want to reference (Pages 865 - 869) Section 19.6 while completing this problem. Part A standard conditions Express your answer in units of volts. Ecell = V Part B [Fe3+]= 1.2×10−3 M ; [Mg2+]= 1.70 M Express your answer in units of volts. Ecell = V SubmitRequest Answer Part C [Fe3+]= 1.70 M ; [Mg2+]=1.2×10−3 M...
Item 16 You may want to reference (Pages 910 - 914) section 19.6 while completing this problem. Part A A voltaic cell employs the following redox reaction: 2 Fe+ (aq) + 3 Mg(s) + 2 Fe(s) + 3 Mg?+ (aq) Calculate the cell potential at 25°C under each of the following conditions. standard conditions Express your answer in units of volts. 180 AD O ? Ecell = Submit Request Answer Part B FeS+] = 1.6x10-4M; Mg2+] = 2.40 M Express...