Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
expand_more
expand_more
format_list_bulleted
Related questions
Question
Transcribed Image Text:Consider the following reaction.
Fe3+(aq) + Sn2+(aq)
→ Fe2+(aq) + Sn4+(aq)
(a) Select all that apply.
Sn2+ is the reducing agent.
Fe3+ is the substance being reduced.
Fe3+ is the substance being oxidized.
Fe3+
is the reducing agent.
Sn2+ is the substance being reduced.
Fe3+ is the oxidzing agent.
Sn2+ is the oxidzing agent.
Sn2+ is the substance being oxidized.
Type the following answers using the formats given. Use only the format '1+' or '1-' for the charge on an ion. If only one electron is present in the half-cell reaction, type the answer as e- instead of 1e-.
Half-cell Equation
Au3+(aq) + 3 e¯ →
Au(s)
Typed Answer
Au3+(aq) + 3e- > Au(s)
Balanced Equation 2 Au3+(aq) + 3 Zn(s)
2 Au(s) + 3 Zn²+(aq)
Typed Answer
2AU3+(aq) + 3Zn(s) > 2Au(s) + 3Zn2+(aq)
(b) Write the half-cell reaction for the oxidation.
(c) Write the half-cell reaction for the reduction.
(d) Write the balanced equation for the cell reaction. Keep substances in the order given in the original equation.
O O O
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
This is a popular solution
Trending nowThis is a popular solution!
Step by stepSolved in 2 steps with 2 images
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- A common shorthand way to represent a voltaic cell isanode& anode solution& & cathode solution&cathodeA double vertical line represents a salt bridge or a porousbarrier. A single vertical line represents a change in phase,such as from solid to solution. (a) Write the half-reactionsand overall cell reaction represented by Fe| Fe2+ || Ag+ |Ag;calculate the standard cell emf .(b) Write the half-reactions and overall cell reaction representedby Zn| Zn2+ || H+ |H2; calculate the standard cell emf and use Pt for the hydrogen electrode.(c) Using the notation just described, represent a cellbased on the following reaction:ClO3-(aq) + 3 Cu(s) + 6 H+(aq) --->Cl-(aq) + 3 Cu2+(aq) + 3 H2O(l)Pt is used as an inert electrode in contact with the ClO3-and Cl-. Calculate the standard cell emf given: ClO3-(aq) +6 H+(aq) + 6 e- ------>Cl-(aq) + 3 H2O(l); E° = 1.45 V.arrow_forwardEnter electrons as e". A voltaic cell is constructed in which the anode is a Fe|Fe2+ half cell and the cathode is a F"|F2 half cell. The half-cell compartments are connected by a salt bridge. (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) The anode reaction is: + + The cathode reaction is: + The net cell reaction is: + In the external circuit, electrons migrate e the Fe|Fe2+ electrode e the F"|F2 electrode. from or to ? from or to? In the salt bridge, anions migrate e the F'|F2 compartment e the Fe|Fe2+ compartment. from or to? from or to ? +arrow_forwardConsider the following two half-reactions and their standard reduction potentials for a voltaic cell. N2O(g)+2H+ (aq)+2e-N2(g)+H2O(l) E° = 1.766 V MnO-4(aq)+4H+ (aq)+3e-MnO2(s)+2H2O(l) E° = 1.673 V 3N2O(g)+2MnO2(s)+H2O(l)3N2(g)+2MnO- 4(aq)+2H+(aq) Calculate the value of AG for the reaction above.arrow_forward
- A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential Br,(1)+2e - 2 Br (aq) =+1.065 V ʼred MnO,(aq)+2 H,O(1)+3e MnO,(s)+4 ОН (аq) E=+0.59 V (red Answer the following questions about this cell. Write a balanced equation for the half-reaction that happens at the cathode. x10 Write a balanced equation for the half-reaction that happens at the anode. Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written.arrow_forwardFor the following reaction, predict the measured cell potential (Ecell) if the pressure of O₂ is 1.83 atm, the concentration of H* is 7.59 x 10-3 M and the bromide ion concentration is 2.53 M. O₂(g) + 4H*(aq) + 4Br (aq) → 2H₂O(l) + 2Br₂(!) Half reactions: 2Br₂ (1)+4e4 Br (aq) O₂(g) + 4H*(aq) + 4e¯→ 2H₂O(l) O 0.054 V O 2.208 V 0.007 V O 0.250 V 0.033 V E° = +1.077 V E° - +1.229 Varrow_forwardWrite the overall reaction for the Redox reaction (below) when it occurs in a basic environment. H3ASO4 (aq) + Zn (s) → AsH3 (1) + Zn²+ (aq) Steps for writing half-cell reactions and overall Redox reactions: 1. Balance atoms other than H and O by changing their coefficients 2. Balance the O's and H's by adding OH and/or H₂O 3. Add electrons to balance the charge 4. Add the Oxidation and Reduction equations once the electrons in each cancel out 5. Cancel out (or reduce to the lowest possible numbers) any other species that are present on both sides of the reaction More Information H3ASO4 + AsH3 Zinc + Zinc ionsarrow_forward
- Consider the galvanic cell based on the following half-reactions. Ag+ + e Ni²+ + 2e →→ Ni (a) Determine the overall cell reaction and calculate Omit states-of-matter from your answer.) chemPad XX→ (c) 8 cell → Ag 8⁰ = +0.80 V 8° -0.23 V Calculate 8 Help Greek º (b) Calculate AGº (in kJ) and K for the cell reaction at 25°C. AGO kJ K (in V). (Use the lowest possible whole number coefficients. cell (in V) at 25°C when [Ag+] = 1.0x10-4 M and [Ni²+] = 1.0×10-² M. cell Varrow_forwardA galvanic cell is represented by the shorthand Cu | Cu²* || Ag* | Ag. Which reaction occurs at the anode? A) Cu(s) → Cu²*(aq) + 2e- B) Ag*(aq) + e¯ → Ag(s) C) Cu2*(aq) + 2e → Cu(s) D) Ag(s) → Ag*(aq) + e-arrow_forward13. The standard reduction potentials sh for four half-cells at 298 K are given (B in Table 1, * Table 1 Half-cell equation 2H (aq) +O2 (g) +2e H2O2 (aq) H2O2 (aq)+ 2H (aq) +2e 2H20 () C2 (g) + 2e" - 2Cl (aq) MnO2 (s) +4H* (aq) + 2e Mn* (aq) +2H20 (1) E V +0.68 +1.77 +1.36 +1.22 In which of the following mixture there is NO effervescence observed? A. H2O2 (aq) + Ch (g) B. acidified H2O2+ MnO2 (s) C NaCl (aq) + acidified H2O2 (aq) D. NaCl (ag) + acidified MnO2 (s)arrow_forward
arrow_back_ios
arrow_forward_ios
Recommended textbooks for you
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
ChemistryChemistryISBN:9781259911156Author:Raymond Chang Dr., Jason Overby ProfessorPublisher:McGraw-Hill Education
Principles 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 Education
Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning
Elementary Principles of Chemical Processes, Bind...ChemistryISBN:9781118431221Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. BullardPublisher:WILEY
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemistry
Chemistry
ISBN:9781259911156
Author:Raymond Chang Dr., Jason Overby Professor
Publisher:McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:9781305577213
Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:Cengage Learning
Organic Chemistry
Chemistry
ISBN:9780078021558
Author:Janice Gorzynski Smith Dr.
Publisher:McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
Elementary Principles of Chemical Processes, Bind...
Chemistry
ISBN:9781118431221
Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:WILEY