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
Concept explainers
Question
thumb_up100%
Transcribed Image Text:2+
4+
a. Will Fe+ oxidize Sn
to Sn*t ? Assume that the reaction occurs at standard electrochemical conditions.
Half-Reaction
e° (V)
Fes+ +e → Fe2+
+0.77
Sn
n4+
+ 2e → Sn²+
+0.15
O yes
O no
b. Will dichromate ions oxidize chloride ions to free chlorine in acidic solution? Assume that the reaction occurs at standard electrochemical conditions.
Half-Reaction
e° (V)
Cr2 0, + 14H+ + 6e¯ → 2Cr³+ + 7H2O +1.33
Cl2 + 2e → 2C1
+1.36
O yes
O no
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
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 galvanic cell is prepared using copper and silver. Its cell notation is shown below: Cu(s) | Cu2+(aq) || Ag+(aq) | Ag(s) Which of the following processes occurs at the cathode? A. Cu(s) → Cu2+(aq) + 2e- B. Cu2+(aq) + 2e- → Cu(s) C. Ag+(aq) + e- → Ag(s) D. Ag(s) → Ag+(aq) + e- E. Cu(s) + 2Ag+(aq) → Cu2+(aq) + 2Ag(s) Copper is electroplated from a CuSO4 solution. A constant current of 4.54 A is applied by an external power supply. How long (minutes) will it take to deposit 0.985 g of Cu? (the answer should be entered with 3 significant figures; do not enter units; give answer in normal notation--examples include 1.23 and 120. and -123 and 123. and 12.3) DOnt need work shown just answer asap Predict the sign of ΔSorxn (positive or negative) for the following reactions: CH3OH(l) → CH3OH(s) CH4(g) + H2O(g) → CO(g) + 3…arrow_forwardCalculate the concentration of an unknown solution in a concentration cell. A concentration cell consisting of two hydrogen electrodes (P H2- latm), where the cathode is a standard hydrogen electrode and the anode solution has an unknown pH, has a cell voltage of 0.193 V. What is the pH in the unknown solution? Assume the temperature of the solutions is 298 K. !! pH =arrow_forwardA student wanted to measure the concentration of cobalt(II) ion in an aqueous solution. For the cathode half-reaction, she used a silver electrode with a 0.51 M solution of AgNO3. For the anode half-reaction, she used a cobalt electrode dipped into the aqueous solution. If the cell gave a potential of 1.043 V at 25 °C, what was the concentration of Co2+ in the solution? Half-reaction E° (V) Ag*(aq) + e- Ag(s) +0.7996 Co2+(aq) + 2 e- -0.28 Co(s) Your Answer: Answer unitsarrow_forward
- › Calculate the standard free-energy change for the reaction at 25 °C. Refer to the list of standard reduction potentials. 2 Au³ +(aq) + 3 Ni(s) = 2 Au(s) + 3 Ni² + (aq) AGⓇ = kJarrow_forward5. Consider the following under acidic conditions: Cu(s) + MnO4¹ (aq) → Mn²+ + Cu²+ i ii Write the balanced half-reaction for the oxidation that occurs. Write the balanced half-reaction for the reduction that occurs. iii Write the balanced redox reaction. iv Write the potential for each half-reaction next to it (the values are in your text) V Calculate the cell potential. vi Calculate AG at 25 °C. vii Is this reaction spontaneous? Why? viii Draw and label the cell for this reaction. ix Write the line notation for the cell.arrow_forwardConsider the following voltaic cellat 25°C: Al(s) | Al3*(0.20 M, aq) || Al3+(0.75 M, aq) | Al(s) If the standard reduction potential for the Al3+(aq) /Al(s) redox couple is -1.66 V, what is the overall cell reaction and the cell potential of the voltaic cell shown above? (Reference the cell as written above.) The overall cell reaction is Al3+(0.75 M, aq) AIS*(0.20 M, ag) and E°cell = +0.0113 V. There is no overall cell reaction and E°cell = 0.00 V. The overall cell reaction is Al3+(0.20 M, aq) Als*(0.75 M, aq) and E°cell = +0.0113 V. The overall cell reaction is Al3+(0.20 M, aq) →A13+(0.75 M, ag) and E°cell| = -0.0113 V. The overall cell reaction is Al3*(0.75 M, aq) →AI3*(0.20 M, aq) and E°cell = -0.0113 V. None of thesearrow_forward
- 29barrow_forwardCalculate the cell potential for the galvanic cell in which the given reaction occurs at 25 °C, given that [Nit] = 0.00170 M and [Au] = 0.868 M. Standard reduction potentials can be found in this table. %3D 3 Ni(s) + 2 Au*(aq) 3 Ni?+(aq) + 2 Au(s) E = Varrow_forwardA silver oxide–zinc cell maintains a fairly constant voltage during discharge (1.60 V).The button form of this cell is used in watches, hearing aids, and other electronic devices.The half-reactions are:Zn(s) + 2OH- (aq) → Zn(OH)2(s) + 2eAg2O(s) + H2O(l) + 2e- → 2Ag(s) + 2OH(aq)(a) Identify the anode and the cathode reactions.(b) What’s the overall reaction in this galvanic cell?arrow_forward
- Consider the following reduction potentials. Ag*(aq) + e → Ag(s) E° = + 0.80 V Sn2*(aq) + 2 e -→Sn(s) E° = - 0.14 V Mg2 (aq) + 2 e - → Mg(s) E° = - 2.37 V a.) Calculate the cell potential at standard conditions (E°cell) for a voltaic cell of Mg2+/Mg and Ag*/Ag, in Volts. E° cell = v b.) Calculate Ecel in V at 298 K if [Mg2*] = 0.100 M and [Ag*] = 0.100 M. %3D Ecell = Varrow_forwardBalance the following reactions. Calculate the cell potential and the Gibbs free energy of these reactions at standard conditions. Identify the reactions with K > 1 among the following redox reactions. Write the line representations for the Galvanic cells, indicating the anode and 1. cathode. a. Cl2 + Br → Ct + Br2 b. Mnoa + H* + Ce → Cet + Mn2 + H20arrow_forwardGibbs free energy= -434250 J/mol for a galvanic cell whose two half-reactions: Mt3+ (aq) + 3 e1- → Mt (s), and R2+ (aq) + 2 e1- → R (s), have standard reduction potentials of 1.09 V and 0.34 V respectivelyarrow_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