Galvanic Cells. Calculate the cell voltage for a voltaic cell created by connecting a copper electrode to a tin electrode. The copper electrode is immersed.

Slides:

Advertisements

Similar presentations

Chapter 7- Molecular Formulas

Advertisements

Chapter 7 Chemical Reactions.

ELECTROCHEMISTRY.

Reactions in Aqueous Solutions Chapter 7

Chapter 9 Chemical Quantities.

Redox potentials Electrochemistry ICS.

What is the % composition of carbon in benzene (C6H6)?

Oxidation Numbers HV2O4-  V6+

Electrochemistry Applications of Redox.

Learning Chemical Formulas

HKCEE Chemistry Volumetric Analysis &

Solution Stoichiometry (Lecture 3) More examples on volumetric analysis calculations.

Ionic Bonding Chapter 20.

Basic Concepts of Electrochemical Cells

Chemical Reaction and Equations

Calculations from Chemical Equations Chapter 9 Outline I.Stoichiometry using Chemical Equations A.Mole Relationships B.Limiting Reagent C.Percent Yield.

Chapter 7 Chemical Reactions.

Electrochemistry Generating Voltage (Potential)

Electrochemistry.

1 © 2006 Brooks/Cole - Thomson Balancing Equations for Redox Reactions Some redox reactions have equations that must be balanced by special techniques.

Chapter 20 Principles of Reactivity: Electron Transfer Reactions

IB topic 9 Oxidation-reduction

Chpater 4 Oxidation-Reduction

Electrochemistry Chapter 19

Chapter 20: Electrochemistry

A galvanic cell is made from two half cells. In the first, a platinum electrode is immersed in a solution at pH = 2.00 that is M in both MnO 4 -

(c) 2006, Mark Rosengarten Voltaic Cells  Produce electrical current using a spontaneous redox reaction  Used to make batteries!batteries  Materials.

Standard Reference Electrode Standard Hydrogen Electrode (SHE) SHE: Assigned V Can be anode or cathode Pt does not take part in reaction Difficult.

Galvanic Cells What will happen if a piece of Zn metal is immersed in a CuSO 4 solution? A spontaneous redox reaction occurs: Zn (s) + Cu 2 + (aq) Zn 2.

Electrochemistry II. Electrochemistry Cell Potential: Output of a Voltaic Cell Free Energy and Electrical Work.

Lecture 253/27/06 Bottle and Can drive today 11-3 Hagan Info Booth Seminar today at 4 pm.

Lecture 223/19/07. Displacement reactions Some metals react with acids to produce salts and H 2 gas Balance the following displacement reaction: Zn (s)

Electrochemistry Chapter 11 Web-site:

Chapter 20 Preview Multiple Choice Short Answer Extended Response

ELECTROCHEMICAL CELLS. TASK Sequence these elements starting from the most reactive to the least reactive: Na, Pt, Au, C, H, Sn, Pb, Al, C, Mg, Li, Ca,

GALVANIC AND ELECTROLYTIC CELLS

Activity Series lithiumpotassiummagnesiumaluminumzincironnickelleadHYDROGENcoppersilverplatinumgold Oxidizes easily Reduces easily Less active More active.

What is powering this clock?. How much Voltage You can see the battery is missing and the clips are attached to the terminals. What is the voltage required.

1 Chapter Eighteen Electrochemistry. 2 Electrochemical reactions are oxidation-reduction reactions. The two parts of the reaction are physically separated.

OXIDATION AND REDUCTION. Oxidation Losing electrons The higher positive oxidation number the more the atom has loss control over the electrons, therefore.

Electrochemistry: Oxidation-Reduction Reactions Zn(s) + Cu +2 (aq)  Zn 2+ (aq) + Cu(s) loss of 2e - gaining to 2e - Zinc is oxidized - it goes up in.

III, IV, VIII, and IX 2.I, II, VI, and IX 3.II, III, VI,

Cells and corrosion. AN ACTIVITY SERIES FOR METALS ■ With oxygen Li, Na, K, Ca and Ba react rapidly at room temperature, while Mg, Al, Zn and Fe react.

REDOX Part 2 - Electrochemistry Text Ch. 9 and 10.

Electrochemistry Chapter 5. 2Mg (s) + O 2 (g) 2MgO (s) 2Mg 2Mg e - O 2 + 4e - 2O 2- Oxidation half-reaction (lose e - ) Reduction half-reaction.

Nernst Equation Walther Nernst

Ions: Naming Practice SNC2D. F-F-F-F- F - Fluoride.

Reactions of Metals. Reactions of Metals with H 2 O The metal is the anode and will be oxidized. 2H 2 O + 2e-  2OH - + H 2 E° = V Mg  Mg 2+ +

Chapter 20 Problem Set: p , 11, 13, 17, 23, 27, 31, 35, 43, 45, 47, 53, 61, 63, 69, 72, 75, 79, 85, 87, 95.

Daily Quiz. Calculate the cell potential of voltaic cells that contain the following pairs of half-cells:

Zn (s) + Cu2+ (aq)  Zn2+ (aq) + Cu (s)

Electrochemistry Lesson 2

Bell Ringer Complete and balance each of the following synthesis reactions by writing chemical equations. a. Na + O2→ ______ b. Mg + F2 → ______ a. 4Na.

CONSTRUCTING RELATIVE REACTIVITY TABLES

Ionic compounds continued

Cell Potentials and Good Batteries

Oxidation-Reduction Chapter 17

Reactions of Metals.

Voltaic Cells Aim: To identify the components and explain the functions of an electrochemical (voltaic) cell.

Cell Potentials and Good Batteries

Section 3: Transition Metal Ions

Electrochemistry Lesson 3

Semester 2 Final Review College Chemistry.

Electrochemical Cells (Batteries)

Write the oxidation half reaction for lithium oxidizing

Zn (s) + Cu2+ (aq)  Zn2+ (aq) + Cu (s)

Ionic Compounds An ionic compound results when a metal is attracted to a nonmetal The metal becomes positive because they have a tendency to lose electrons.

Presentation transcript:

Galvanic Cells

Calculate the cell voltage for a voltaic cell created by connecting a copper electrode to a tin electrode. The copper electrode is immersed in a solution of copper(II) nitrate. The tin electrode is immersed in tin(II) nitrate V V V V V

Determine the voltage for the following reaction. All solutions are 1.0 M and the temperature is 25 o C. Mn 2+ + Pb  Mn + Pb V V V V V

Calculate the standard free energy change, ∆G o, for the reaction below. Cu 2+ + Fe  Cu + Fe kJ kJ kJ kJ kJ

A piece of copper metal is placed into solutions containing each of the following three cations. Which ion will be reduced by the copper metal? I. Sn 2+ II. Zn 2+ III. Ag + 1.I only 2.II only 3.III only 4.I and II 5.I, II, and III

Determine the voltage for the following reaction. The manganese solution is 1.0 M while the lead solution is M. The temperature is 25 o C. Mn + Pb 2+  Mn 2+ + Pb V V V V V

In the following equation, ____ is being oxidized and ____ is being reduced. Cr 2 O Fe 2+ + H + + HSO 4 -  Cr 3+ + Fe 3+ + H 2 O + SO S, H 2.Cr, O 3.Fe, S 4.Fe, Cr 5.Fe, H 1234

Determine the oxidation state of sulfur in the compound Na 2 SO

4 NH O 2  4 NO + 6 H 2 O In the above reaction, 3.10 g of NH 3 reacts with 2.50 g of O 2. What is the theoretical yield of NO? g g g g g 1234

A solution is made by dissolving g of K 2 CrO 4 in 1.00 kg of water. What will the freezing point of the new solution be? K f for water is 1.86 o C m -1. : o C o C o C o C o C 1234