Unit A Review Questions
... The reduction of the chromium ion appears below the oxidation of copper metal. Therefore, this reaction is non-spontaneous. b. The reduction of the hydrogen ion appears above the oxidation of zinc metal. Therefore, this reaction is spontaneous. c. The reduction of the hydrogen ion appears below the ...
... The reduction of the chromium ion appears below the oxidation of copper metal. Therefore, this reaction is non-spontaneous. b. The reduction of the hydrogen ion appears above the oxidation of zinc metal. Therefore, this reaction is spontaneous. c. The reduction of the hydrogen ion appears below the ...
Slide 1
... Electrolytic cell: electrical energy is used to bring about a non spontaneous reaction. Oxidation-reduction (redox) reactions occur when electrons are given up by the substance being oxidized (the reducing agent) and simultaneously gained by the substance being reduced (the oxidizing agent). 2 Ag+ + ...
... Electrolytic cell: electrical energy is used to bring about a non spontaneous reaction. Oxidation-reduction (redox) reactions occur when electrons are given up by the substance being oxidized (the reducing agent) and simultaneously gained by the substance being reduced (the oxidizing agent). 2 Ag+ + ...
determining oxidation numbers
... 1. The oxidation number (ON) for any element is zero. 2. For monatomic ions, the ON is equal to the charge on the ion. 3. Fluorine always has an ON = -1 in compounds. 4. The ON for oxygen is -2 in compounds, except in peroxides, when it is 1, or bound to fluoride, when it is +2. 5. Other halogens ha ...
... 1. The oxidation number (ON) for any element is zero. 2. For monatomic ions, the ON is equal to the charge on the ion. 3. Fluorine always has an ON = -1 in compounds. 4. The ON for oxygen is -2 in compounds, except in peroxides, when it is 1, or bound to fluoride, when it is +2. 5. Other halogens ha ...
ch19 MSJ jlm
... Cu will be oxidized to produce Cu2+ {Cu(s) Cu+2(aq) + 2e-}. Ag+ will be reduced to produce Ag {Ag+(aq) + e- Ag(s)}. This needs to be balanced by negative (-) charges. But how? Add a salt bridge (inverted U tube with solution of ions, e.g. Na+ NO3-) Through salt bridge, anions (NO3-) can now move ...
... Cu will be oxidized to produce Cu2+ {Cu(s) Cu+2(aq) + 2e-}. Ag+ will be reduced to produce Ag {Ag+(aq) + e- Ag(s)}. This needs to be balanced by negative (-) charges. But how? Add a salt bridge (inverted U tube with solution of ions, e.g. Na+ NO3-) Through salt bridge, anions (NO3-) can now move ...
Nel 4U: UNIT 7 LESSONS “ELECTROCHEMISTRY”
... Oxidation & Reduction reactions occur in many chemical systems. Examples include the rusting of iron, the displacement of metals and photosynthesis in plants. All of these reactions involve the transfer of electrons from one chemical species to another. Because “electrons” are involved in all these ...
... Oxidation & Reduction reactions occur in many chemical systems. Examples include the rusting of iron, the displacement of metals and photosynthesis in plants. All of these reactions involve the transfer of electrons from one chemical species to another. Because “electrons” are involved in all these ...
Student Notes
... 10e– + 16H+(aq) + 2MnO4– (aq) 2Mn2+(aq) + 8H2O(l) 5C2O42– (aq) 10CO2(g) + 10e– • Now add the reactions and simplify. 16 H+1(aq) + 2 MnO4–1 (aq) + 5 C2O42– (aq) 2 Mn2+(aq) + 8 H2O(l) + 10 CO2(g) • The equation is now balanced! • Note that all of the electrons have cancelled out ! Balancing Equa ...
... 10e– + 16H+(aq) + 2MnO4– (aq) 2Mn2+(aq) + 8H2O(l) 5C2O42– (aq) 10CO2(g) + 10e– • Now add the reactions and simplify. 16 H+1(aq) + 2 MnO4–1 (aq) + 5 C2O42– (aq) 2 Mn2+(aq) + 8 H2O(l) + 10 CO2(g) • The equation is now balanced! • Note that all of the electrons have cancelled out ! Balancing Equa ...
Unit Powerpoint
... Electrochemistry is the branch of chemistry that deals with the conversion of chemical energy to electrical energy. 1. Electrochemical Cells – spontaneous chemical reactions convert chemical energy into electrical energy. Batteries are an example. 2. Electrolytic Cells – electrical energy is used ...
... Electrochemistry is the branch of chemistry that deals with the conversion of chemical energy to electrical energy. 1. Electrochemical Cells – spontaneous chemical reactions convert chemical energy into electrical energy. Batteries are an example. 2. Electrolytic Cells – electrical energy is used ...
Electrochemistry
... it is bonded to metals in binary compounds. In these cases, its oxidation number is –1. 5. Group IA metals are +1, IIA metals are +2 and fluorine is always –1. ...
... it is bonded to metals in binary compounds. In these cases, its oxidation number is –1. 5. Group IA metals are +1, IIA metals are +2 and fluorine is always –1. ...
half-reactions - Clayton State University
... - Produces electrical energy from chemical energy - Can be reversed electrolytically for reversible cells Example Rechargeable batteries ...
... - Produces electrical energy from chemical energy - Can be reversed electrolytically for reversible cells Example Rechargeable batteries ...
Oxidation and Reduction Reactions
... Describe, using a diagram, the essential components of an electrolytic cell. The diagram should include the source of electric current and conductors, positive and negative electrodes and the electrolyte. State that oxidation occurs at the positive electrode (anode) and reduction occurs at the negat ...
... Describe, using a diagram, the essential components of an electrolytic cell. The diagram should include the source of electric current and conductors, positive and negative electrodes and the electrolyte. State that oxidation occurs at the positive electrode (anode) and reduction occurs at the negat ...
Chemistry B2A Chapter 18 Oxidation
... In some reactions, it is not easy to see the electron loss and gain, so chemists developed another definition of oxidation and reduction: Oxidation is the gain of oxygen atoms and/or the loss of hydrogen atoms. Reduction is the loss of oxygen atoms and/or the gain of hydrogen atoms. CH4(g) + 2O2(g) ...
... In some reactions, it is not easy to see the electron loss and gain, so chemists developed another definition of oxidation and reduction: Oxidation is the gain of oxygen atoms and/or the loss of hydrogen atoms. Reduction is the loss of oxygen atoms and/or the gain of hydrogen atoms. CH4(g) + 2O2(g) ...
Chapter 1: Fundamental Concepts
... 1. A large electrolytic cell that produces metallic aluminum from Al2O3 ore is capable of making 250 kg of aluminum in 24 hours. Determine the current (in amps) that is required for this process. Include appropriate chemical reactions. 3.1 x 104 amps (Al3+(aq) + 3 e– --> Al(s) is ½-reaction, overall ...
... 1. A large electrolytic cell that produces metallic aluminum from Al2O3 ore is capable of making 250 kg of aluminum in 24 hours. Determine the current (in amps) that is required for this process. Include appropriate chemical reactions. 3.1 x 104 amps (Al3+(aq) + 3 e– --> Al(s) is ½-reaction, overall ...
03.Thermodynamics in Corrosion Engineering
... control corrosion of pure metals in the aqueous environment By altering the pH and potential to the regions of immunity and passivation, corrosion can be controlled. For example, on increasing the pH of environment in moving to slightly alkaline regions, the corrosion of iron can be controlled C ...
... control corrosion of pure metals in the aqueous environment By altering the pH and potential to the regions of immunity and passivation, corrosion can be controlled. For example, on increasing the pH of environment in moving to slightly alkaline regions, the corrosion of iron can be controlled C ...
AP* Chemistry ELECTROCHEMISTRY Terms to Know
... – The electrons in a voltaic or galvanic cell ALWAYS flow From the Anode To the CAThode – the cathode is + in galvanic (voltaic) cells, so it stands to reason the anode is negative Salt Bridge – bridge between whose purpose is to provide to balance the charge. Usually made of a salt filled agar (KNO ...
... – The electrons in a voltaic or galvanic cell ALWAYS flow From the Anode To the CAThode – the cathode is + in galvanic (voltaic) cells, so it stands to reason the anode is negative Salt Bridge – bridge between whose purpose is to provide to balance the charge. Usually made of a salt filled agar (KNO ...
IntroRedoxDCIAns
... d. Define the terms oxidation, reduction, oxidizing agent and reducing agent. Oxidation is characterized by the loss of electrons. Reduction is characterized by the gain of electrons. An oxidizing agent is a chemical which causes another chemical to be oxidized and itself to be reduced. A reducing a ...
... d. Define the terms oxidation, reduction, oxidizing agent and reducing agent. Oxidation is characterized by the loss of electrons. Reduction is characterized by the gain of electrons. An oxidizing agent is a chemical which causes another chemical to be oxidized and itself to be reduced. A reducing a ...
Introduction to Oxidation Reduction
... d. Define the terms oxidation, reduction, oxidizing agent and reducing agent. Oxidation is characterized by the loss of electrons. Reduction is characterized by the gain of electrons. An oxidizing agent is a chemical which causes another chemical to be oxidized and itself to be reduced. A reducing a ...
... d. Define the terms oxidation, reduction, oxidizing agent and reducing agent. Oxidation is characterized by the loss of electrons. Reduction is characterized by the gain of electrons. An oxidizing agent is a chemical which causes another chemical to be oxidized and itself to be reduced. A reducing a ...
Wet Corrosion Conditions for Wet Corrosion Just as we live in an
... 1. There must be two dissimilar metals. Metals of different chemistry provide the obvious example, such as using steel nails to secure a copper sheet. Not as obvious is that, even with the same chemistry, differences in grain size or different amounts of cold working can drive electrochemical attack ...
... 1. There must be two dissimilar metals. Metals of different chemistry provide the obvious example, such as using steel nails to secure a copper sheet. Not as obvious is that, even with the same chemistry, differences in grain size or different amounts of cold working can drive electrochemical attack ...
Chemistry Handout 08 - (Redox)
... According to the Activity Series chemistry reference table, which of these metals will react most readily with 1.0 M HCl to produce H2 (g)? A) Zn ...
... According to the Activity Series chemistry reference table, which of these metals will react most readily with 1.0 M HCl to produce H2 (g)? A) Zn ...
Electrochemistry
Electrochemistry is the branch of physical chemistry that studies chemical reactions which take place at the interface of an electrode, usually a solid metal or a semiconductor, and an ionic conductor, the electrolyte. These reactions involve electric charges moving between the electrodes and the electrolyte (or ionic species in a solution). Thus electrochemistry deals with the interaction between electrical energy and chemical change.When a chemical reaction is caused by an externally supplied current, as in electrolysis, or if an electric current is produced by a spontaneous chemical reaction as in a battery, it is called an electrochemical reaction. Chemical reactions where electrons are transferred directly between molecules and/or atoms are called oxidation-reduction or (redox) reactions. In general, electrochemistry describes the overall reactions when individual redox reactions are separate but connected by an external electric circuit and an intervening electrolyte.