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- https://chem.libretexts.org/Courses/University_of_North_Texas/UNT%3A_CHEM_1410_-_General_Chemistry_for_Science_Majors_I/Text/04%3A_The_Structure_of_Atoms/4.09%3A_The_ElectronThus the molar mass of an electron is 5.48 × 10 –4 g mol –1 , and if we think of the electron as an “atom“(or indivisible particle) of electricity, its atomic weight would be 0.000548—only \(\tfrac{1}...Thus the molar mass of an electron is 5.48 × 10 –4 g mol –1 , and if we think of the electron as an “atom“(or indivisible particle) of electricity, its atomic weight would be 0.000548—only \(\tfrac{1}{1837}\) that of hydrogen, the lightest element known.
- https://chem.libretexts.org/Bookshelves/General_Chemistry/Map%3A_Chemistry_-_The_Central_Science_(Brown_et_al.)/20%3A_Electrochemistry/20.03%3A_Voltaic_CellsA galvanic (voltaic) cell uses the energy released during a spontaneous redox reaction to generate electricity, whereas an electrolytic cell consumes electrical energy from an external source to force...A galvanic (voltaic) cell uses the energy released during a spontaneous redox reaction to generate electricity, whereas an electrolytic cell consumes electrical energy from an external source to force a reaction to occur. Electrochemistry is the study of the relationship between electricity and chemical reactions. The oxidation–reduction reaction that occurs during an electrochemical process consists of two half-reactions, one representing the oxidation process and one the reduction process.
- https://chem.libretexts.org/Bookshelves/Analytical_Chemistry/Supplemental_Modules_(Analytical_Chemistry)/Analytical_Sciences_Digital_Library/In_Class_Activities/Electrochemical_Methods_of_Analysis/02_Text/7%3A_Electrochemical_Analytical_Methods/7.1%3A_Ion-Selective_ElectrodesIn solutions with exceptionally low ionic strength and low conductivity, the reading on a pH meter often takes a long time to stabilize after the pH electrode is inserted into the solution (rainwater ...In solutions with exceptionally low ionic strength and low conductivity, the reading on a pH meter often takes a long time to stabilize after the pH electrode is inserted into the solution (rainwater is an excellent example of a solution with a low ionic strength – a pH measurement is a convenient way to monitor the acidity in acid rain).
- https://chem.libretexts.org/Bookshelves/General_Chemistry/ChemPRIME_(Moore_et_al.)/11%3A_Reactions_in_Aqueous_Solutions/11.02%3A_Ions_in_Solution_(Electrolytes)In Binary Ionic Compounds and Their Properties we point out that when an ionic compound dissolves in water, the positive and negative ions originally present in the crystal lattice persist in solution...In Binary Ionic Compounds and Their Properties we point out that when an ionic compound dissolves in water, the positive and negative ions originally present in the crystal lattice persist in solution. Their ability to move nearly independently through the solution permits them to carry positive or negative electrical charges from one place to another. Hence the solution conducts an electrical current.
- https://chem.libretexts.org/Courses/Hope_College/CHEM_125/Exam_I/03%3A_The_Structure_of_Atoms/3.09%3A_The_ElectronThus the molar mass of an electron is 5.48 × 10 –4 g mol –1 , and if we think of the electron as an “atom“(or indivisible particle) of electricity, its atomic weight would be 0.000548—only \(\tfrac{1}...Thus the molar mass of an electron is 5.48 × 10 –4 g mol –1 , and if we think of the electron as an “atom“(or indivisible particle) of electricity, its atomic weight would be 0.000548—only \(\tfrac{1}{1837}\) that of hydrogen, the lightest element known.
- https://chem.libretexts.org/Bookshelves/General_Chemistry/ChemPRIME_(Moore_et_al.)/04%3A_The_Structure_of_Atoms/4.09%3A_The_ElectronThus the molar mass of an electron is 5.48 × 10 –4 g mol –1 , and if we think of the electron as an “atom“(or indivisible particle) of electricity, its atomic weight would be 0.000548—only \(\tfrac{1}...Thus the molar mass of an electron is 5.48 × 10 –4 g mol –1 , and if we think of the electron as an “atom“(or indivisible particle) of electricity, its atomic weight would be 0.000548—only \(\tfrac{1}{1837}\) that of hydrogen, the lightest element known.
- https://chem.libretexts.org/Courses/Bellarmine_University/BU%3A_Chem_104_(Christianson)/Phase_3%3A_Harnessing_Chemical_Power/10%3A_Electrochemistry/10.2%3A_Voltaic_CellsA galvanic (voltaic) cell uses the energy released during a spontaneous redox reaction to generate electricity, whereas an electrolytic cell consumes electrical energy from an external source to force...A galvanic (voltaic) cell uses the energy released during a spontaneous redox reaction to generate electricity, whereas an electrolytic cell consumes electrical energy from an external source to force a reaction to occur. Electrochemistry is the study of the relationship between electricity and chemical reactions. The oxidation–reduction reaction that occurs during an electrochemical process consists of two half-reactions, one representing the oxidation process and one the reduction process.
- https://chem.libretexts.org/Courses/Stanford_Online_High_School/TEN2B-Voltage/03%3A_Potential/3.03%3A_Voltaic_CellsA galvanic (voltaic) cell uses the energy released during a spontaneous redox reaction to generate electricity, whereas an electrolytic cell consumes electrical energy from an external source to force...A galvanic (voltaic) cell uses the energy released during a spontaneous redox reaction to generate electricity, whereas an electrolytic cell consumes electrical energy from an external source to force a reaction to occur. Electrochemistry is the study of the relationship between electricity and chemical reactions. The oxidation–reduction reaction that occurs during an electrochemical process consists of two half-reactions, one representing the oxidation process and one the reduction process.
- https://chem.libretexts.org/Bookshelves/Physical_and_Theoretical_Chemistry_Textbook_Maps/Thermodynamics_and_Chemical_Equilibrium_(Ellgen)/17%3A_Electrochemistry/17.02%3A_Electrochemical_CellsThe connection is made such that the electrical potential from the reference device opposes the potential from the electrochemical cell; that is, we connect the positive terminal of the reference devi...The connection is made such that the electrical potential from the reference device opposes the potential from the electrochemical cell; that is, we connect the positive terminal of the reference device to the positive terminal of the cell, and the negative terminal of the device to the negative terminal of the cell. (See Section 17.7.) We then vary the potential of the reference device until current flow in the circuit stops.
- https://chem.libretexts.org/Courses/Los_Angeles_Trade_Technical_College/Analytical_Chemistry/2%3A_Analytical_Chemistry_2.0_(Harvey)/12%3A_Electrochemical_Methods/12.1%3A_Overview_of_ElectrochemistryThe focus of this chapter is on analytical techniques that use a measurement of potential, charge, or current to determine an analyte’s concentration or to characterize an analyte’s chemical reactivit...The focus of this chapter is on analytical techniques that use a measurement of potential, charge, or current to determine an analyte’s concentration or to characterize an analyte’s chemical reactivity. Collectively we call this area of analytical chemistry electrochemistry because its originated from the study of the movement of electrons in an oxidation–reduction reaction. Despite the difference in instrumentation, all electrochemical techniques share several common features.
- https://chem.libretexts.org/Courses/Williams_School/Chemistry_IIA/06%3A_Electrochemistry/6.03%3A_Voltaic_CellsA galvanic (voltaic) cell uses the energy released during a spontaneous redox reaction to generate electricity, whereas an electrolytic cell consumes electrical energy from an external source to force...A galvanic (voltaic) cell uses the energy released during a spontaneous redox reaction to generate electricity, whereas an electrolytic cell consumes electrical energy from an external source to force a reaction to occur. Electrochemistry is the study of the relationship between electricity and chemical reactions. The oxidation–reduction reaction that occurs during an electrochemical process consists of two half-reactions, one representing the oxidation process and one the reduction process.
