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Electrochemistry

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  • In galvanic cells, what produces electricity?
    Chemical changes
  • Without electrolysis, it would be possible to produce many of the materials and products that we use today.
    False
  • Rusting
    The corrosion of iron and steel is called rusting
  • Which of the following when dissolved in water and placed in the conductivity apparatus would cause the light to glow?
    Sugar (C12H22O11)
    Glycerine (C3H8O3)
    Ethyl alchol (C2H5OH)
    Table Salt (NaCl)
  • is another version of a primary cell. It also uses zinc and manganese oxide as reactants, but under basic conditions.
    Alkaline Dry Cel
  • product of galvanisation
    Galvanized iron
  • is the gains of electrons by a substance
    Reduction
  • The useful metal is oxidized to create a metal oxide
    Anodising
  • it will be positive in Voltaic cell but in Electrolytic is Negative
    E• cell
  • The process of covering iron or steel objects with a layer of metal in order to stop the original product from corrosion.
    Metal Plating
  • The positive electrode connected to the positive terminal of the d.c. power source
    Anode
  • The surface of an is covered with layer of substance. The layer stops air and water from reaching the iron and steel underneath.
    Surface Protection
  • Electro
    Electrical
  • more positive standard electrode potential
    cathode
  • is the ddecomposition of compound by the use of electricity
    Electrolysis
  • describes the process that happen by itself
    Spontaneous
  • is an ionic compound which, conducts an electric current in the process
    Electrolyte
  • is covered with a layer of substance
    Surface protection
  • the process of covering iron or steel with a protective layer of zinc metal
    Galvanization
  • Ionic compounds will conduct an electric current when they are
    Dehydrated
    Melted
    Solidified
    Frozen
  • is the charge an atom would have if it existed as an ion
    Oxidation state(number)
  • With electrolysis, it would be possible to produce many of the materials and products that we use today.
    True
  • a part of a Galvanic cell in which either oxidation or reduction can happen
    A half-cell
  • a type of Galvanic cell that comprises of two half-cells which undergo the same half-reaction, but have different electrolyte concentrations.
    Concentration Cells
  • is an ionic compound which, conducts an electric current in the process
    Electrolyte
  • anode
    the more negative standard electrode potential
  • is a non-rechargeable cell which irreversible converts chemical energy to electrical energy.
    Primary cells
  • Galvanization
    is the process of covering iron or steel with a protective layer of zinc metal.
  • 27. What is the scientific name for rust and its chemical formula?
    Iron (II) Oxide FeO *xH2O
  • is an alloy of iron containing chromium or nickel
    Stainless steel
  • The coating of an object with a thin layer of a metal by eletrolysis
    Electroplating
  • What does “electro-” mean?
    movement of electrons / electricity
  • Cathode
    more positive standard electrode potential
  • Iron at the beach rusts faster than iron in the mountain.
    True
  • are used to produce electricity
    Chemical changes
  • What is shelf life?
    Storage life
  • What does “lysis” mean?
    to cut or to break
  • is the decomposition of compound by the use of electricity
    Electrolysis
  • is the process of covering iron or steel with a protective layer of zinc metal.
    Galvanization
  • more positive standard electrode potential
    anode
  • In electrolytic cells, what produces chemical changes?
    A battery
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