Redox reactions Flashcards

1
Q

Oxidising agent

A
  1. accepts electrons from another reagent
  2. is reduced
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2
Q

Reducing agent

A
  1. gives electrons to another reagent
  2. is oxidised
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3
Q

Draw an electrochemical cell

A
  1. salt bridge
  2. high resistance voltmeter
  3. metal electrodes
  4. aqueous solution (1moldm^-3)
  5. standard conditions 298K, 100KPa
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4
Q

Negative standard electrode potential

A
  1. produces more electrons
  2. oxidised
  3. stronger reducing agent
  4. equilibrium shifts to the left
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5
Q

Standard electrode potential

A
  1. the potential difference of a cell
  2. when the electrode is connected to the standard hydrogen electrode
  3. under standard conditions
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6
Q

Draw the standard hydrogen electrode

A
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7
Q

Cell voltage formula

A

right E- left E

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8
Q

Affect of concentration on electrode potential

A
  1. equilibrium will shift to counteract the change
  2. changes concentration of electrons
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9
Q

Feasibility of reaction

A
  1. must have positive cell potential
  2. rate of reaction has no effect
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10
Q

Lithium half cell battery advantage

A
  1. low density
  2. high reactivity
  3. high electrode potential
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11
Q

Lithium half cell battery disadvantage

A
  1. toxic
  2. fire risk- high reactivity
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12
Q

Fuel cell

A
  1. energy from reaction of fuel with oxyegn
  2. fuel- hydrocarbon, hydrogen or alcohol
  3. creates a voltage
  4. acidic or alkaline solution
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13
Q

Advantage of fuel cell

A
  1. greater efficiency
  2. only H2O formed- not polluting
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14
Q

Disadvantage of fuel cell

A
  1. H2 difficult to store
  2. H2 difficult to manufacture initially
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15
Q

Positive standard electrode potential

A
  1. gains electrons
  2. reduced
  3. stronger oxidising agent
  4. equilibrium shifts to the right
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16
Q

Potassium manganate titration

A
  1. manganate MnO4- is oxidising agent
  2. reduced to Mn^2+
  3. Fe^2+ is reducing agent
  4. oxidised to Fe^3+
  5. turns from purple to pink
17
Q

Acid in KMnO4

A
  1. dilute sulfuric acid
  2. doesnt oxidise
  3. doesnt react with manganate ions
18
Q

Iodine-thiosulfate titration

A
  1. S2O3^2- is reducing agent
  2. oxidised to S4O6^2-
  3. I2 is oxidising agent
  4. reduced to I-
19
Q

Iodine-thiosulfate indicator

A

yellow to blue-black