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Chemistry > Midterm review- Kinetics/Energetics > Flashcards

Midterm review- Kinetics/Energetics Flashcards

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1
Q

Exothermic Reaction: Chemicals gain or lose enthalpy

A

Lose enthalpy

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2
Q

Exothermic: Heat energy lost or gained?

A

Lost

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3
Q

Exothermic: Surrounding temperature?

A

Hotter

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4
Q

Exothermic: Delta H?

A

Negative

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5
Q

Exothermic: Reactants or Products?

A

H of reactants > H of products

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6
Q

Endothermic: Gain or lose enthalpy?

A

Gain

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7
Q

Endothermic: Heat energy lost of gained?

A

Gained

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8
Q

Endothermic: surrounding temperature?

A

Colder

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9
Q

Endothermic: Delta H?

A

Positive

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10
Q

Endothermic: Reactants or Products?

A

H of products > H of reactants

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11
Q

Spontaneous Reactions

A

Occur without heating when mixing reagents

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12
Q

Enthalpy (H)

A

energy contained in chemical bonds that can be converted into heat

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13
Q

Factors affecting enthalpy

A

value of deltaH, concentration of reactants, states of reactants and products, temperature of reactions, pressure of reaction

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14
Q

Ways to find enthalpy change

A

Hess’s law, bond enthalpies, and delta Hs of formations

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15
Q

Bond enthalpies

A

(Sum of BEs of reactants) minus (Sum of BEs of products)

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16
Q

Delta Hs of formations

A

(Sum of Delta Hs of products) minus (Sum of Delta Hs of reactants)

Multiply by coefficients
Elements in standard state = 0

17
Q

Ways to measure Reaction Rates

A
  • Mass or volume changes for gaseous reactions
  • Change in pH for acid/base reactions
  • Change in conductivity for electrolytes
  • Use of spectrometer for color change reactions
18
Q

Collision Theory must…

A

…take place for reactions to occur

19
Q

3 Parts of Collision Theory

A
  • The two particles must collide
  • The two particles must collide so that the reactive parts hit
  • The reactive parts must hit with sufficient energy (activation energy)
20
Q

Activation Energy

A

minimum amount of energy required to bring about a reaction

21
Q

Factors affecting Reaction Rates

A
  • Temperature: increases frequency of collisions
  • Catalyst: lowers activation energy
  • Surface Area of reactants: increases chances of collisions
  • Concentration of reactants: increases amount of collisions

Chemistry (11 decks)

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