Topic 6 - Rate And Extent Of Chemical Change Flashcards

1
Q

What is the collision theory

A

In order for a chemical reaction to happen reactant particles must collide with each other and the particles must have enough energy for them to react

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2
Q

What’s a successful collision

A

A collision that produces a reaction

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3
Q

What is activation energy

A

The minimum amount of energy needed for a collision to be successful

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4
Q

What’s the equation for mean rate of reaction

A

Quantity of reactant used or product formed ÷ time taken

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5
Q

What are other ways to determine the rate of reaction

A

Measuring mass (when a gas is produced), measuring volume (useful when a gas is produced, using a gas syringe etc)

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6
Q

What happens when the concentration of a reacting solution or the pressure of a reacting gas is increased

A
  • the reactant particles become more crowded
  • the frequency of collisions between reactant particles increases
  • the rate of reaction increases
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7
Q

What happens when the surface area to volume ratio of the reactant increases

A
  • more reactant particles are exposed at the surface
  • the frequency of collisions between reactant particles increases
  • the rate of reaction increases
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8
Q

How do you increase the surface area to volume ratio

A

Break a large lump into smaller chunks or grind it into a powder

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9
Q

What would happen if the temperature of the reaction mixture is increased

A
  • reactant particles move more quickly
  • the energy of the particles increases
  • the proportion of collisions which are successful increases
  • the rate of reaction increases
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10
Q

What is a catalyst

A

A substance that increases the rate of reaction, does not alter the products of the reaction, and is not used up at then end of the reaction

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11
Q

How do catalysts work

A

They provide an alternative reaction pathway that has a lower activation energy

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12
Q

What happens if you add a catalyst to a reaction

A
  • it increases the frequency of successful collisions as more particles have energy greater than the activation energy
  • rate of reaction increases
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13
Q

What’s a reversible reaction

A

The products of the reaction can react together to produce the original reactants . The same amount of energy is transferred in both the forward and backward reaction but one direction will be endothermic and the other exothermic

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14
Q

What is dynamic equlibrium

A

The forwards and backwards reactions are still happening, they have the same rate of reaction, the concentrations of all the reacting substances remain constant. This haplend when a reversible reaction happens in a closed container.

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15
Q

What is Le Chatelier’s principle

A

The equilibrium can be changed by changing the reacting conditions through either changing the concentration, pressure, or temperature

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