Rates Of Reaction Flashcards

1
Q

The rate of chemical reaction

A

How fast the reactants are changed into products.

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2
Q

Slow reactions

A
  • rusting of iron

- chemical weathering-acid rains damage to limestone buildings

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3
Q

Moderate reactions

A

Magnesium with acid

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4
Q

Fast reactions

A
  • burning

- explosion

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5
Q

Factors affecting rates of reaction

A
  • temperature
  • concentration of the solution or the pressure of gas
  • surface area
  • use of catalyst
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6
Q

The rate of reaction depends…

A

On the frequency of successful collisions.

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7
Q

Temperature increases the rate

A

Particles move faster, they are going to collide more frequently

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8
Q

A formula for a rate of reaction (reactant)

A

rate = amount of reactant / time

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9
Q

A formula for a rate of reaction (product)

A

rate = amount of product / time

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10
Q

The steeper the gradient of a line on the graph is…

A

the faster the reaction is.

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11
Q

How can you measure the rate of reaction in experiments?

A
  • measuring the decreasing mass of a reaction mixture
  • measuring the increasing volume of gas given off
  • measuring the decreasing light passing through a solution( decrease is caused by precipitate)
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12
Q

Collision theory

A

Chemical reactions can only occur when reacting particles collide with each other and with sufficient amount of energy.

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13
Q

Activation energy

A

The minimum amount of energy that particles must have to react.

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14
Q

Increasing pressure of a gas or concentration of a solution

A

Increase the

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15
Q

Reactions are rapid, initially…

A

because we have a large number of reactant molecules. So we have a large number of collision per second.

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16
Q

Over time reactions…

A

slow down because the number of reactant molecules is running out. So smaller number of collisions per second.

17
Q

The reaction stops when…

A

all the reactant molecules have run out, so the number of collisions per second is 0.

18
Q

How does concentration/ pressure affect the rate?

A

The higher the concentration or pressure, the more reactant particles are available and so the frequency of successful collision is higher.

19
Q

How does surface area affect the rate?

A

The greater the surface area, the more particles can react with the solution/gas, so the frequency of collisions increases. The solution cannot react with particles which are not on the surface.