Topic 7- Rates Flashcards

1
Q

Exothermic Reaction

A
  • Gives out energy
  • Gives out heat
  • Shown by a rise in temperature
  • Mexo
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2
Q

Endothermic Reaction

A
  • Takes in energy
  • Takes in heat
  • Fall in surrounding temperature
  • Bendo
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3
Q

Activation Energy

A

The amount of energy required to start a reaction

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4
Q

Reaction Profiles

A

Show the starting energy of the reactants and the end energy of the products
Exothermic : Reactants higher than products
Endothermic : Products higher than reactants

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5
Q

Catalyst

A
  • Increase the rate of a reaction
  • Is not chemically changed in a reaction
  • Will not change the products
  • Provides an alternative reaction pathway
  • Increase the rate of a reaction
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6
Q

Enzymes

A
  • Biological Catlysts
  • Speeee up chemical reactions in living cells
  • Used in protein synthesis, respiration and photosynthesis
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7
Q

Rate of Reaction

A

How fast a reaction occurs. Can be worked by when all the reactants are used up or how quickly the products formed.

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8
Q

How to work out rate of reaction

A

Amount of reactant used or product formed over time

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9
Q

Precipitation experiment to measure rates

A
  • Mixing two see through reactions forms a precipitate which clouds the solution
  • Mix the two solutions on a piece of paper with an X on it
  • Observe the mark until it can no longer be seen as it clouds
  • The faster it disappears, the faster the rate
  • This is subjective
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10
Q

Changes in mass to measure rates

A
  • Gas needs to be measured using a mass balance
  • As gas is released, lost mass is easily measured using the mass balance
  • The quicker the drop, the faster the reaction
  • ## The reaction bas finished when the balance stops changing
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11
Q

Gas Syringe

A
  • Shows the volume of gas given off
  • The more gas given off, the faster the reaction
  • When no more gas is given off, the reaction has finished
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12
Q

Surface area rate

A
  • Use an experiment using HCl and marble chips
  • Measure the volume of gas produced using a gas syringe
  • Take regular time readings
  • Repeat the experiment with same mass of chips but different surface areas
  • The larger the surface area, the quicker the reaction
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13
Q

Rates on a graph

A
  • When the mass/volume produced reaches a constant, the reacton will have finished
  • The steeper the gradient, the faster the reaction
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14
Q

Affect of concentration on rates

A
  • The higher the concentration, the faster the rate

- Same effect as surface area

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15
Q

How temperature effects rates

A
  • The rate can be measured by the reaction of hcl and Sodium Thiosulfate
  • Both clear and when reacted from a yellow precipitate and sulfur
  • Measure the amount of time it takes for the precipiate to form
  • Use the X from the precipitation
  • Use a water bath to heat the solution and maintain a constant
  • Change the temperature to measure the time difference
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16
Q

Effect of temperature on rates

A

The highter the temperature, the higher the rate

The molecules have more energy and move around faster increasing the chances of successful collisons

17
Q

Calculating rates

A
  • Faster rates of reactions are shown by steeper gradients

- Gradient = Change in Y divided by change in x

18
Q

Gradient of a curve

A
  • At different points on a curve, the gradient will be different
  • Draw a tangent at a certain point
  • A tangent has the same gradient as the point
  • Use the tangent as the gradient
19
Q

Collision Theory

A
  • Particles must collide with a certain amount of energy to react
  • The more successful collisons, the faster the reaction
  • These particles must have more than the activation energy to start the required reaction
20
Q

Factors affecting rates

A
  • Catalyst - Lowers activation energy
  • Surfacee Area - More area to react
  • Concentration- More reactants in a given volume
  • Temperature - gives the molecules more energy to move around faster and create more successful reactions
21
Q

Measuring temperature changes

A
  • The change can be measured
  • Put a polystyrene cup in a beaker with cotton wool for insulation to limit energy lost
  • Add the first reagent and measure the intial temperature
  • Add the second reagent
  • Put a lid on the beaker to limit energy lost in evaporation
  • Record the maximum and minimum temperature and then calculate the change
22
Q

Bond Energies

A
  • Energy must always be supplied to break bonds
  • Endothermic produces a strong bond being broken whilst exothermic is opposite
  • Exothermic releases energy and endothermic consumes energy
23
Q

How to work out energy change

A

Energy required to break bonds - Energy released by bonds

Positive value means endothermic
Negative value means exothermic

Values will always be given in papers if needed