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20 Terms

1
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Collision theory

  • Proper orientation

  • Collision

  • Sufficient energy to overcome repulsive forces and break the bonds (activation energy)

2
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What is the cause behind unsuccessful collisions?

Particles don’t have sufficient energy

3
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Define activation energy

Minimum energy required for colliding particles to react

4
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Rate of dissociaciation

  • negative
  • change in concentration of reactants / change in time
  • mol dm-3 s-1
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Rate of formation

  • positive
  • change in product concentration/ change in time
  • mol dm-3 s-1
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When can you use a colorimeter to measure rate?

If the solution changes color

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How to measure rate of reaction for gas in an open system?

Change in mass/Change in time

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How can volume be used to measure rate?

  • gas syringe, inverted measuring cylinder
  • Gas production is measure in a closed system
  • Change in volume/Change in time
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Exothermic reactions

  • Reactants are higher than products
  • Higher Ea than endothermic reactions
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Endo thermic reactions

  • Products are higher than reactants
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Where is transition state on a graph and what does it indicate?

  • Highest energy peak
  • Simultaneous breaking and forming of bonds
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Where is the activation energy on a graph?

The distance between reactants and the transition state

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What is the effect of a catalyst on activation energy?

  • provide an alternative reaction pathway with lower Ea
  • increases frequency of proper collision
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What is the effect of increasing concentration on reactions?

  • more particles in set volume = higher collision frequency, higher rate
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What is the effect of increasing pressure on reactions?

  • gases
  • less space = increased collision frequency = higher rate
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What is the effect of increasing temperature on reactions?

  • higher velocity = higher frequency of collisions = higher rate
  • higher proportion with Ea = higher proportion of successful collisions = higher rate
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What is the effect of size on rate of reaction?

  • smaller size = higher SA = more particles able to collide = higher frequency of successful collisions = higher rate
  • solids
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What does Maxwell-Boltzmann curve show?

distribution of kinetic energy at a certain temperature

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Effect of increasing temperature on Maxwell-Boltzmann curve

  • Curve flattens
  • peak shifts to the right
  • right line goes over the original curve
  • higher proportion of molecules at or beyond Ea
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Effect of catalyst on Maxwewll-Boltzmann curve

  • curve doesn’t shift
  • line indicating molecules with Ea shifts to the left