Lesson 3.1.5.1
3.1.5.1 Collision theory Quiz: AQA Chemistry, Unit 1
20 questions
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Lesson 3.1.5.1, Collision theory: 20 multiple choice questions for the AQA Chemistry (7405), Unit 1: Physical chemistry, written with Revision Ninja.
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The 20 questions
-
What is defined as the minimum energy required for colliding particles to react?
- Bond enthalpy
- Activation energy
- Lattice energy
- Reaction enthalpy
-
Why do most particle collisions fail to produce a chemical reaction?
- High particle speed
- Presence of catalyst
- Incorrect reaction enthalpy
- Insufficient collision energy
-
According to collision theory, what must occur for a reaction to happen?
- Phase changes
- Thermal equilibrium
- Complete bond dissociation
- Energetic particle collisions
-
On a reaction profile diagram, activation energy is measured from reactants to where?
- Product level
- Peak of curve
- Origin of axes
- Enthalpy change
-
What happens to the activation energy when a catalyst is added?
- It is unchanged
- It is lowered
- It is raised
- It becomes zero
-
Which particles can undergo a successful collision in a reaction?
- Sufficiently energetic particles
- Only uncharged particles
- Low energy particles
- All colliding particles
-
Besides collision frequency, what directly determines reaction rate in collision theory?
- Total reactant mass
- Activation energy value
- Container volume
- Fraction of successful collisions
-
Why does increasing temperature significantly increase the rate of reaction?
- Higher reactant concentration
- Lower activation energy
- More successful collisions
- Decreased collision frequency
-
Two reactions at equal concentrations have different rates. What causes this?
- Different volume units
- Different activation energies
- Different temperature scales
- Equal collision frequencies
-
In an exothermic reaction, how do product energy levels compare to reactants?
- Equal to reactants
- Lower than reactants
- Higher than reactants
- Double the reactants
-
A reaction has activation energy 75 kJ mol-1 and an enthalpy change of -40 kJ mol-1. How far is the top of the energy hump above the reactants?
- 40 kJ mol-1
- 35 kJ mol-1
- 115 kJ mol-1
- 75 kJ mol-1
-
What effect does a high activation energy have on reaction rate?
- Slower reaction rate
- Higher collision frequency
- No effect on rate
- Faster reaction rate
-
Besides having sufficient energy, what is needed for particles to react?
- Equal kinetic energy
- High molecular mass
- Correct collision orientation
- Opposite electrical charge
-
What would happen to the reaction rate if activation energy were zero?
- No collision occurs
- Extremely fast reaction
- Reaction would stop
- Extremely slow reaction
-
At a fixed temperature, what proportion of gas collisions exceed activation energy?
- Half
- Small fraction
- Majority
- All collisions
-
Why is a reaction faster at 50 °C than at 20 °C?
- More successful collisions
- Higher activation energy
- Lower collision frequency
- Fewer successful collisions
-
A forward reaction has Ea = 80 kJ mol-1 and delta H = -20 kJ mol-1. What is the activation energy of the reverse reaction?
- 20 kJ mol-1
- 60 kJ mol-1
- 80 kJ mol-1
- 100 kJ mol-1
-
Which factor is NOT a component of collision theory?
- Collision frequency
- Mean bond enthalpy
- Collision orientation
- Activation energy
-
Which activation energy results in the faster rate for reactions with equal collision frequency?
- 200 kJ mol-1
- 150 kJ mol-1
- 100 kJ mol-1
- 50 kJ mol-1
-
How does increasing temperature affect the activation energy of a reaction?
- Doubles
- Increases
- Unchanged
- Decreases
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