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Worksheets7.4 Collision Theory
Total questions: 15
Worksheet time: 8mins
What describes a reaction?
Products react and become reactants.
Reactants react and become products.
Reactants and products react and become new reactants.
Reactants and products react and become new products.
Collision theory states that
particles collide at random and react
collisions between particles often result in a reaction
collision between molecules are sometimes needed before a reaction occurs
reacting particles must collide with enough energy in order to reac
What criteria must be met for reactant collisions to result in a successful product?
The reactants must collide with each other only
The reactants must collide with enough energy and be in the right positions
The reactants must have enough energy to form the activated complex
The reactants must collide with enough energy only
Reactions in which the products have more energy than the reactants are_______ reactions.
Endothermic
Exothermic
Redox reaction
Elimination
Increase in temperature of the reactants can do one of the following
Slow collision frequency
Allow less effective collision between the particles
Neutralise the reaction
Increase collision between the particles thus increasing the rate.
Why does a catalyst increase the rate of reaction?
it produces extra energy for the reactants
it increases the speed of the reactant particles
it increases the frequency of particle collisions
it reduces the activation energy of the reaction
Why don't all collisions between particles cause a reaction?
The particles also need to collide with a catalyst
Not all the particles collide with enough energy
Not all the particles collide at a high enough temperature
The particles need to collide with each other twice
Which of the following is/are the fundamental idea(s) of collision theory?
Molecules react by colliding together
The effective collisions must occur with certain minimum amounts of energy
In a large sample, the greater the number of effective collisions, and the faster the rate of reaction
All of the above
Under the collision theory, the particles must collide with ____ and ____ for a reaction to occur.
sufficient rate and sufficient energy
sufficient surface area and correct orientation
sufficient catalyst and sufficient energy
sufficent energy and correct orientation
What is activation energy?
Energy barrier that does not need to be overcome before a reaction can take place.
Maximum energy required to break the bonds and form new bonds.
Minimum energy required to break the bonds in reactant particles
Energy required to end a reaction
What factors are required for successful collisions?
collision of particles
sufficient energy
favorable orientation
all of these
If two reactants collided with energy but no reaction occurred, what would the most like explanation be?
The collision was too soft
The colliding particles were in the incorrect orientation
The colliding particles were in the correct orientation
The colliding particles were too big
A catalyst increases the rate of a chemical reaction by
decreasing potential energy of the reactants
increasing potential energy of the reactants
decreasing activation energy
increasing activation energy
When the concentration of reactants increases, the rate of reaction increases.
Which of the following explains the statement?
The activation energy of the reaction increases.
It provides an alternative reaction pathway.
The kinetic energy of the reactant particles increases.
The number of reactant particles per unit volume increases.
B represents
energy absorbed
energy released
activation energy
net energy released
