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WorksheetsGCPS Kinetics
Total questions: 21
Worksheet time: 17mins
In the chemical reaction, the successful formation of products depends on the following factors EXCEPT:
The collisions between reacting molecules must be effective
The colliding molecules must approach each other in the right orientation
The energy of colliding molecules must be equal to or more than activation energy
A collision between molecules must produce sufficient energy to overcome the activation energy
The catalyst alters the rate of a chemical reaction by,
providing an alternative pathway with a lower Ea
changing the products formed in the direction of the reaction
providing a surface on which the molecules react
increasing the frequencies of collisions between molecules
The ____________ states that atoms, ions, or molecules must collide in order to react.
transition state
activation energy
rate law
collision theory
Liz observes 2 reactions, A and B.
Reaction A is performed in a beaker placed on top of a hotplate.
Reaction B is is performed in a beaker placed within a container of ice.
Which of the following statements is true?
Reaction A will react slower because the higher temperature will cause more collisions because the heat makes the molecules tired.
Reaction A will react slower because the higher temperature will cause give the reactants higher speed and kinetic energy.
Reaction B will react faster because the lower temperature causes the particles to move slower, allowing them to have more time to attach to one another.
Reaction B will react slower because the lower temperature makes the particles move slower, resulting in less collisions.
Which of the following best describes why increasing temperature increase reaction rate?
Activation energy is reduced.
Collisions become more frequent.
Collisions become more energetic.
Collisions become more frequent and more energetic.
To measure rate of reaction, we can monitor the concentration change in which of the following?
Reactants only
Products only
Reactants or products
What is the best definition of rate of reaction?
The time it takes to use up all the reactants
The rate at which all the reactants are used up
The change in concentration of a reactant/product per unit time
The time it takes for one of the reactants to be used up
The question below is about the Maxwell–Boltzmann distribution shown for a sample of a gas, X, at two different temperatures.
Which statement is correct for the higher temperature?
The area under the curve to the left of Ea decreases.
The total area under the curve increases.
The activation energy decreases.
More molecules have the mean energy.
This question is about the Maxwell–Boltzmann distribution of molecular energies in a sample of a gas shown in the figure below.
What does the area under the curve represent?
The total energy of the particles.
The total number of particles.
The number of particles that can react with each other.
The total number of particles that have activation energy.
The graph below shows a typical energy distribution for particles of an ideal gas in a sealed container at a fixed temperature.
Which of the following statements is true?
Position A represents the mean energy of a molecule in the container.
Addition of a catalyst moves the position of EA to the right.
The area under the curve to the right of EA represents the number of molecules with enough energy to react.
The position of the peak of the curve at a higher temperature is further away from both axes.
The graph shows the Maxwell−Boltzmann distribution of molecular energies in a sample of gas at a fixed temperature.
The horizontal axis label is
energy
J mol−1
E
mean energy
If the reactant particles collide with less than the activation energy, the particles will be rebound, and no reaction will occur. (BONUS)
True
False
The diagram represents the Maxwell‒Boltzmann energy distribution curve of the reactants for a chemical reaction with different activation energies, Ea1 and Ea2.
What is the reason why the rate of the reaction with activation energy Ea2 is greater?
More frequent collisions between the particles occur.
More energetic collisions between the particles occur.
A catalyst has been added.
The temperature is higher.
