Practice Collision theory with authentic MYP MYP Chemistry exam questions for both SL and HL students. This question bank mirrors Paper 1, 2, 3 structure, covering key topics like atomic structure, chemical reactions, and organic chemistry. Get instant solutions, detailed explanations, and build exam confidence with questions in the style of MYP examiners.
According to the collision theory, which of the following conditions must be met for a collision between two reactant molecules to result in a reaction?
Activation energy () is defined as the __________ energy required for a collision to result in a chemical reaction.
According to collision theory, why is the correct orientation of particles an essential condition for a successful collision between molecules?
Consider the following statement:
"Increasing the temperature of a reaction mixture provides particles with more energy, thereby lowering the activation energy () required for the reaction."
Is this statement correct?
Why must the activation energy () be overcome even in an exothermic reaction where the products are more stable than the reactants?
When the pressure of a gas-phase reaction is increased by reducing the volume of the container, what happens to the particles on a molecular level?
A small increase in temperature can lead to a large increase in reaction rate. This is primarily because:
Increasing the concentration of a solution affects the reaction rate. Which of the following properties of the system does NOT change when concentration is increased at a constant temperature?
According to collision theory, which of the following combinations would describe a reaction that is likely to be very slow?
A reaction with a very high activation energy () is likely to be:
Practice Collision theory with authentic MYP MYP Chemistry exam questions for both SL and HL students. This question bank mirrors Paper 1, 2, 3 structure, covering key topics like atomic structure, chemical reactions, and organic chemistry. Get instant solutions, detailed explanations, and build exam confidence with questions in the style of MYP examiners.
According to the collision theory, which of the following conditions must be met for a collision between two reactant molecules to result in a reaction?
Activation energy () is defined as the __________ energy required for a collision to result in a chemical reaction.
According to collision theory, why is the correct orientation of particles an essential condition for a successful collision between molecules?
Consider the following statement:
"Increasing the temperature of a reaction mixture provides particles with more energy, thereby lowering the activation energy () required for the reaction."
Is this statement correct?
Why must the activation energy () be overcome even in an exothermic reaction where the products are more stable than the reactants?
When the pressure of a gas-phase reaction is increased by reducing the volume of the container, what happens to the particles on a molecular level?
A small increase in temperature can lead to a large increase in reaction rate. This is primarily because:
Increasing the concentration of a solution affects the reaction rate. Which of the following properties of the system does NOT change when concentration is increased at a constant temperature?
According to collision theory, which of the following combinations would describe a reaction that is likely to be very slow?
A reaction with a very high activation energy () is likely to be: