true or false
Collision theory states that a chemical reaction occurs when particles collide with insufficient energy.
false
Explain collision theory in the context of chemical reactions, providing an example from real life.
Collision theory proposes that chemical reactions happen when particles of the reactants collide with sufficient energy. For instance, the combustion of gasoline in a car engine exemplifies collision theory, where gasoline molecules collide with oxygen molecules with enough energy to initiate the reaction, producing carbon dioxide, water vapor, and heat.
What is the term for the theory that explains a chemical reaction occurring when reactant particles collide with sufficient energy?
Collision theory
An increase in concentration of reactants leads to a decrease in the speed of a chemical reaction.
false
An increase in temperature decreases the rate of a chemical reaction because it lowers the activation energy required for the reaction to occur.
false
Define the term "activation energy" in the context of chemical reactions.
Activation energy represents the minimum energy required for a chemical reaction to occur. It is the energy threshold that reactant particles must surpass during collisions to form products.
Activation energy is the energy required for reactant particles to overcome the energy barrier and transform into product molecules during a chemical reaction, with the activation energy representing the minimum energy necessary for this transformation.
true
Activation energy is a fixed value for each reaction, meaning that all collisions between reactant particles must surpass this threshold energy for the reaction to occur.
false
Explain the concept of collision theory in the context of chemical reactions, using an example from everyday life.
Collision theory posits that chemical reactions occur when particles collide with sufficient energy. For instance, in the combustion of gasoline in a car engine, gasoline molecules must collide with oxygen molecules with enough energy to initiate the reaction, producing carbon dioxide, water vapor, and heat.
A catalyst increases the rate of a chemical reaction by providing an alternative reaction pathway with higher activation energy.
false
Describe the concept of activation energy in chemistry and its role in chemical reactions.
Activation energy represents the minimum energy required for a chemical reaction to occur. When particles collide, they must have combined energy greater than the activation energy to initiate the reaction. Otherwise, the reaction won't proceed.
What does it mean when it is stated that a catalyst provides an alternative reaction pathway with lower activation energy?
A catalyst provides an alternative reaction pathway with lower activation energy by facilitating the formation of temporary intermediate species. This lowers the energy barrier required for the reaction to occur, thereby increasing the reaction rate.
Activation energy is the energy required for a chemical reaction to occur, and if the colliding particles have energy greater than this threshold, they will react.
true
Activation energy represents the total energy released during a chemical reaction.
false
Describe how the concentration of reactants influences the rate of a chemical reaction, based on collision theory principles.
According to collision theory, an increase in the concentration of reactants leads to more frequent collisions between reactant particles. This increases the likelihood of successful collisions, resulting in a higher reaction rate.