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Kinetics key terms
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key terms
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Topic
Kinetics
Key terms
Activation Energy
The minimum energy required for a chemical reaction to occur.
Arrhenius Equation
An equation that expresses the relationship between the rate constant of a reaction and temperature, incorporating activation energy.
Effective collision
A collision between reactant molecules that results in a reaction due to sufficient energy and proper orientation.
Rate of reaction
The change in concentration of reactants or products per unit time.
Collision frequency
The number of collisions that occur per unit time in a given volume of reactants.
Reaction rate
The speed at which reactants are converted into products in a chemical reaction.
Temperature
A measure of the average kinetic energy of the particles in a substance, typically measured in Kelvin (K).
Distribution Curve
A graphical representation of the distribution of a variable, such as molecular speeds, showing the frequency of different energy levels.
Kinetic Energy
The energy possessed by an object due to its motion, directly related to the temperature of a substance.
Collision Theory
A theory that states that for a reaction to occur, reactant particles must collide with sufficient energy and proper orientation.
Activation Energy
The minimum energy that must be overcome for a reaction to occur.
Maxwell-Boltzmann Distribution
A statistical distribution of the energies of particles in a gas, illustrating the spread of molecular speeds.
Kinetic Energy
The energy that a body possesses due to its motion, which is directly related to temperature.
Collision Theory
A theory that states that for a reaction to occur, reactant particles must collide with sufficient energy and proper orientation.
Collision Frequency
The number of collisions that occur per unit time between reactant particles in a chemical reaction.
Effective Collision
A collision between reactant particles that results in a chemical reaction, requiring sufficient energy and proper orientation.
Reaction Rate
The speed at which reactants are converted into products in a chemical reaction, often measured in terms of concentration change over time.
Pressure
The force exerted by gas molecules per unit area, which can influence the concentration of gases in a reaction.
Activation Energy
The minimum energy required for a chemical reaction to occur.
Catalyst
A substance that increases the rate of a reaction by providing an alternative pathway with a lower activation energy.
Rate of reaction
The change in concentration of a reactant or product per unit time.
Catalyst
A substance that increases the rate of a reaction without being consumed in the process.
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