The basics
What reactions care about
rate laws
Order
Integration
100
It is the term that describes how fast or slow a reaction occurs over time.
What is a reaction rate
100
When the reactant -------- increases, then the reaction shifts to the right.
What is the concentration.
100
In a rate expression, k is referred to as this.
What is the rate constant
100
The order of a reaction show this.
What is the relationship between the participating species and the rate of a reaction.
100
These graphs are two ways to plot this type of reaction:
What are the first order reactions.
200
A reaction occurs when particles collide with sufficient energy and proper orientation.
What is according to collision theory.
200
This is an environmental factor which contributes to the increase in the rate of a reaction.
What is the temperature?
200
The rate of a reaction at a point where a tangent touches the reaction rate curve.
What is instantaneous rate?
200
The overall order of the reaction shown below:
Rate = k[KI]2[Pb(NO3)2]1
What is 3.
200
The photocatalysis of hydrogen gas and chlorine gas produces hydrogen chloride gas which can be plotted to produce a graph which follows --------------order reaction: 
What is zero order.
300
The minimum energy required for a reaction to occur
What is the Activation Energy Ea.
300
Oh! This is not consumed during a reaction, or is recreated at the end of the reaction.
What is a catalyst?
300
The reaction does not respond to the concentration of the reactants at any time during the reaction.
What is a zero order reaction?
300
The Order of a reaction as determined by taking the ratio of rates for two initial concentration is:
Rate2 /Rate 1 = k(0.0060) Ms-1/k(0.0015) Ms-1
What is two.
300
Predict the amount of reactant or product present after a period of time.
What are integrated rate laws.
400
The energy required to remove an electron from an atom or an ion.
What is an Ionization energy.
400
This is an important factor, determining how fast or slow the reaction may proceed.
What is the nature of reacting atoms and molecules; What is their electronic configuration?
400
Integrated rate laws.
What is the relationship between the reactant concentration and time.
400
True or false: Reaction order can be deduced from the balanced chemical equation of the overall reaction.
False
400
Reactions that exhibit larger rate constants and correspondingly shorter half-lives when fast; smaller rate constants with longer half-lives when slow.
What are first order reactions.
500
This is how the crystal structure is determined
What is the X-ray diffraction technique.
500
A finely divided piece of Magnesium reacts more violently with HCl than a large nugget of Magnesium.
What is due to larger available surface area?
500
In a rate law, this is typically used to determine the units of the rate constant, k.
What is the method of initial rates?
500
The expression Rate = k[A]0 informs us about an important relationship.
What is the rate is independent of the initial reactant concentration.
500
The rate constant cannot be calculated directly from the half life of this type of reactions.
What are second order reactions
600
The minimum amount of energy needed by a chemical reaction to occur in addition to the proper orientation of the molecules.
What is the energy of activation.
600
The reaction proceeds along this path on the reaction coordinate.
What is the lowest energy path.
600
This picture explains the rate of reaction.
What is the collision theory.
600
Radiocarbondating is based on the fact that C14 decay follows a certain kinetics order.
What is the first order kinetics.
600
For this type of reactions, as the concentration of reactants decreases, the half-life increases.
What are the second order reactions.