Collision theory homework
Collision theory is a special type of kinetic theory that states that for a chemical reaction to take place there must be a collision between reactants. In addition, to cause a reaction the colliding reactant molecules must surpass a minimum energy termed the activation energy and, in many cases, the reactant molecules must have a certain spatial orientation with respect to each other. The collision theory provides an explanation for the experimental observation that, in a chemical reaction, if two types of molecules in the gas phase are combined, not all of the molecules instantly enter the reaction. Reactions between molecules can occur in the solid, liquid, or gaseous state. Reactions also occur in solution. The simplest reactions are those which occur between molecules in the gas phase.
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Click here to read about Ms. This semester we will used Google Classroom to organize daily work, homework and assignments. Please go to the class Google Classroom site for updates. Some of you will be able to start your titration of unknown. Your analysis report is due on Wednesday individual. See Unit outline f or overview.
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12: Kinetics (Exercises)
First, a general reaction rate must be defined to know what any variation of a rate is. The reaction rate is defined as the measure of the change in concentration of the reactants or products per unit time. The rate of a chemical reaction is not a constant and rather changes continuously, and can be influenced by temperature. Rate of a reaction can be defined as the disappearance of any reactant or appearance of any product.
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