CHEM 154 Lecture Notes - Lecture 24: Reactive Intermediate, Toothpaste, Hydrogen Peroxide
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The half-life of a reactant is the time it takes for its concentration to fall to one-half of its original values. Do worksheet question #4: chemical reactions: a molecular view. In order for a reaction to occur, collisions between molecules must have: As temperature increases, more collisions between reactants have the energy necessary for reaction to occur: activation energy (ea) Minimum energy that reactant molecules must possess to undergo a particular chemical reaction: collision geometry. Some collision may have enough energy but not the right orientation: arrhenius behaviour. The arrhenius equation describes the relationship between the rate constant (k) and temperature (t). k=ae -ea/rt lnk = -e a /r x (1/t) + lna. A is called the frequency factor: reaction mechanisms. A reaction mechanism is a collection of one or more molecular steps that account for the way reactants become products. [ no2(g) + no2(g) no3(g) +no(g) ] + [ no3(g) + cp(g) no2(g) + co2(g) ] =
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