CHEM 135 1st Edition Lecture 12Outline of Last Lecture I. Integrated Rate Lawa. Graphsb. Equationsc. ExamplesII. Half lifea. Equationsb. ExamplesOutline of Current Lecture I. Factors affecting the rate of a reactiona. Concentration b. Temperaturec. Surface areaII. Demo observationsa. Glow sticksb. Blue solution c. Corn starchCurrent LectureFactors affecting the rate of a reaction1. Concentration- If there is an increase in the concentration, there is an increase in the frequency of collisions2. Temperature- If there is an increase in temperature, the frequency of collisions also increase3. Surface areaThese notes represent a detailed interpretation of the professor’s lecture. GradeBuddy is best used as a supplement to your own notes, not as a substitute.Among the colliding molecules, only effective collisions, i.e. collisions in right orientation and with right energy can lead to product formation.Frequent collisions raise the rate of the reaction Collisions need sufficient energy to break reactant bondsDEMO:Glow stick- Has two chemicals, separate at first when the glow stick is bent, the chemicals react resulting in the glow- One glow stick is placed into an ice bath, the other is placed into hot water- After a certain amount of time, the glow sticks are observedo Ice bath glow stick has a low intensity glowo Hot water glow stick has a high intensity glowBlue solution - There are four beakers containing a blue solutiono Control beaker, +5mL bleach at room temperature, +25mL bleach at room temperature, +5mL bleach less than room temperature - 25mL of bleach causes the blue color to dissipate - Higher temperature and 5mL of bleach causes for the color to disappear- 5mL/ room temperature has color for the longestCornstarch- Cornstarch in petri dish and was held under flame, did not catch fire- Cornstarch was placed into a turkey baster and released in front of a propane torch, resulted in a LARGE