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1 Science 10: Chemistry! Factors Affecting Reaction Rates (Textbook Chapter 94) Rate of reaction or reaction rate is how quickly or slowly reactants turn into products reaction rate = A slow reaction has a reaction rate A fast reaction has a reaction rate Example: Example: A rusting bicycle chain, which is the oxidation of iron Burning wood, which is combustion of a hydrocarbon Every chemical reaction proceeds at a definite rate, but we can speed up or slow down a reaction rate *Side note Kinetic Molecular Theory (KMT) The kinetic molecular theory explains that particles in matter are in constant motion These particles move constantly in random directions Kinetic energy is the energy of a particle or an object due to its motion When particles collide, energy is transferred between them There are four main factors that affect the movement of the particles and therefore the reaction rate TEMPERATURE Temperature is a measure of the temperature in a substance the temperature Example: How do you change the reaction rate of food breaking down into smaller components? Reactant particles move, which causes between particles and more energy and an increase in reaction rate Reactant particles move, which causes between particles and less energy and a decrease in reaction rate 1

2 EXPERIMENT - temperature Given the following materials and method, formulate a testable hypothesis to quantitatively show how a cold, medium and hot temperature will affect the reaction rate Hypothesis: (Write an If then because statement) Two 400 ml beakers Thermometer Ice water Hot water 3 Alka Seltzer tablets Stopwatch Method: 1 Fill one beaker with ice water Fill the second beaker with very hot water Use a thermometer to measure the temperature in each beaker Record the temperatures 2 Drop an effervescent tablet into each beaker at the same time Observe Use a stopwatch to measure how many seconds it takes for each tablet to finish dissolving Record the times Dispose of beaker contents down the sink 3 Fill one of the beakers with a mixture of hot water and ice water Adjust the temperature by adding more warm or cool water until the temperature is halfway between the temperatures recorded in step 1 4 Make a prediction of the length of time it will take for an effervescent tablet to finish dissolving Record your prediction 5 Add a tablet to the water that is at a middle temperature Observe and record the time it takes to dissolve Dispose of beaker contents down the sink Data Table: Alka Seltzer tablet + hot water Alka Seltzer tablet + ice water Water Temp ( C) Mass of Tablet (g) Reaction Time (s) Reaction Rate (g/s) Prediction: How long will the tablet take to dissolve in the medium temperature water? Alka Seltzer tablet + medium water Conclusion: An in temperature caused the reaction rate to 2

3 2 CONCENTRATION Concentration is how much solute (usually solid) is dissolved in a solution (liquid) the concentration the concentration Example: At which point during the school day are you MORE likely to bump into someone? Why? A higher concentration of particles means there will be with other particles so the reaction rate increases A lower concentration of particles means there will be with other particles so the reaction rate decreases EXPERIMENT - concentration Given the following materials and method, formulate a testable hypothesis to quantitatively show how changing the concentration will affect the reaction rate Hypothesis: (Write an If then because statement) 2 small test tubes Test tube rack Method: 2 ml of concentrated (30M) hydrochloric acid 2 ml of diluted (05 M) hydrochloric acid 2 equal size small pieces of magnesium strips 1 Place the two test tubes in the test tube rack 2 Fill one test tube with dilute hydrochloric acid to a depth of about 2cm (2mL) 3 Fill the second test tube with the concentrated hydrochloric acid to a depth of about 2cm (2mL) 4 Simultaneously, place equal sized strips of magnesium in each test tube 5 Time the length of the reaction in each test tube and record your results Stop timing when there are no longer bubbles being formed in the tube and/or when the magnesium strip is no longer visible (whichever comes first) 6 Clean up and put away the equipment you have used Follow your teacher s instructions for disposal of wastes 3

4 Data Table: Concentration of Reaction Rate (g/s) Mass of Mg (g) Reaction Time (s) HCl (M) Mg strip + 2 ml diluted HCl g Powdered CaCO ml concentrated HCl g Conclusion: An in concentration caused the reaction rate to 3 SURFACE AREA Surface area is how much area of an object is What kind of solid has the fastest reaction rate? the surface area the surface area Example: How do you change the reaction rate of burning wood? In the same amount of time, can collide with molecules of wood In the same amount of time, can collide with molecules of wood EXPERIMENT surface area Given the following materials and method, formulate a testable hypothesis to quantitatively show how changing the surface area will affect the reaction rate Hypothesis: (Write an If then because statement) Mortar and pestle 4 small test tubes Test tube rack 4 ml (total) of 10 M hydrochloric acid Solid pieces of calcium carbonate 4

5 Method: 1 Use the pestle to grind some calcium carbonate lumps into a fine powder in the mortar Place the four test tubes in the test tube rack 2 Place lumps of calcium carbonate into one of the test tubes to a depth of about 1 cm Place some finely ground calcium carbonate into a second test tube to a depth of about 1 cm 3 Measure dilute hydrochloric acid solution into the two remaining test tubes to a depth of about 2 cm 4 Simultaneously, pour the dilute HCl solution into each of the test tubes containing calcium carbonate Observe Note which reaction was faster 5 Clean up and put away the equipment you have used Follow your teacher s instructions for disposal of wastes Data Table: Mass of CaCO 3 (g) Reaction Time (s) Reaction Rate (g/s) Pieces of CaCO ml HCl Powdered CaCO ml HCl 156 g 156 g Conclusion: An in surface area caused the reaction rate to 4 PRESENCE OF A CATALYST A catalyst is a substance that increases the rate of a chemical reaction in the chemical reaction A catalyst is usually not written in the chemical equation of a reaction An is a biological catalyst Example: Saliva contains amylase that breaks down starch a catalyst a catalyst Catalysts do NOT create collisions between particles, they make better geometry for reactions to occur is needed to break old bonds and form new bonds in any chemical reaction We can increase the reaction rate by the amount of energy needed to break chemical bonds Catalysts allow reactions to occur with than what would be needed to break old chemical bonds and form new chemical bonds 5

6 TEACHER DEMO Given the following, formulate a testable hypothesis to qualitatively show how the presence of a catalyst will affect the reaction rate Hypothesis: (Write an If then because statement) 100mL graduated cylinder Collection tray Dish soap potassium iodide (KI) 6% hydrogen peroxide (H 2 O 2 ) Word Equation: Hydrogen peroxide decomposes in the presence of a catalyst to Balanced Chemical Equation: H 2 O 2 à Qualitative Observations Quantitative Observations (s) H 2 O 2 + dish soap H 2 O 2 + dish soap + KI Conclusion: The presence of a catalyst caused the reaction rate to 6

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