Reaction Rates I Expressing Reaction Rates reaction rate

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Reaction Rates I. Expressing Reaction Rates -____ reaction ____, rate or the ____ rate

Reaction Rates I. Expressing Reaction Rates -____ reaction ____, rate or the ____ rate at which a _____ chemical ____ reaction occurs, is expressed in terms of change ______ in ______ concentration of a ____ reactant or _______ product per unit ____ time What is the reaction rate of the following reaction, in moles/liter·second, if the concentration of NO is 0. 000 moles/liter at t 1 = 0. 00 seconds and 0. 010 moles/liter 2 seconds after the reaction begins? 1 CO (g) + 1 NO 2(g) Average reaction rate = 1 CO 2(g) + 1 NO(g) Δquantity Δt (t 2 – t 1) 0. 010 M – 0. 000 M 2. 00 s – 0. 00 s 0. 0050 mol/L·s

Reaction Rates I. Expressing Reaction Rates -____ reaction ____ rate can be expressed as

Reaction Rates I. Expressing Reaction Rates -____ reaction ____ rate can be expressed as the ____ rate at which a ____ product is produced or the ____ rate at which a reactant is consumed ____ What is the reaction rate of the following reaction, in moles/liter·second, if the concentration of C 4 H 9 Cl is 0. 220 M at t 1 = 0. 00 seconds and 0. 100 M 4. 00 seconds after the reaction begins? 1 C 4 H 9 Cl + 1 H 2 O Average reaction rate = 1 C 4 H 9 OH + 1 HCl Δquantity Δt 0. 100 M – 0. 220 M 4. 00 s – 0. 00 s 0. 0300 mol/L·s brackets indicate the concentration of butyl chloride

Reaction Rates I. Expressing Reaction Rates What is the reaction rate of the following

Reaction Rates I. Expressing Reaction Rates What is the reaction rate of the following reaction, in moles/liter·second, expressed in moles of H 2 consumed, if the concentration of H 2 is 0. 030 M at t 1 = 0. 00 seconds and 0. 020 M 4. 00 seconds after the reaction begins? 1 H 2 + 1 Cl 2 Average reaction rate = 0. 010 moles H 2 x 2 HCl Δquantity Δt 0. 020 M – 0. 030 M 4. 00 s – 0. 00 s 0. 0025 mol/L·s 2 moles HCl _______ 1 mole H 2 = 0. 020 moles HCl

Reaction Rates I. Expressing Reaction Rates What is the reaction rate of the following

Reaction Rates I. Expressing Reaction Rates What is the reaction rate of the following reaction, in moles/liter·second, expressed in moles of HCl produced, if the concentration of HCl is 0. 000 M at t 1 = 0. 00 seconds and 0. 020 M 4. 00 seconds after the reaction begins? 1 H 2 + 1 Cl 2 2 HCl Average reaction rate = Δquantity Δt 0. 020 M – 0. 000 M 4. 00 s – 0. 00 s 0. 0050 mol/L·s

Reaction Rates I. Expressing Reaction Rates What is the reaction rate of the following

Reaction Rates I. Expressing Reaction Rates What is the reaction rate of the following reaction, in moles/liter·minute, expressed in moles of H 2 O 2 consumed, if the concentration of H 2 O 2 is 2. 50 M at t 1 = 0. 00 minutes and 2. 12 M 2. 00 minutes after the reaction begins? 2 H 2 O 2 1 O 2 + 2 H 2 O Average reaction rate = Δquantity Δt 2. 12 M – 2. 50 M 2. 00 min – 0. 00 min 0. 19 mol/L·min

Reaction Rates I. Expressing Reaction Rates What is the reaction rate of the following

Reaction Rates I. Expressing Reaction Rates What is the reaction rate of the following reaction, in moles/liter·minute, expressed in moles of O 2 produced, if the concentration of H 2 O 2 is 1. 82 M at t 1 = 0. 00 minutes and 1. 48 M 5. 00 minutes after the reaction begins? 2 H 2 O 2 0. 34 moles H 2 O 2 x 1 mole O 2 _______ 2 mole H 2 O 2 Average reaction rate = 1 O 2 + 2 H 2 O = 0. 17 mole O 2 Δquantity Δt 0. 17 M – 0. 00 M 5. 00 min – 0. 00 min 0. 034 mol/L·min

Reaction Rates II. The Collision Theory -the _____ Collision Theory ______ states that, in

Reaction Rates II. The Collision Theory -the _____ Collision Theory ______ states that, in order for a ____ chemical ____ reaction to take place, the ______, atoms ____, ions or _____ molecules must _______ collide in order to _____ react Look at the picture of the cars to the right. Observe their position and orientation. What do you predict happened to the cars? Why do some of the cars appear to be more damaged than others?

Reaction Rates II. The Collision Theory -according to the _____ Collision Theory ______, ___

Reaction Rates II. The Collision Theory -according to the _____ Collision Theory ______, ___ Cl 2 and ___ H 2 molecules must _______ collide in order to _____, react but in the reaction of Carbon Nitrogen dioxide ______ monoxide ____ and ______, fraction of the _____ collisions only a small _______ produce ____ reactions Why? 1 CO (g) + 1 NO 2(g) 1 Cl 2 + 1 H 2 2 HCl 1 CO 2(g) + 1 NO(g)

Reaction Rates II. The Collision Theory Collision CO CO Collision NO 2 CO NO

Reaction Rates II. The Collision Theory Collision CO CO Collision NO 2 CO NO 2 Rebound Incorrect orientation NO 2 CO NO 2

Reaction Rates II. The Collision Theory Collision Correct orientation CO Activated complex NO 2

Reaction Rates II. The Collision Theory Collision Correct orientation CO Activated complex NO 2 Collision Cl 2 Orientation Always Correct H 2 NO

Reaction Rates II. The Collision Theory -according to the _____ Collision Theory ______, the

Reaction Rates II. The Collision Theory -according to the _____ Collision Theory ______, the _________ particles of ____ reacting substances must __ 1. _______, collide __ 2. _______ collide with the correct ______, orientation and __ 3. _______ collide with sufficient energy ______ to form the _______ activation complex Collision CO NO 2 Rebound Insufficient energy CO NO 2

Reaction Rates II. The Collision Theory -the minimum amount of ______ energy that reacting

Reaction Rates II. The Collision Theory -the minimum amount of ______ energy that reacting particles must have to form the ____ activation _______ complex is called the If you wanted to travel from Kalispell, Montana, to Browning, you could take the ____ activation ______, energy or ___ Ea scenic Going-to-the-Sun Highway through Glacier National Park. First, you would have to climb 1100 m to cross the continental divide at Logan Pass, but after that, it would be downhill all the way activation complex activation energy products reactants -a ____ high _____ activation ______ energy means that relatively ___ few _____ collisions will have sufficient ______ energy to produce the activation complex low _______, while a ___ activation ______ energy means that _____ many _____ collisions will have the required energy _____ to form the _____ activation _______, complex and the _______ reaction ____ rate will be ______ higher On the other hand, if you wanted to turn around and go back to Kalispell from Browning, you would only have to climb 700 m to Logan Pass, after which it would be downhill all the way, and you would end up at a lower elevation that when you started

Reaction Rates II. The Collision Theory -once ____ activation ______ energy has been supplied

Reaction Rates II. The Collision Theory -once ____ activation ______ energy has been supplied to the ____, reactants if the ____ products end up lying at a _____ lower ______ energy _____ state reactants then ______ energy is than the _____, released by the _______, reaction and the reaction ______ is _____ exothermic -if the ____ products end up lying at a _______ higher ______ energy _____ state than the _____, reactants then ______ energy is ____ absorbed by the _______, reaction and reaction is _____ endothermic the ____

Reaction Rates III. Factors Affecting Reaction Rates A. The Nature of the Reactants -one

Reaction Rates III. Factors Affecting Reaction Rates A. The Nature of the Reactants -one factor that affects the ____ rate of chemical _____ reactions is the ____ reactive _______ nature of the ____ reactants 1 Ca (s) + 2 H 2 O(l) 1 Ca(OH)2(aq) + 1 H 2(g) Calcium reacts with cold water to produce Calcium hydroxide and Hydrogen gas 2 Na (s) + 2 H 2 O(l) 2 Na. OH(aq) Sodium reacts with cold water to produce Sodium hydroxide and Hydrogen gas + 1 H 2(g)

Reaction Rates III. Factors Affecting Reaction Rates B. Concentration -when the _______ concentration of

Reaction Rates III. Factors Affecting Reaction Rates B. Concentration -when the _______ concentration of the _____ reactants is _____, increased reactions ______ speed ___ up collision is necessary for _____ chemical -since _____ reactions to take place, _____ increasing the ____________ concentration of the ____ reacting _____ particles increases the likelihood that the _____ particles of one ____ reactant will _______ collide with the particles of the other _____ reactant _____ 4 Fe + 3 O 2 2 Fe 2 O 3 +

Reaction Rates III. Factors Affecting Reaction Rates B. Concentration 4 Fe + 3 O

Reaction Rates III. Factors Affecting Reaction Rates B. Concentration 4 Fe + 3 O 2 2 Fe 2 O 3 + The concentration of oxygen in the air is about 21%, so the concentration of pure oxygen is about 5 times higher than that of air

Reaction Rates III. Factors Affecting Reaction Rates C. Surface Area -if the _______ surface

Reaction Rates III. Factors Affecting Reaction Rates C. Surface Area -if the _______ surface _____ area of the _____ same _____ mass of reactant is _____ increased by _____ reducing particle _____, size the _______ reaction ____ rate will ____, increase since surface _____ area allows the greater ____ particles of one ____ reactant to _______ collide with _____ more particles of the other ____ reactant per unit time 4 Fe + 3 O 2 2 Fe 2 O 3 +

Reaction Rates III. Factors Affecting Reaction Rates D. Temperature -_____ increasing the ______ temperature

Reaction Rates III. Factors Affecting Reaction Rates D. Temperature -_____ increasing the ______ temperature at which a reaction occurs _____ increases the _______ reaction ____ rate _______ According to the curve of the graph, increasing the ______ temperature _____ increases the -_____ what temperature increase, in Kelvin, kinetic energy particles that average _______ of the _____ doubles the rate of reaction? _______K make up a substance, causing the ____ particles to At what Kelvin temperature is the _______ collide more ______ frequently relative reaction rate 25? 40 _______K 290 Relative Reaction Rate 2 310 8 320 16 35 Relative Reaction Rate Temperature (in K) 30 25 20 15 10 5 330 32 0 280 290 300 310 320 Temperature (in K) 330

Reaction Rates III. Factors Affecting Reaction Rates increasing the ______ temperature also ____ increases

Reaction Rates III. Factors Affecting Reaction Rates increasing the ______ temperature also ____ increases D. Temperature -_____ rate of _______ reaction by _____ increasing the _______ number of _____ particles with _____ sufficient ____ collision ______ energy to cause a _______ reaction -_______ increasing the ______, temperature then, increases the _______ reaction ____ rate by _____ increasing the collision _____ frequency and the _____ collision _____ energy ______

Reaction Rates III. Factors Affecting Reaction Rates E. Catalysts -_____ catalysts are _____ substances

Reaction Rates III. Factors Affecting Reaction Rates E. Catalysts -_____ catalysts are _____ substances that increase _______ the _____ rate of ____ reaction without being _____ consumed by Substrate (Reactant) the ____ reaction enzymes are _____ biological ____ catalysts which cause -____ reactions to happen or happen ______ faster without _____ raising the _____, temperature which could ____ damage _______ Enzyme living things by _____ denaturing their ____ proteins -____ catalysts increase ____ reaction ____ rate by ____ lowering activation ______ energy for a _____, reaction so that the _____ particles that had ______ insufficient energy before ____ sufficient energy to ______ react now have _____ -_____ inhibitors make reactions _____ less likely to _______ proceed by ____ raising the _____ activation ______ energy

Reaction Rates III. Factors Affecting Reaction Rates 1. Hypothesis: What is the effect of

Reaction Rates III. Factors Affecting Reaction Rates 1. Hypothesis: What is the effect of temperature on the rate of reaction? 2. Prediction: 3. Gather Data: A. Safety: The surfaces of the hot plates and the water will be hot enough to cause burns. Use caution. B. Procedure: 1. Obtain an effervescent tablet and break it into 4 pieces of roughly equal size. 2. Measure and record the mass of 1 piece of effervescent tablet.

Reaction Rates III. Factors Affecting Reaction Rates 3. Gather Data: B. Procedure: 3. Using

Reaction Rates III. Factors Affecting Reaction Rates 3. Gather Data: B. Procedure: 3. Using a 100 -m. L graduated cylinder, measure 50 m. L of room temperature water (about 20°C) into a plastic cup. Measure and record the temperature to the nearest Celsius degree. 4. Using a stopwatch to record the elapsed time between the time the reaction begins and the time the reaction ends, drop the tablet into the cup to begin the reaction. Record the time in seconds. 1 H 3 C 6 H 5 O 7 + 1 C 4 H 8 O 4 + 4 Na. HCO 3 Citric acid Acetylsalicylic acid Sodium bicarbonate 1 Na. C 4 H 7 O 4 + 1 Na 3 C 6 H 5 O 7 + 4 H 2 O + 4 CO 2 Sodium acetyl salicylate Sodium citrate Water Carbon dioxide

Reaction Rates III. Factors Affecting Reaction Rates 3. Gather Data: B. Procedure: 5. Repeat

Reaction Rates III. Factors Affecting Reaction Rates 3. Gather Data: B. Procedure: 5. Repeat steps 2, 3, and 4 twice, except with 50 m. L of water at about 50°C, and 65°C. Temperature (in °C) Mass of Tablet (in g) Reaction Time (in s) Reaction Rate (in g/s) 4. Analyze Data: A. Calculate the reaction rate (in g/s) for each of the three trials

Reaction Rates III. Factors Affecting Reaction Rates 4. Analyze Data: 0. 10 0. 09

Reaction Rates III. Factors Affecting Reaction Rates 4. Analyze Data: 0. 10 0. 09 Relative Reaction Rate (in g/s) B. Graph the temperature versus the reaction rate on the following graph, and draw a best-fit curve for the data 0. 08 0. 07 0. 06 0. 05 0. 04 0. 03 0. 02 0. 01 0. 00 0 10 20 30 40 50 60 70 Temperature (in °C) 80 90 100

Reaction Rates III. Factors Affecting Reaction Rates 4. Analyze Data: C. Using the data

Reaction Rates III. Factors Affecting Reaction Rates 4. Analyze Data: C. Using the data from the graph, predict the reaction rate, in g/s, of the reaction at a temperature of 40°C. _________ D. Measure and record the mass of the last piece of effervescent tablet. E. Using a 100 -m. L graduated cylinder, measure 50 m. L of water at about 40°C into a plastic cup. Measure and record the temperature to the nearest Celsius degree. F. Using a stopwatch to record the elapsed time between the time the reaction begins and the time the reaction ends, drop the tablet into the cup to begin the reaction. Record the time in seconds, and calculate and record the reaction rate. How does your calculation compare to your prediction?

Reaction Rates III. Factors Affecting Reaction Rates 5. Draw Conclusions: using the analysis of

Reaction Rates III. Factors Affecting Reaction Rates 5. Draw Conclusions: using the analysis of the data, answer the question of the hypothesis ________________________________________

Reaction Rates IV. Reaction Rate Laws -when we divide the ____ change in _______

Reaction Rates IV. Reaction Rate Laws -when we divide the ____ change in _______ molar ______, concentration _____ (Δquantity) by the _______ change in _____, time ____, (Δt) we get an average ____ reaction _____ rate ____ -chemical reactions tend to _____ slow _____ down as ____ reactants are _____, consumed because in order particles must for a reaction to proceed, _____ collide and as _____ reactants are _____ consumed _______, there are ______ fewer ____ particles left to _______ collide Hitting the cue ball gives the cue ball kinetic energy, and as it collides with the other balls, they, in turn, receive kinetic energy and collide with other balls Decreasing the number of balls on the table reduces the number of collisions ultimately caused by the initial collision of the cue ball

Reaction Rates IV. Reaction Rate Laws -_____ rate ______ laws ____ quantify the results

Reaction Rates IV. Reaction Rate Laws -_____ rate ______ laws ____ quantify the results of the _____ collision _______ theory in terms of a ______ mathematical ______ relationship between the rate of a _____ chemical ____ reaction and the _____ reactant _______ concentration ____ -in the reaction __ A ___ → __, B there is only ___ one _______ between the ____ activated complex reactants products so the _____ rate ____ law for the and ____, Rate = __ k ____, [A] where ____ [A] is reaction is _____ concentration of the _____ reactant __ A the _______ and __ k is the _______ experimentally _____ determined _____ specific ____ rate ____, constant which depends reaction conditions on _________, especially the temperature ______ -the ____ reaction _____, rate then, is _____ directly _______ proportional to the _______ concentration

Reaction Rates V. Reaction Orders -in the reaction __ A ___ → __, B

Reaction Rates V. Reaction Orders -in the reaction __ A ___ → __, B the _____ Rate = __ k [A] ___, [A] means the same and it is understood that ____ [A]1 and the _____ exponent __ 1 is the ____ reaction as ____, order ______ 2 H 2 O 2 2 H 2 O + 1 O 2 -the _____ rate ____ law for the _______ decomposition of _____ H 2 O 2 is _____ Rate = __ k ______, [H 2 O 2]1 and the ____ reaction is said to be _____ first _____ order in _____ H 2 O 2 A + B products -for _____ reactions with _____ more than _____ one _______, ____ is reactant the _____ rate law m _____ Rate = __ k [A] [B]n m is the _______ reaction _____ order for __ A and __ n is where __ reaction _____ order for __ B the _______

Reaction Rates V. Reaction Orders -for the ____ reaction that has the _____ rate

Reaction Rates V. Reaction Orders -for the ____ reaction that has the _____ rate ____ law _________, Rate = k [NO]2 [H 2]1 the reaction is described as _______ second _____ order in ___, NO _____ first _____ order in ___, H 2 third _____ order overall and _____ -an ______ experimental _______ method of evaluating ____ the _______ reaction ______is order method of _______ initial ______, rates in which the _______ concentrations of the reactants are _______ varied and the effect on the _____ reaction _____ rate is observed ____ A + B Trial Initial [A] (in M) Initial [B] (in M) products Initial Rate (in mol/L·s) 1 0. 100 2. 00 x 10 -3 2 0. 200 0. 100 4. 00 x 10 -3 3 0. 200 16. 00 x 10 -3

Reaction Rates V. Reaction Orders -the _____ rate ____ law for this type of

Reaction Rates V. Reaction Orders -the _____ rate ____ law for this type of reaction is _________. Rate = k [A]m [B]n From the data, you can [B] was held constant, the see that, while ____ reaction _____ rate has ____ doubled in Trial 2 ____ [A] has compared to Trial 1, at the same time ________, ______ __ doubled so the ____ reaction order m must equal __, 1 or because ___ 2 m = __, 2 __ m = __ 1 [B] is -in Trial 3 compared to Trial 2, _______, doubled and the _______ reaction ____ rate ______, quadruples so the ____ reaction ______ order __ n must equal __, 2 or overall _____ rate ____ law is ___ 2 n = __, 4 and the _______ Rate = k [A]1 [B]2 _________ overall ____ reaction ______ order is ______ third and the _______ order _______ (2 + 1)

Reaction Rates V. Reaction Orders Given the following experimental data, use the method of

Reaction Rates V. Reaction Orders Given the following experimental data, use the method of initial rates to determine the rate law for the reaction and the overall reaction order. A + B Trial [A] = 2 m Initial [A] (in M) 1 0. 100 2 0. 200 Initial [B] (in M) 0. 200 Initial Rate (in mol/L·s) 0. 100 2. 00 x 10 -3 0. 100 10 -3 [B] = 3 products 2. 00 x 2 n 0. 200 rate = 1 rate = 2 4. 00 x 10 -3 Rate = k [A]m [B]n Rate = k [A]0 [B]1 Rate = k [B], overall reaction order = first order

Reaction Rates V. Reaction Orders Given the following experimental data, use the method of

Reaction Rates V. Reaction Orders Given the following experimental data, use the method of initial rates to determine the rate law for the reaction and the overall reaction order. CH 3 CHO] = 2 m Trial Initial [CH 3 CHO] (in M) 1 2. 00 x 10 -3 2 [CH 3 CHO] = 2 m 3 CH 4 + CO Initial Rate (in mol/L·s) 2. 70 x 10 -11 rate = 4 4. 00 x 10 -3 10. 8 x 10 -11 8. 00 x 10 -3 43. 2 x 10 -11 rate = 4 Rate = k [CH 3 CHO]m Rate = k [CH 3 CHO]2, overall reaction order = second order

Reaction Rates V. Reaction Orders Given the following experimental data, use the method of

Reaction Rates V. Reaction Orders Given the following experimental data, use the method of initial rates to determine the rate law for the reaction, the overall reaction order, and the value of the specific rate constant. 2 NO + Cl 2 2 NOCl Trial Initial [NO] (in M) Initial [Cl 2] (in M) Initial Rate (in mol/L·min) [NO] = 2 m 1 0. 50 2 1. 00 3 1. 00 0. 50 1. 90 x 10 -2 0. 50 10 -2 1. 00 [Cl 2] = 2 n 7. 60 x rate = 4 rate = 2 15. 20 x 10 -2 Rate = k [NO]m [Cl 2]n Rate = k [NO]2 [Cl 2]n (or 0. 15 L 2/mol 2·min) Rate = k [NO]2 [Cl 2]1 (or 0. 152 L 2/mol 2·min) overall reaction order = third order, k = 0. 16 L 2/mol 2·min

Reaction Rates V. Reaction Orders Given the following experimental data, use the method of

Reaction Rates V. Reaction Orders Given the following experimental data, use the method of initial rates to determine the rate law for the reaction, the overall reaction order, and the value of the specific rate constant. 2 Cl. O 2(aq) + 2 OH-(aq) 1 Cl. O 3 - + 1 Cl. O 2 - + 1 H 2 O(1) Trial Initial [Cl. O 2] (in M)Initial [OH-] (in M) Initial Rate (in mol/L·min) [Cl. O 2] = 2 m 1 2 3 0. 0500 0. 100 0. 200 0. 100 6. 90 [OH-] = ½n 27. 6 rate = 4 rate = ½ 13. 8 Rate = k [Cl. O 2]m [OH-]n Rate = k [Cl. O 2]2 [OH-]1 overall reaction order = third order, k = 1. 38 x 104 L 2/mol 2·min

Reaction Rates V. Reaction Orders Given the following experimental data, use the method of

Reaction Rates V. Reaction Orders Given the following experimental data, use the method of initial rates to determine the rate law for the reaction, the overall reaction order, and the value of the specific rate constant. A + B 2 C Trial 1 [A] = 2 m 2 Initial [A] (in M) 0. 010 0. 020 Initial [B] (in M) 0. 010 3 0. 020 0. 0060 0. 010 [B] = Initial Rate (in mol/L·s) 0. 0240 2 n 0. 020 rate = 4 0. 0960 Rate = k [A]m [B]n Rate = k [A]2 [B]2 overall reaction order = fourth order, k = 6. 0 x 105 L 3/mol 3·s

Reaction Rates V. Reaction Orders Given the following experimental data, use the method of

Reaction Rates V. Reaction Orders Given the following experimental data, use the method of initial rates to determine the rate law for the reaction, the overall reaction order, and the value of the specific rate constant. A + B products Trial 1 [A] = 1½m 2 Initial [A] (in M) 0. 010 0. 015 Initial [B] (in M) Initial Rate (in mol/L·hr) 0. 020 [B] = 3 0. 015 0. 020 0. 030 2 n 0. 040 rate = 1½ rate = 8 0. 240 Rate = k [A]m [B]n Rate = k [A]1 [B]3 overall reaction order = fourth order, k = 2. 5 x 105 L 3/mol 3·hr

Reaction Rates V. Reaction Orders A chemical reaction involving compound A and compound B

Reaction Rates V. Reaction Orders A chemical reaction involving compound A and compound B as reactants is found to be first order in A and second order in B. What will the reaction rate be for Trial 2? Trial Initial [A] (in M) Initial [B] (in M) Initial Rate (in mol/L·s) 1 1. 0 0. 20 0. 10 2 2. 0 0. 60 ? Rate = k [A]m [B]n Rate = k [A]1 [B]2 0. 10 mol/L·s = k (1. 0 mol/L)1 (0. 20 mol/L)2 k = 2. 5 L 2/mol 2·s Rate = k [A]1 [B]2 Rate = (2. 5 L 2/mol 2·s)(2. 0 mol/L)1 (0. 60 mol/L)2 = 1. 8 mol/L·s

Reaction Rates V. Reaction Orders -most _____ chemical _____ reactions obey ____ one of

Reaction Rates V. Reaction Orders -most _____ chemical _____ reactions obey ____ one of ______ three _____ rate ______: laws zero _____, order _____ first _____, order or _______ second _____, order and the ______ units of specific _____ rate ____, constant __, k vary with the _____ order of the ____ reaction the ______ reaction with ____ one or _____ more _____ reactants -if a ____ experimentally _____ determined to be _____ zero was _______ order _______, overall the _____ rate _____ law would be _____________ Rate = k [A]0 or ________ Rate = k [A]0 [B]0 -in ______ zero ______ order reactions, the _____ rate _____ law is _____, Rate = k and the ______ units of __ k are ____ mol/L·s

Reaction Rates V. Reaction Orders A [A] = 2 m Trial Initial [A] (in

Reaction Rates V. Reaction Orders A [A] = 2 m Trial Initial [A] (in M) 1 2. 00 x 10 -3 2 3 B Initial Rate (in mol/L·s) 1. 75 x 10 -11 rate = 1 4. 00 x 10 -3 1. 75 x 10 -11 8. 00 x 10 -3 1. 75 x 10 -11 Rate = k [A]m Rate = k [A]0, overall reaction order = zero order Rate = k rate = 1

Reaction Rates V. Reaction Orders -plot the data from the table on the graph

Reaction Rates V. Reaction Orders -plot the data from the table on the graph below: 10. 00 Reaction Rate x 10 -11 (in mol/L·s) 9. 00 8. 00 7. 00 6. 00 5. 00 4. 00 3. 00 2. 00 1. 00 0 . 0 10 00 9. 00 8. 00 7. 00 6. 00 5. 00 4. 00 3. 00 2. 00 1. 00 0. Concentration [A] x 10 -3 (in mol/L)

Reaction Rates reaction with ____ one or _____ more _____ reactants V. Reaction Orders

Reaction Rates reaction with ____ one or _____ more _____ reactants V. Reaction Orders -if a ____ experimentally _____ determined to be _____ first was _______ order _______, overall the _____ rate _____ law would be _____________ Rate = k [A]1 or ________ Rate = k [A]1 [B]0 -in ______ first ______ order reactions, the _____ rate _____ law is _______, Rate = k [A] and the ______ units of __ k are ____ 1/s A + B products Trial 2. 00 x 10 -11 1. 00 x m 10 -3 2. 00 x 10 -11 3 2. 00 x 10 -3 4. 00 x 10 -11 4 4. 00 x 10 -3 2. 00 x 10 -3 8. 00 x 10 -11 2 1. 00 x 10 -3 Initial Rate (in mol/L·s) 1. 00 x 10 -3 1 [B] = 2 n Initial [A] (in M) Initial [B] (in M) [A] = 2 rate = 1 rate = 2 Rate = k [A]m [B]n Rate = k [A]m [B]0 Rate = k [A]1 [B]0 Rate = k [A], overall reaction order = first order

Reaction Rates V. Reaction Orders -plot the data from the table on the graph

Reaction Rates V. Reaction Orders -plot the data from the table on the graph below: 10. 00 Reaction Rate x 10 -11 (in mol/L·s) 9. 00 zero-order reaction 8. 00 7. 00 6. 00 5. 00 4. 00 3. 00 2. 00 1. 00 0 . 0 10 00 9. 00 8. 00 7. 00 6. 00 5. 00 4. 00 3. 00 2. 00 1. 00 0. Concentration [A] x 10 -3 (in mol/L)

Reaction Rates reaction with ____ one or _____ more _____ reactants V. Reaction Orders

Reaction Rates reaction with ____ one or _____ more _____ reactants V. Reaction Orders -if a ____ experimentally _____ determined to be ______ second was _______ A + B order _______, overall the _____ rate _____ law would be _____________ Rate = k [A]2 or ________ Rate = k [A]1 [B]1 -in ______ second ______ order reactions, the _____ rate _____ law is ________ Rate = k [A] [B] or ______, Rate = k [A]2 and the ______ units of __ k are_______ L/mol·s products Trial 1 [B] = 2 m 2 Initial [A] (in M) Initial [B] (in M) 1. 00 x 10 -3 -3 1. 00 x 10 n [A] = 2 Initial Rate (in mol/L·s) 1. 00 x 10 -3 0. 500 x 10 -11 2. 00 x 10 -3 10 -11 0. 500 x 10 -11 3 2. 00 x 10 -3 2. 00 x 4 4. 00 x 10 -3 2. 00 x 10 -3 8. 00 x 10 -11 Rate = k [A]m [B]n Rate = k [A]m [B]0 Rate = k [A]2, overall reaction order = second order rate = 1 rate = 4

Reaction Rates V. Reaction Orders -plot the data from the table on the graph

Reaction Rates V. Reaction Orders -plot the data from the table on the graph below: second-order reaction first-order reaction 10. 00 Reaction Rate x 10 -11 (in mol/L·s) 9. 00 zero-order reaction 8. 00 7. 00 6. 00 5. 00 4. 00 3. 00 2. 00 1. 00 0 . 0 10 00 9. 00 8. 00 7. 00 6. 00 5. 00 4. 00 3. 00 2. 00 1. 00 0. Concentration [A] x 10 -3 (in mol/L)

Reaction Rates VI. Instantaneous Reaction Rates -while the ____ average _____ reaction _____ rate

Reaction Rates VI. Instantaneous Reaction Rates -while the ____ average _____ reaction _____ rate gives the ____ reaction _____ rate over a period of _____, time the ______ Time, t (in s) [C 4 H 9 Cl] (in M) Average rate (in mol/L·s) instantaneous rate reaction shows the ____ Calculate w/Δquantity/Δt 0. 1000 0. 0 _____ rate at a ____ specific _____ time 50. 0905 1. 9 x 10 -4 100. 0820 1. 7 x 10 -4 150. 0741 1. 6 x 10 -4 200. 0671 1. 4 x 10 -4 300. 0549 1. 22 x 10 -4 400. 0448 1. 01 x 10 -4 500. 0368 0. 80 x 10 -4 800. 0200 0. 560 x 10 -4 1 C 4 H 9 Cl + 1 H 2 O 1 C 4 H 9 OH + 1 HCl

Reaction Rates VI. Instantaneous Reaction Rates -plot the data from the table on the

Reaction Rates VI. Instantaneous Reaction Rates -plot the data from the table on the graph below: 0. 10 0. 09 Instantaneous = rate rise run Δ[C 4 H 9 Cl] Δt 0. 07 0. 06 0. 05 Δ[C 4 H 9 Cl] Instantaneous = Slope of rate the tangent [C 4 H 9 Cl (in M) 0. 08 0. 04 0. 03 0. 02 Instantaneous 0. 03 mol/L 0. 01 = rate 400 s 0. 00 Instantaneous = 0. 8 x 10 -4 mol/L·s rate Δt 0 100 200 300 400 500 600 700 800 900 1000 Time (in s)

Reaction Rates VI. Instantaneous Reaction Rates -as the reaction proceeds, and the rate of

Reaction Rates VI. Instantaneous Reaction Rates -as the reaction proceeds, and the rate of _____ collision goes _____ down as ____ particles of _____ reactants are _____, consumed the ______ slope of the line ____ tangent to the _____ curve _____ goes _____ down as the ____ reaction ____ rate goes _____ down

Reaction Rates VI. Instantaneous Reaction Rates If the following equation is first order in

Reaction Rates VI. Instantaneous Reaction Rates If the following equation is first order in H 2 and second order in NO with a rate constant of 2. 90 x 102 L 2/mol 2·s, what is the instantaneous rate when [NO] = 0. 00200 M and [H 2] = 0. 00400 M ? 2 NO + 1 H 2 1 N 2 O + 1 H 2 O Rate = k [NO]2 [H 2]1 Rate = (2. 90 x 102 L 2/mol 2·s)(0. 00200 mol/L)2 (0. 00400 mol/L)1 Rate = 4. 64 x 10 -6 mol/L·s

Reaction Rates VI. Instantaneous Reaction Rates If the following equation is first order in

Reaction Rates VI. Instantaneous Reaction Rates If the following equation is first order in H 2 and second order in NO with a rate constant of 2. 90 x 102 L 2/mol 2·s, what is the instantaneous rate when [NO] = 0. 00500 M and [H 2] = 0. 00200 M ? 2 NO + 1 H 2 1 N 2 O + 1 H 2 O Rate = k [NO]2 [H 2]1 Rate = (2. 90 x 102 L 2/mol 2·s)(0. 00500 mol/L)2 (0. 00200 mol/L)1 Rate = 1. 45 x 10 -5 mol/L·s

Reaction Rates VI. Instantaneous Reaction Rates If the following equation is first order in

Reaction Rates VI. Instantaneous Reaction Rates If the following equation is first order in H 2 and second order in NO with a rate constant of 2. 90 x 102 L 2/mol 2·s, what is the instantaneous rate when [NO] = 0. 0100 M and [H 2] = 0. 00125 M ? 2 NO + 1 H 2 1 N 2 O + 1 H 2 O Rate = k [NO]2 [H 2]1 Rate = (2. 90 x 102 L 2/mol 2·s)(0. 0100 mol/L)2 (0. 00125 mol/L)1 Rate = 3. 62 x 10 -5 mol/L·s

Reaction Rates VI. Instantaneous Reaction Rates If the following equation is first order in

Reaction Rates VI. Instantaneous Reaction Rates If the following equation is first order in H 2 and second order in NO with a rate constant of 2. 90 x 102 L 2/mol 2·s, what is the instantaneous rate when [NO] = 0. 00446 M and [H 2] = 0. 00282 M ? 2 NO + 1 H 2 1 N 2 O + 1 H 2 O Rate = k [NO]2 [H 2]1 Rate = (2. 90 x 102 L 2/mol 2·s)(0. 00446 mol/L)2 (0. 00282 mol/L)1 Rate = 1. 63 x 10 -5 mol/L·s

Reaction Rates VI. Instantaneous Reaction Rates If the following equation is first order in

Reaction Rates VI. Instantaneous Reaction Rates If the following equation is first order in A and second order in B with a specific rate constant of 4. 75 x 10 -7 L 2/mol 2·s, what is the instantaneous rate when [A] = 0. 355 M and [B] = 0. 0122 M ? A + B products Rate = k [A]1 [B]2 Rate = (4. 75 x 10 -7 L 2/mol 2·s)(0. 355 mol/L)1(0. 0122 mol/L)2 Rate = 2. 51 x 10 -11 mol/L·s

Reaction Rates VII. Reaction Mechanisms -_____ most chemical reactions consist of a ______ series

Reaction Rates VII. Reaction Mechanisms -_____ most chemical reactions consist of a ______ series of ____ one or _____ more simpler _____ reactions -a ____ complex ____ reaction consists of ____ two more ______ elementary steps or _____ 1 Cl + 1 O 3 1 Cl. O + 1 O 2 O 3 -for example, the _______ decomposition of ______, ozone an _____ allotrope of ____, oxygen in the ______ ozone _____ layer is a ____ complex reaction consisting of ______ three ____ elementary _____ reactions in the ______ reaction _____: mechanism following ____ 1 O 2 + 1 Cl. O 1 O 2 + 1 Cl 3 O 2

Reaction Rates VII. Reaction Mechanisms -because ____ Cl is a _______ reactant in the

Reaction Rates VII. Reaction Mechanisms -because ____ Cl is a _______ reactant in the _____ first _____ elementary step and is _____ re-formed in the _____ last ______ elementary step, it technically _____ increases the _____ rate of reaction without being _____ consumed _____ itself, and so is a _____ catalyst to the _______ decomposition of ozone Cl. O and ___ O are formed -because both _____ one ______ elementary step of the in _______ complex reaction and _____ consumed in a ___________ subsequent step, they are intermediates 1 Cl + 1 O 3 1 Cl. O + 1 O 1 O 2 2 O 3 3 O 2 + 1 Cl. O + 1 Cl

Reaction Rates VII. Rate-Determining Step in a Complex -the _______ slowest elementary Reaction Mechanism

Reaction Rates VII. Rate-Determining Step in a Complex -the _______ slowest elementary Reaction Mechanism step in the ____ reaction _____ mechanism of a 2 NO 1 N 2 O 2 ____ complex ____limits reaction 1 N 2 O 2 + 1 H 2 1 N 2 O + 1 H 2 O the ______ instantaneous ____ rate overall _______, reaction 1 N 2 O + 1 H 2 1 N 2 + 1 H 2 O of the _______ and so is called the 2 NO + 2 H 2 1 N 2 + 2 H 2 O _______ rate-determining ____ step Energy Rate-Determining Step 2 NO + 2 H 2 -the elementary step with the _______ highest _____ activation ______ energy is the _______, slowest and so is the rate-determining ____ step _______ 1 N 2 O 2 + 2 H 2 1 N 2 O + 1 H 2 Reaction progress 1 N 2 + 2 H 2 O