15. Chemical Kinetics

Average Rate of Reaction

15. Chemical Kinetics

Average Rate of Reaction

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Average Rate of Reaction Concept 1

Average Rate of Reaction Example 1

Average Rate of Reaction Example 2

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Average Reaction Rate and Unique Average Reaction Rate

06:04

Average Reaction Rate and Unique Average Reaction Rate

Kinetics: Initial Rates and Integrated Rate Laws

Professor Dave Explains

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Introduction to reaction rates | Kinetics | AP Chemistry | Khan Academy

09:14

Introduction to reaction rates | Kinetics | AP Chemistry | Khan Academy

Khan Academy Organic Chemistry

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Chemical Kinetics: Calculating Average Rates and Instantaneous Rates

19:15

Chemical Kinetics: Calculating Average Rates and Instantaneous Rates

Average versus Instantaneous Reaction Rates

Ben's Chem Videos

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Multiple Choice

Consider the following reaction:2 H₂O₂ (aq) → 2 H₂O (l) + O₂ (g)

Calculate the rate of the reaction between 25 sec and 65 sec.

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Multiple Choice

The rate of consumption of C₃H₆ in the following reaction is 0.45 M/s. Calculate the rate of production of H₂O.
2 C₃H₆ + 2 NH₃ + 3 O₂ → 2 CH₂CHCN + 6 H₂O

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Textbook Question

Use the following equation and graph to answer questions 1 and 2. Hydrogen iodide decomposes at 410 °C, according the reaction: 2 HI1g2¡H21g2 + I21g2 The graph shows how the concentration of HI changes over time. What is the average rate of loss of HI over the time period 0–40 s (LO 14.1) (a) 7.5 * 10-3 M>s (b) 4.8 * 10-3 M>s (c) 3.0 * 10-2 M>s (d) 3.5 * 10-3 M>s

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Textbook Question

You study the rate of a reaction, measuring both the concentration of the reactant and the concentration of the product as a function of time, and obtain the following results:

Which chemical equation is consistent with these data: (i) A → B, (ii) B → A, (iii) A → 2 B, (iv) B → 2 A?

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Textbook Question

(a) What are the units usually used to express the rates of reactions occurring in solution?

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Textbook Question

Consider the following hypothetical aqueous reaction: A1aq2S B1aq2. A flask is charged with 0.065 mol of A in a total volume of 100.0 mL. The following data are collected: Time (min) 0 10 20 30 40 Moles of A 0.065 0.051 0.042 0.036 0.031 (a) Calculate the number of moles of B at each time in the table, assuming that there are no molecules of B at time zero and that A cleanly converts to B with no intermediates.

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Textbook Question

Consider the following hypothetical aqueous reaction: A1aq2S B1aq2. A flask is charged with 0.065 mol of A in a total volume of 100.0 mL. The following data are collected: Time (min) 0 10 20 30 40 Moles of A 0.065 0.051 0.042 0.036 0.031 (b) Calculate the average rate of disappearance of A for each 10-min interval in units of M>s.

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Textbook Question

A flask is charged with 0.100 mol of A and allowed to react to form B according to the hypothetical gas-phase reaction A1g2¡B1g2. The following data are collected: Time (s) 0 40 80 120 160 Moles of A 0.100 0.067 0.045 0.030 0.020 (c) Which of the following would be needed to calculate the rate in units of concentration per time: (i) the pressure of the gas at each time, (ii) the volume of the reaction flask, (iii) the temperature, or (iv) the molecular weight of A?

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Textbook Question

The isomerization of methyl isonitrile 1CH3NC2 to acetonitrile 1CH3CN2 was studied in the gas phase at 215 C, and the following data were obtained: Time (s) 3CH3nC4 1M2 0 0.0165 2000 0.0110 5000 0.00591 8000 0.00314 12,000 0.00137 15,000 0.00074 (b) Calculate the average rate of reaction over the entire time of the data from t = 0 to t = 15,000 s.

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Textbook Question

The rate of disappearance of HCl was measured for the following reaction: CH3OH1aq2 + HCl1aq2¡CH3Cl1aq2 + H2O1l2 The following data were collected: Time (min) 3HCl 4 1M2 0.0 1.85 54.0 1.58 107.0 1.36 215.0 1.02 430.0 0.580 (b) Calculate the average rate of reaction for the entire time for the data from t = 0.0 min to t = 430.0 min.

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Textbook Question

The rate of disappearance of HCl was measured for the following reaction: CH3OH1aq2 + HCl1aq2¡CH3Cl1aq2 + H2O1l2 The following data were collected: Time (min) 3HCl 4 1M2 0.0 1.85 54.0 1.58 107.0 1.36 215.0 1.02 430.0 0.580 (a) Calculate the average rate of reaction, in M>s, for the time interval between each measurement.

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Textbook Question

The rate of disappearance of HCl was measured for the following reaction: CH3OH1aq2 + HCl1aq2¡CH3Cl1aq2 + H2O1l2 The following data were collected: Time (min) 3HCl 4 1M2 0.0 1.85 54.0 1.58 107.0 1.36 215.0 1.02 430.0 0.580 (c) Which is greater, the average rate between t = 54.0 and t = 215.0 min, or between t = 107.0 and t = 430.0 min?

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Textbook Question

For each of the following gas-phase reactions, indicate how the rate of disappearance of each reactant is related to the rate of appearance of each product: (c) N21g2 + 3 H21g2¡2 NH31g2

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Textbook Question

(b) The reaction 2 NO1g2 + Cl21g2¡2 NOCl1g2 is carried out in a closed vessel. If the partial pressure of NO is decreasing at the rate of 56 torr/min, what is the rate of change of the total pressure of the vessel?

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Textbook Question

Consider the reaction: 2 HBr( g) ¡ H2( g) + Br2( g) a. Express the rate of the reaction in terms of the change in concentration of each of the reactants and products.

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Textbook Question

Consider the reaction:

2 HBr (g) → H₂ (g) + Br₂ (g)

c. If the volume of the reaction vessel in part b was 1.50 L, what amount of Br₂ (in moles) was formed during the first 15.0 s of the reaction?

Consider the reaction: 2 HBr( g) ¡ H2( g) + Br2( g) b. In the first 25.0 s of this reaction, the concentration of HBr dropped from 0.600 M to 0.512 M. Calculate the average rate of the reaction during this time interval.

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Textbook Question

Consider the reaction: 2 N2O( g) ¡ 2 N2( g) + O2( g) a. Express the rate of the reaction in terms of the change in concentration of each of the reactants and products.

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Textbook Question

For the reaction 2 A( g) + B( g) ¡ 3 C( g), b. when A is decreasing at a rate of 0.100 M>s, how fast is B decreasing? How fast is C increasing?

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Textbook Question

For the reaction 2 A( g) + B( g) ¡ 3 C( g), a. determine the expression for the rate of the reaction in terms of the change in concentration of each of the reactants and products.

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Textbook Question

Consider the reaction: 8 H2S( g) + 4 O2( g) ¡ 8 H2O( g) + S8( g) Complete the table.

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Textbook Question

Consider the reaction: C4H8( g) ¡ 2 C2H4( g) The tabulated data were collected for the concentration of C4H8 as a function of time: a. What is the average rate of the reaction between 0 and 10 s? Between 40 and 50 s?

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Textbook Question

Consider the reaction: NO2( g) ¡ NO( g) + 1 2 O2( g) The tabulated data were collected for the concentration of NO2 as a function of time: a. What is the average rate of the reaction between 10 and 20 s? Between 50 and 60 s?

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Textbook Question

Consider the reaction: NO2( g) ¡ NO( g) + 1 2 O2( g) The tabulated data were collected for the concentration of NO2 as a function of time: b. What is the rate of formation of O2 between 50 and 60 s?

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Textbook Question

Consider the reaction: H2( g) + Br2( g) ¡ 2 HBr( g) The graph shows the concentration of Br2 as a function of time.

a. Use the graph to calculate each quantity: (i) the average rate of the reaction between 0 and 25 s

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Textbook Question

Consider the reaction: 2 H2O2(aq) ¡ 2 H2O(l ) + O2( g) The graph shows the concentration of H2O2 as a function of time. Use the graph to calculate each quantity: d. If the initial volume of the H2O2 is 1.5 L, what total amount of O2 (in moles) is formed in the first 50 s of reaction?

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Textbook Question

A 1.50 L sample of gaseous HI having a density of 0.0101 g>cm3 is heated at 410 °C. As time passes, the HI decomposes to gaseous H2 and I2. The rate law is -Δ3HI4>Δt = k3HI42, where k = 0.031>1M ~ min2 at 410 °C. (b) What is the partial pressure of H2 after a reaction time of 8.00 h?

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Open Question

Which species has the greatest rate of appearance in the reaction below? 2 H₂S + O₂ → 2 S + 2 H₂O

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Open Question

Which species has the greatest rate of disappearance in the reaction below? CH₄ + 2 O₂ → CO₂ + 2 H₂O

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Open Question

Which species has the greatest rate of disappearance in the reaction below? CH₄ + 2 O₂ → CO₂+ 2 H₂O

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15. Chemical Kinetics

Average Rate of Reaction

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