15. Chemical Kinetics

Collision Theory

15. Chemical Kinetics

Collision Theory

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Collision Theory Concept 1

Collision Theory Example 1

Collision Theory Concept 2

Collision Theory Example 2

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Collision theory | Kinetics | AP Chemistry | Khan Academy

08:48

Collision theory | Kinetics | AP Chemistry | Khan Academy

Khan Academy Organic Chemistry

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14.4 Collision Theory and the Arrhenius Equation

12:57

14.4 Collision Theory and the Arrhenius Equation

Introduction to Collision Theory

Energy Diagrams, Catalysts, and Reaction Mechanisms

Professor Dave Explains

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Textbook Question

What must happen before a chemical reaction can begin?

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Textbook Question

(a) What factors determine whether a collision between two molecules will lead to a chemical reaction?

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Textbook Question

(b) Does the rate constant for a reaction generally increase or decrease with an increase in reaction temperature?

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Textbook Question

Indicate whether each statement is true or false. (c) Increasing the reaction temperature increases the fraction of successful collisions between reactants.

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Textbook Question

Indicate whether each statement is true or false. (c) If you double the temperature for a reaction, you cut the activation energy in half.

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Textbook Question

Indicate whether each statement is true or false. (a) If you measure the rate constant for a reaction at different temperatures, you can calculate the overall enthalpy change for the reaction.

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Textbook Question

Based on their activation energies and energy changes and assuming that all collision factors are the same, rank the following reactions from slowest to fastest. (a) Ea = 45 kJ>mol; E = -25 kJ>mol (b) Ea = 35 kJ>mol; E = -10 kJ>mol (c) Ea = 55 kJ>mol; E = 10 kJ>mol

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Textbook Question

Why don't all collisions between reactant molecules lead to a chemical reaction?

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Textbook Question

Two reactions have the same activation energy, but their rates at the same temperature differ by a factor of 10. Explain.

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Textbook Question

When the temperature of a gas is raised by 10 °C, the collision frequency increases by only about 2%, but the reaction rate increases by 100% (a factor of 2) or more. Explain.

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Textbook Question

What fraction of the molecules in a gas at 300 K collide with an energy equal to or greater than Ea when Ea equals 50 kJ/mol? What is the value of this fraction when Ea is 100 kJ/mol?

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Textbook Question

This reaction has an activation energy of zero in the gas phase: CH3 + CH3¡C2H6 a. Would you expect the rate of this reaction to change very much with temperature?

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Textbook Question

Consider the two reactions: O + N2¡NO + N Ea = 315 kJ>mol Cl + H2¡HCl + H Ea = 23 kJ>mol b. The frequency factors for these two reactions are very close to each other in value. Assuming that they are the same, calculate the ratio of the reaction rate constants for these two reactions at 25 °C.

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Textbook Question

Consider the two reactions: O + N2¡NO + N Ea = 315 kJ>mol Cl + H2¡HCl + H Ea = 23 kJ>mol a. Why is the activation barrier for the first reaction so much higher than that for the second?

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Textbook Question

The gas-phase reaction of NO with F2 to form NOF and F has an activation energy of Ea = 6.3 kJ>mol. and a frequency factor of A = 6.0 * 108 M-1 s-1. The reaction is believed to be bimolecular: NO1g2 + F21g2 ¡ NOF1g2 + F1g2 (e) Suggest a reason for the low activation energy for the reaction.

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Open Question

What must happen before a chemical reaction can begin? The activation energy must be exceeded. The activation energy must be reached. The concentrations of products and reactants must be equal. The concentration of reactant molecules must be reduced.

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Open Question

What factors determine whether a collision between two reactant molecules will result in a reaction?

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Open Question

What must happen before a chemical reaction can begin?

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Open Question

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