Kinetics Flashcards

1
Q

What is the definition of the rate of reaction?

A

The rate of reaction is the change in concentration of a reactant or product per unit time, usually measured in mol dm⁻³ s⁻¹.

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2
Q

How can the rate of a reaction be calculated?

A

Rate = change in concentration ÷ time, or expressed mathematically as: rate = Δ[concentration] ÷ Δtime.

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3
Q

What does collision theory state?

A

Collision theory states that particles must collide with sufficient energy (activation energy) and with the correct orientation for a reaction to occur.

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4
Q

What is activation energy?

A

Activation energy (Ea) is the minimum amount of energy that colliding particles need to have for a reaction to occur.

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5
Q

How does increasing temperature affect the rate of reaction?

A

Increasing temperature increases the kinetic energy of particles, leading to more frequent and successful collisions, which increases the rate of reaction.

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6
Q

Why does increasing the concentration of reactants increase the rate of reaction?

A

Higher concentration means more particles per unit volume, leading to more frequent collisions and a higher chance of successful collisions.

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7
Q

How does increasing pressure affect the rate of a reaction involving gases?

A

Increasing pressure forces gas particles closer together, increasing the frequency of collisions and hence increasing the rate of reaction.

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8
Q

What effect does a catalyst have on the rate of reaction?

A

A catalyst provides an alternative reaction pathway with a lower activation energy, increasing the rate of reaction without being used up.

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9
Q

How do catalysts affect the energy distribution of particles?

A

Catalysts lower the activation energy, so a greater proportion of particles have sufficient energy to overcome the activation barrier and react successfully.

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10
Q

What is the Maxwell-Boltzmann distribution?

A

The Maxwell-Boltzmann distribution shows the distribution of energies of molecules in a gas at a given temperature.

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11
Q

Why does the Maxwell-Boltzmann distribution start at the origin?

A

No particles have zero energy, so the graph starts at the origin (0,0).

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12
Q

How does temperature affect the Maxwell-Boltzmann distribution?

A

At higher temperatures, the curve shifts to the right, becomes flatter, and more particles have energy greater than the activation energy.

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13
Q

What happens to the area under the curve in a Maxwell-Boltzmann distribution when temperature increases?

A

The area under the curve remains the same because it represents the total number of particles, which does not change.

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14
Q

Why does a small increase in temperature cause a large increase in reaction rate?

A

A small increase in temperature significantly increases the number of particles with energy greater than the activation energy, resulting in more successful collisions.

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15
Q

What is a heterogeneous catalyst?

A

A heterogeneous catalyst is in a different phase from the reactants, typically a solid catalyst with gaseous or liquid reactants.

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16
Q

What is a homogeneous catalyst?

A

A homogeneous catalyst is in the same phase as the reactants, often forming an intermediate species.

17
Q

What is a rate equation?

A

The rate equation shows how the rate of reaction depends on the concentration of reactants. It is of the form: Rate = k[A]ᵐ[B]ⁿ, where m and n are the orders.

18
Q

What is the rate constant (k)?

A

The rate constant (k) is a proportionality constant that links the rate of reaction to the concentration of reactants raised to their respective powers.

19
Q

How is the overall order of a reaction determined?

A

The overall order of a reaction is the sum of the powers of the concentration terms in the rate equation (m + n).

20
Q

What is the order of reaction with respect to a reactant?

A

The order of reaction with respect to a reactant is the power to which its concentration is raised in the rate equation.

21
Q

How does the rate of reaction change in a zero-order reaction?

A

In a zero-order reaction, the rate is independent of the concentration of the reactant. Rate = k.

22
Q

How does the rate of reaction change in a first-order reaction?

A

In a first-order reaction, the rate is directly proportional to the concentration of the reactant. Rate = k[A].

23
Q

How does the rate of reaction change in a second-order reaction?

A

In a second-order reaction, the rate is proportional to the square of the concentration of the reactant. Rate = k[A]².

24
Q

How can the order of a reaction be determined experimentally?

A

The order of reaction can be determined by the initial rates method or by plotting concentration-time graphs and analyzing the gradients.

25
Q

What is a half-life (t₁/₂) in the context of reaction kinetics?

A

The half-life is the time taken for the concentration of a reactant to halve.

26
Q

What is the characteristic of a first-order reaction in terms of half-life?

A

A first-order reaction has a constant half-life, independent of concentration.

27
Q

How can rate constants be calculated from half-life data?

A

For a first-order reaction: k = ln(2) ÷ t₁/₂.

28
Q

What is the Arrhenius equation?

A

The Arrhenius equation is: k = Ae^(-Ea/RT), where k is the rate constant, A is the pre-exponential factor, Ea is the activation energy, R is the gas constant, and T is temperature in Kelvin.

29
Q

How does a graph of ln(k) against 1/T relate to the Arrhenius equation?

A

A graph of ln(k) against 1/T gives a straight line with a gradient of -Ea/R and an intercept of ln(A).

30
Q

What is the significance of the pre-exponential factor (A) in the Arrhenius equation?

A

The pre-exponential factor accounts for the frequency of collisions and the orientation of reactants, representing the maximum possible rate if all collisions were successful.

31
Q

How can the rate of a reaction be measured experimentally?

A

The rate can be measured by monitoring changes in reactant or product concentrations over time using methods like gas volume, mass change, or color change.

32
Q

How can gas volume be used to measure rate?

A

The volume of gas produced is measured over time using a gas syringe.

33
Q

How can mass loss be used to measure rate?

A

The decrease in mass is measured when a gas is released, often using a balance.

34
Q

How can color change be used to measure rate?

A

A colorimeter is used to measure the change in absorbance during a reaction involving colored species.

35
Q

How can pH change be used to measure rate?

A

A pH meter is used to monitor changes in pH during acid-base reactions.

36
Q

How can time for a precipitate to form be used to measure rate?

A

The time taken for a cross to disappear when a precipitate forms can be measured.

37
Q

How can titration be used to measure rate?

A

Samples are taken at regular intervals, quenched, and titrated to determine the concentration of a reactant or product over time.