Rate Equations Flashcards

1
Q

What is the general form of a rate equation?

A

Rate = k [A]^m [B]^n, where k is the rate constant, [A] and [B] are concentrations of reactants, and m and n are their orders.

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2
Q

What does the rate constant (k) represent?

A

The rate constant k links the rate of reaction to the concentrations of reactants. It is constant at a given temperature.

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3
Q

What is meant by the order of a reaction?

A

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

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4
Q

How do you determine the overall order of a reaction?

A

By adding the powers (orders) of all reactants in the rate equation: overall order = m + n.

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5
Q

What are the units of the rate constant k?

A

Units depend on the overall order of the reaction. They are derived by rearranging the rate equation to make k the subject.

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6
Q

What is the unit of k for a first-order reaction?

A

s⁻¹

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7
Q

What is the unit of k for a second-order reaction?

A

mol⁻¹ dm³ s⁻¹

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8
Q

What is the unit of k for a third-order reaction?

A

mol⁻² dm⁶ s⁻¹

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9
Q

How is the rate of reaction determined experimentally?

A

By measuring the change in concentration of a reactant or product over time.

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10
Q

How do you determine the order of a reaction from experimental data?

A

By varying the concentration of one reactant while keeping others constant and measuring the effect on the rate.

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11
Q

What is a concentration–time graph?

A

A graph that shows how the concentration of a reactant changes with time.

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12
Q

What is a rate–concentration graph?

A

A graph showing how the rate of reaction changes with changing reactant concentration.

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13
Q

What does a straight line through the origin on a rate–concentration graph show?

A

First-order with respect to that reactant (rate ∝ [A]).

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14
Q

What does a horizontal line on a rate–concentration graph show?

A

Zero-order with respect to that reactant (rate is independent of [A]).

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15
Q

What does a curved line on a rate–concentration graph show?

A

Second-order with respect to that reactant (rate ∝ [A]²).

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16
Q

What is the initial rate of a reaction?

A

The rate at the very start of a reaction, where t = 0.

17
Q

How is initial rate determined from a concentration–time graph?

A

By drawing a tangent at t = 0 and finding its gradient.

18
Q

What is a clock reaction?

A

A method of measuring the initial rate by timing how long it takes for a visible change (like color change) to occur.

19
Q

What assumption is made in a clock reaction?

A

That the average rate over the time measured is approximately equal to the initial rate.

20
Q

What is the rate-determining step?

A

The slowest step in a multi-step reaction mechanism that limits the overall rate.

21
Q

How can you identify the rate-determining step from a rate equation?

A

Only species present in the rate equation appear in the rate-determining step.

22
Q

How can you propose a reaction mechanism from a rate equation?

A

Use the order of each reactant to deduce which molecules are involved in the rate-determining step.

23
Q

How does temperature affect the rate constant k?

A

As temperature increases, k increases exponentially due to more molecules having energy ≥ activation energy.

24
Q

How is the Arrhenius equation written?

A

k = Ae^(-Ea/RT), where A is the frequency factor, Ea is activation energy, R is the gas constant, and T is temperature in Kelvin.

25
Q

How can the Arrhenius equation be used in the form of a straight-line graph?

A

ln k = -Ea/R × (1/T) + ln A — plot ln k against 1/T to get a straight line with gradient -Ea/R and y-intercept ln A.

26
Q

What is the significance of the Arrhenius plot?

A

It allows determination of activation energy and frequency factor from experimental data.