Rate Equations Flashcards

1
Q

What does a rate equation show

A

How changes in the concentrations of reactants affect the rate of reaction, shows the molecules that are reactants in rate determining step (slowest)

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2
Q

What does each letter stand for in rate=k[A]^x[B]^y

A

-constant k is rate constant
-[A] and [B] represent the concentrations of reactants in mol/dm3
-powers x and y are the reaction orders with respect to A and B in equation

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3
Q

What is the overall order of a reaction

A

The sum of the orders for all the substances that appear in the rate equation

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4
Q

What does factor does rate constant (k) vary with

A

Temperature

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5
Q

What is a first order reactant

A

Reaction is first order with respect to a reactant if the rate of reaction is proportional to concen of that reactant, raised to power one in the rate equation

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6
Q

What type of line is on graph for first order reaction for concen rate

A

Straight line passing through the origin

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7
Q

What is the half-life of a reaction

A

The time for the concentration of one of the reactants to fall by half

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8
Q

What is a second order reactant

A

If the rate of reaction is proportional to the concentration of that reaction squared, raised to the power two in the rate equation for that reactant

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9
Q

What does doubling concentration of X raised to power 2 in rate equation do to rate

A

Increases rate by factor of four

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10
Q

What does concentration-time graph look like for second order reaction and how to find gradient

A

Curve, draw tangents to curve to find gradient

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11
Q

What is a zero order reaction and what does concentration-rate graph look like

A

When concentration of that reactant does not affect the rate of reaction, raised to the power zero
-graph is straight line across

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12
Q

What do the units of the rate constant depend on

A

The overall order of the reaction

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13
Q

Does the half-life of a first order reaction change depending on starting concentration

A

No it is the same whatever the starting concentration

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14
Q

How to find the half-life of a second order reaction

A

Half-life is inversely proportional to the starting concentration

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15
Q

If reactant involved in mechanism after rate determining step what is its order and what about before

A

Zero, if before either first or second

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16
Q

Units of rate constant for zero order reaction

A

mol dm^-3 s^-1

17
Q

Units of rate constant for first order reaction

18
Q

Units for rate constant for second order reaction

A

Mol^-1 dm^3 s^-1

19
Q

Units for rate constant for third order reaction

A

Mol^-2 dm^6 s^-1

20
Q

How to get units for rate constant

A

Rearrange to get rate/concens and unit for rate is moldm^-3 s^-1

21
Q

What do concentration time graphs look like for first and second order reactions

22
Q

Is half life constant throughout first order reaction

23
Q

How are rate equations determined

A

Experimentally, cannot be found from stoichiometric equations

24
Q

What does and doesn’t feature in the rate equation

A

Products and catalysts may feature in rate equations but intermediates do not feature (generated in slowest step and reactants in another step)

25
What is the overall order of reaction
The sum of the powers of the reactants in a rate equation
26
Why wouldn’t clock reaction be order of reaction with respect to iodide ions as 5
Because the chance of five or more ions colliding in rate determining step is negligible