11A - Kinetic Rates Flashcards

1
Q

What does the rate of reaction refer to?

A

The change in the amount or concentration of a reactant or product per unit time.

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2
Q

What are the units for the rate of reaction?

A

mol dm^-3 s^-1.

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3
Q

What are the methods to measure the rate of reaction?

A

-Mass lost over time.
- Volume of product produced over time.
- Color changes, including by the use of colorimetry.
- pH changes over time.
- Changes in electrical conductivity.

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4
Q

How can the rate of reaction be calculated?

A

Rate of reaction (mol dm^-3 s^-1) = Δ[Reactants/Products] / Δtime
When reactants are used, a negative sign needs to be used so that final rate value is positive.

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5
Q

Why cannot the method of change in mass over time be used for an experiment releasing hydrogen gas?

A

Hydrogen has a low relative molecular formula so the mass changes over time will be very small leading to significant measurement uncertainties.

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6
Q

What are the advantages of using a gas syringe than collecting over water into measuring cylinder?

A
  • There’s a greater degree of precision in gas syringes.
  • Some gases are water soluble such as SO2 so you can only use a gas syringe.
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7
Q

What are the advantages of using method of collecting over water into measuring cylinder than gas syringe?

A
  • If the gas volume is large, then difference of degree of measurement uncertainty becomes too small.
  • The water in measuring cylinder can be saturated with the gas that will be collected so that it won’t dissolve in it.
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8
Q

What is the rate expression for a directly proportional relationship between rate and concentration?

A

Rate ∝ [D] or Rate = k[D].

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9
Q

What does the rate expression Rate = k[D] mean?

A

It means that if the concentration of D is doubled, the rate doubles; if concentration halves, the rate also halves.

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10
Q

What is the rate equation for the reaction A (aq) + B (aq) → C (aq) + D (g)?

A

Rate of reaction = k[A]^m[B]^n.

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11
Q

How are rate equations determined?

A

Rate equations can only be determined experimentally and cannot be found from the stoichiometric equations. This is due to the following reasons:
Complex Reaction Mechanisms
Reaction Orders
Rate constants
Catalyst and Reaction Conditions

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12
Q

What do [A] and [B] represent in the rate equation Rate = k[A]^m[B]^n?

A

[A] and [B] are the concentrations of the reactants.

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13
Q

What do m and n represent in the rate equation Rate = k[A]^m[B]^n?

A

m and n are orders with respect to each reactant involved in the reaction.

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14
Q

Can products and catalysts feature in rate equations?

A

Yes, products and catalysts may feature in rate equations.

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15
Q

Do intermediates feature in rate equations?

A

No, they don’t.

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