Year 12- Kinetics (Physical Chemistry) Flashcards

1
Q

What is collision theory?

A

Reactions can only occur when successful collisions occur between particles with activation energy.

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2
Q

What is activation energy?

A

The minimum energy which particles need to collide to start a reaction

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3
Q

What is the effect of increasing temperature on the maxwell-botlzmann curve?

A

The Emp and mean energy shift to higher energy values, but eh no. of molecules with those energies decrease.
-The curve shifts to the right, becomes shorter but the line stays above the og curve.

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4
Q

What is the rate of reaction?

A

The change in concentration of a substance in unit time. Units are mol dm-3 s-1.

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5
Q

How do you calculate rate of reaction from a curve?

A

Drawing a tangent to the curve and calculate its gradient.

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6
Q

When is reaction rate measured using 1/time? Explain why.

A

In the experiment between sodium thiosulfate and hydrochloric acid. Time is the amount taken for a cross underneath to disappear due to the cloudiness of sulfur.
-Due to concentration not being included. We assume the amount of sulfur is fixed and constant.

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7
Q

What is the effect of increasing concentration/ pressure on the rate of reaction?

A

There are more particles per unit volume so they collide with greater frequency and there will be higher frequency of successful collisions.

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8
Q

How does maxwell-boltzmann’s curve change with increased concentration/pressure?

A

The curve is raised higher as there are more particles so a greater area but the shape remains the same.
-More molecules have energy greater than the activation energy.

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9
Q

Effect of increasing surface area on the rate of reaction

A

-Causes successful collisions to be more frequent which increases rate of reaction

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10
Q

Effect of a catalyst on the rate of reaction

A

They increase the rate of reaction by providing an alternative pathway with a lowered activation energy. More particles have energy greater than the activation energy so there will be higher frequency of successful collisions.

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