kinetics (physical) Flashcards

1
Q

What must particles do in order to react?

A

Collide with enough energy (activation energy) and the correct orientation

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2
Q

Do most collisions end in a reaction

A

no

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3
Q

Define activation energy

A

The minimum energy needed for particles to collide to form a reaction

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4
Q

What is the effect of increasing temperature on the rate of reaction? Why?

A

Increasing temperature = increased rate of reaction because when the particles get hotter, particles have more energy and move faster so they collide more often

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5
Q

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

A

Increased concentration/pressure = increased rate of reaction because there are more particles/smaller area so the particles are more likely to collide with eachother.

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6
Q

What is a catalyst?

A

A substance which increases the rate of reaction but is not actually used up

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7
Q

How do catalysts work and how do they increase the rate of reaction?

A

They provide an alternative reaction pathway (one with a lower activation energy)
Lowers the activation energy so more particles have energy and therefore there are more frequent collisions so there is an increased reaction rate

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