Chem -6 Flashcards

1
Q

What is rate of reaction

A

A measure of how quickly a reactant is used up or a product is formed

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2
Q

What is needed for a chemical reaction to happen

A

Reactant particle must collide together
And the particles must have enough energy to react

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3
Q

What is activation energy

A

The minimum amount of energy needed for a collision to be successful

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4
Q

What happens to catalyst at the end of a reaction

A

Nothing

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5
Q

What will increase the proportion of successful collisions

A

Increasing the temperature and surface area

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6
Q

Would would speed up a reaction

A

Pressure , concentration or catalyst

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7
Q

What is a reversible reaction

A

The products of the reaction can react together to produce the original reactants

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8
Q

How can the position is equilibrium be changed (le chateliers principle)

A

Change in pressure, concentration and temperature

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9
Q

What has the smallest surface area to volume ratio

A

Large lumps

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10
Q

What happens if a large lumps is divided or ground into powder

A

-total volume stays the same
-area of exposed surface increases
- the surface area to volume ratio increases

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11
Q

What is better at increasing frequency of successful collisions and why
(Lumps or powders)

A

Powders because they have a higher surface area to volume ratio so
-more reactant particles are exposed at the surface
-the frequency of successful collisions are increased
- rate of reaction increases

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12
Q

How do catalyst increase rate of reaction

A

Provide alternative pathway with lower activation energy

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13
Q

How does temp, pressure, concentration and surface area increase rate of reaction and successful collision rate

A

They increase the frequency of particles colliding their for more chance of the collisions being successful and speeding up a reaction

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