Rates of Reaction Flashcards

1
Q

Activation Energy

A

the minimum amount of energy needed for a reaction to happen

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2
Q

Catalyst

A

speeds up a reaction without being used in the reaction itself, lowers the activation energy, causing a higher proportion of successful collisions

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3
Q

Collision Theory

A

explains why rate of reaction changes, states that particles must collide before a reaction takes place and if there is a collision, it might take place, but not all collisions lead to reactions because they need energy in order to react, and reactants must have the activation energy in order to react

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4
Q

Cocentration

A

increasing the particles per unit volume causes more frequent collisions

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5
Q

Mean Rate of Reaction

A

quantity of reactant used / time or quantity of reactant formed / time

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6
Q

Metabolism

A

the sum of all the reactions in the body

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7
Q

Pressure

A

increasing the particles per unit volume causes more frequent collisions

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