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Chemistry > Chemistry unit 5+6 > Flashcards

Chemistry unit 5+6 Flashcards

1
Q

Formula for rate of reaction

A

Amount of reactant used/ time or amount of product formed/time

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2
Q

How do we measure the quanitity of the mass and product

A

In g of cm^3 or in moles

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3
Q

How is rate measured

A

In g/s or cm^3/s or in mol/s

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4
Q

How to find rate of reaction from a graph

A

Draw a tangent at the point on the curve and draw a triangle and then use the equation to work out gradient

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5
Q

Factors affecting rate of chemical reactions

A

Concentration
Pressure
Surface area
Temperature
Catalysts

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6
Q

Defined collision theory

A

Chemical reactions can only occur only when reacting particles collide with each other and with sufficient energy

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7
Q

What is activation energy

A

The minimum amount of energy needed that particles must have to react

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8
Q

Explain how temperature increases reaction rate

A

Higher temperatures = more energy so more frequent collisions leading to quicker reaction

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9
Q

Explain how concentration affects rate of reaction

A

More particles in as smaller area means more frequent collisions so more particles reach activation energy and a quicker rate of reaction

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10
Q

What is a catalyst

A

A substance that can provide an alternate pathway for a reaction in order to decrease activation energy so more particles get the activation energy necessary and increase rate of reaction without being used up

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11
Q

What is a reversible reaction

A

When the products of the reaction react to make the reactants. We use the reversible reactions arrow to show this

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12
Q

Energy changes in reversible reactions

A

A reversible reaction being exothermic one way is endothermic the other way

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13
Q

What three things need to go on a reaction profile graph

A

Overall energy change
Activation energy
Reactant and products

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14
Q

What is an exothermic reaction

A

A reaction where bonds are built up and and energy is released to its surroundings

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15
Q

What is an endothermic reaction

A

A reaction where bonds are broken down and energy is absorbed through into its surroundings.

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16
Q

What do we call the reactions plus products

A

The system (the surroundings are everything else)

16
Q

What does an exothermic reaction profile show us

A

More energy is released when new bonds are formed then the energy absorbed when bonds pare broken

17
Q

What does an endothermic reaction profile show us

A

More energy is absorbed to break the bonds than the energy released when building the bonds

18
Q

What are the uses of an exothermic reaction

A

Hand-warmers that are both single use and reusable by making it with materials that form a reversible reaction, self heating cans that use calcium oxide

19
Q

What are the uses of endothermic reactions

A

Ice packs with ammonium nitrate that numb pain, keeping drink containers to keep them cool

19
Q

What is a bond energy calculation

A

The calculation that shows the change in energy from reactions to products

20
Q

What is dynamic equilibrium

A

When the rate of the forward and reverse reactions are equal, the system is at dynamic equilibrium. The reaction is constantly moving making it dynamic

21
Q

What is le chatiliers principle

A

If conditions in the system are changed, the reaction will try to oppose change to restore the dynamic equilibrium

22
Q

What happens when a reaction at dynamic equilibrium increases in concentration of reactants

A

More product gets produced the balance the equilibrium’s

23
Q

What happens when a reaction at dynamic equilibrium decreases in concentration in products

A

Less reactant gets produced to balance the equilibrium

24
Q

When temperature increases in a substance at dynamic equilibrium what happens

A

Moves in the direction of the endothermic reaction( whether endothermic is forward or reverse

25
Q

When temperature decreases in a substance at dynamic equilibrium what happens

A

Moves in the direction of the exothermic reaction( whether exothermic is forward or reverse

26
Q

When pressure increases in a reaction at dynamic equilibrium what happens

A

Equilibrium moves to the side with less moles

27
Q

When pressure decreases in a reaction at dynamic equilibrium what happens

A

The equilibrium moves to the side with more moles

Chemistry (10 decks)

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