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chem Flashcards

1
Q

Exothermic Reaction

A

Gives out energy to the surroundings usually in the form of heat

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2
Q

Endothermic Reaction

A

Takes energy from its surroundings in the form of heat, showing a fall in temp

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3
Q

reaction profiles?

A

are diagrams that show the relative energies of the reactants and products in a reaction, it also shows how energy changes over time

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4
Q

Activation energy, also known as…

A

Ea

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5
Q

Activation energy?

A

minimum amount of energy the reactants need to collide with each other and react.

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6
Q

Exothermic reactions in reaction profiles?

A

products are at a lower energy than the reactants

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7
Q

Endothermic reactions in reaction profiles?

A

products are at a higher energy than the reactants because the energy is taken in.

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8
Q

Enthalpy change in Exothermic Reactions?

A

Negative

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9
Q

Enthalpy change in Endothermic?

A

Postitive

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10
Q

Enthalpy Change?

A

amount of heat evolved or absorbed in a reaction carried out at constant pressure.

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11
Q

Rate of reaction dependencies?

A

1) temp
2) concentration of a solution or pressure of gas
3) Surface area, changes are dependant of the size of the solid
4) Presence of a catalyst

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12
Q

what does more collisions do to the rate of reactions?

A

It gets it higher

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13
Q

name 4 things that increase the rate of reactions?

A

1) higher temp
2) higher concentration/pressure
3) Catalysts
4) Smaller solid particles combining more Surface Area

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14
Q

reactions only happen if…

A

particles collide with enough energy

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15
Q

In gas, what does it mean by increasing the pressure?

A

getting the particles to be more crowded, frequency of collisions will increase.

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16
Q

What happens if a solution is made more concentrated

A

It means there are more particles of reactant in the same volume

17
Q

What will increase when a solid is breaking into smaller pieces?

A

Surface area

18
Q

A catalyst is a substance which increases the rate of a reaction without…

A

being chemically changed or used up in the reaction.

19
Q

will a catalyst change the products of a reaction?

A

No, so the reaction equation will stay the same.
Because it isn’t used up, you can use catalysts for large amounts of reactants.

20
Q

Do Catalysts work with all reactions?

A

No.

21
Q

How do catalysts work?

A

They decrease the activation energy for a reaction to occur, making it quicker. They do this by providing an alternative reaction pathway that has a lower activation energy

22
Q

What does a catalyst do to the particles?

A

more of the particles will have the minimum amount of energy needed for a reaction to occur when particles collide.

23
Q

What substances make great fuels?

A

Hydrocarbons.

24
Q

Is burning a combustion reaction?

A

Yes.

25
Q

What energy does fuel release when burning?

A

Heat.

26
Q

Why do Hydrocarbons make great fuels

A

When you burn them in oxygen, they give out lots of heat energy. This is a very exothermic reaction.

27
Q

Combustion Equation?

A

hydrocarbon + oxygen –> carbon dioxide + water

28
Q

What is the process called when there isn’t enough oxygen around for a complete combustion reaction.

A

Incomplete combustion.

29
Q

The products of incomplete combustion contain ___________ than carbon dioxide.

A

less oxygen.

30
Q

What does an incomplete combustion produce?

A

carbon monoxide and Soot.

31
Q

What is produced when crude oil is burnt?

A

Sulfur dioxide, nitrogen oxides. (these MAY be produced).

32
Q

How are nitrogen oxides created?

A

When the temp is high enough for the nitrogen and oxygen in the air to react.

33
Q

Nitrogen oxides include… and …

A

nitrogen monoxide (NO) and nitrogen dioxide (NO2).

34
Q

What forms when sulfur dioxide and nitrogen oxides mix with water vapor in the clouds?

A

dilute sulfuric acid and nitric acid.

35
Q

What will you get if you heat a metal carbonate?

A

carbon dioxide and metal oxide.

36
Q

Thermal decomposition?

A

a substance breaks down into simpler substances when heated.

37
Q

Copper Carbonate(II) thermal decomposition and equation?

A

Copper(II) carbonate is a green powder that will easily decompose to form carbon dioxide and copper(II) oxide when you heat it.

Equation: CuCO3 (s) –> CuO (s) + CO2(g)

To do the experiment, heat copper(II) carbonate then collect the gas that’s given off in a test tube.

The gas that is collected can then be tested to see if it is CO2 using limewater.

38
Q

First 5 Hydrocarbons

A

1) Methane
2) Ethane
3) Propane
4) Butane
5) Pentane

39
Q

First 5 Hydrocarbons

A

1) Methane
2) Ethane
3) Propane
4) Butane
5) Pentane

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