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Slide 1
Slide 2
A _________ is a substance that speeds up a chemical reaction
without being permanently consumed in the reaction. catalyst
Slide 3
List the naturally occurring diatomic molecules. H 2, O 2, N 2,
Cl 2, Br 2, I 2, F 2
Slide 4
Using collision theory, EXPLAIN why increasing the temperature
of a reaction increases the reaction rate? Increasing the
temperature also increases the kinetic energy of the reacting
molecules. So molecules are moving faster and will collide more
often. More collisions = faster reaction rate!
Slide 5
_____________ is the speed of the disappearance of a reactant
or the rate of the appearance of a product in a chemical reaction.
Reaction rate
Slide 6
Equations must always be balanced because a certain law of
chemistry cannot be violated. What is the name of the law that
cannot be violated? Law of Conservation of Matter
Slide 7
The arrow between the reactants and products means__________.
yields
Slide 8
List the four indicators that a chemical reaction occurred.
Heat/light Precipitate Gas (bubbles) Color change
Slide 9
In a chemical equation, what is indicated by the symbol? Heat
is added to the reaction
Slide 10
In a chemical equation, what is indicated by the symbol? A
precipitate is formed
Slide 11
What are the 4 factors that affect the reaction rate?
Temperature Concentration Nature of Reactants Catalyst
Slide 12
List the reactants in the following equation: CH 4 (g) + 2O 2
(g) CO 2 + 2H 2 O ( l ) CH 4 + 2O 2
Slide 13
Using collision theory, EXPLAIN why increasing the
concentration of a reactant increases the reaction rate? More
molecules are present as the concentration is increased. So more
molecules present equals more collisions between reacting
molecules. More collisions = faster reaction rate!
Slide 14
In a chemical equation, what is indicated by the H 2 SO 4
symbol? That H 2 SO 4 was used as a catalyst is this reaction
Slide 15
List the products in the following equation: CH 4 (g) + 2O 2
(g) CO 2 + 2H 2 O ( l ) CO 2 + 2H 2 O
Slide 16
How many atoms of O are in 2H 2 O following equation: CH 4 (g)
+ 2O 2 (g) CO 2 + 2H 2 O ( l ) 2
Slide 17
What is does the represent in the following equation: 2H 2 + O
2 2H 2 O A reversible reaction. The reaction can go both ways-
reactants yield products and product can yield reactants
Slide 18
What type of reaction would the following be classified as? AB
+ CD AD + CB Double displacement
Slide 19
Suppose in the following reaction that 10g of Mg was added to
14g of O 2, how many grams of MgO would be produced? 2Mg (s) + 2O 2
(g) 2MgO (s) 24 g b/c the Law of Conservation of Matter (the amount
of matter you start with is the same amount that you end
with!)
Slide 20
How many atoms of C are in CO 2 following equation: CH 4 (g) +
2O 2 (g) CO 2 + 2H 2 O ( l ) 1
Slide 21
How many moles of CH 4 are present following equation: CH 4 (g)
+ 2O 2 (g) CO 2 + 2H 2 O ( l ) 1
Slide 22
What ions are present for H 2 0? H+ and OH-
Slide 23
How many molecules of 2O 2 are present following equation: CH 4
(g) + 2O 2 (g) CO 2 + 2H 2 O ( l ) 2
Slide 24
Which of the following substances would be a gas that is
produced in the following equation: CH 4 (g) + 2O 2 (g) CO 2 + 2H 2
O ( l ) CO 2
Slide 25
What type of reaction would the following be classified as? A +
B AB Synthesis
Slide 26
Which type of reaction has only one REACTANT?
Decomposition
Slide 27
What type of reaction would the following be classified as? A +
BC AC + B Single displacement
Slide 28
Which of the following substances would be a liquid in the
following equation: CH 4 (g) + 2O 2 (g) CO 2 + 2H 2 O ( l ) 2H 2
O
Slide 29
How many molecules of CH 4 are present following equation: CH 4
(g) + 2O 2 (g) CO 2 + 2H 2 O ( l ) 1
Slide 30
What ion is ALWAYS present in any acid? H+
Slide 31
Which type of reaction has only one PRODUCT being produced?
Synthesis
Slide 32
What does (aq) represent after a substance? Aqueous substance
was dissolved in water
Slide 33
Is the following reaction correct? Explain. 2Mg (s) + 2O 2 (g)
2PbO (s) NO! b/c the Law of Conservation of Matter (the same types
of atoms must be present on both sides of the equation. Mg cant be
changed into Pb!
Slide 34
What type of reaction would the following be classified as? AB
A + B Decomposition
Slide 35
Balance the following equation: potassium + water potassium
hydroxide + hydrogen 2K + 2H 2 O 2KOH + H 2
Slide 36
Balance the following equation: fluorine + aluminum oxide
aluminum fluoride + oxygen 6F 2 + 2Al 2 O 3 4AlF 3 + 3O 2
Slide 37
Identify the type of reaction. Finish the word equation &
write the balanced equation: Aluminum + hydrochloric acid Single
Displacement Aluminum chloride + hydrogen 2Al + 6HCl 2AlCl 3 + 3H
2
Slide 38
Identify the type of reaction. Finish the word equation &
write the balanced equation: calcium fluoride + water Double
Displacement Calcium hydroxide + hydrogen fluoride CaF 2 + 2H 2 O
Ca(OH) 2 + 2HF
Slide 39
Identify the type of reaction. Finish the word equation &
write the balanced equation: potassium oxide Decomposition
potassium + oxygen 2K 2 O 4K + O 2
Slide 40
Identify the type of reaction. Finish the word equation &
write the balanced equation: strontium + chlorine synthesis
Strontium chloride Sr + Cl 2 SrCl 2 *Balanced