Unit 7 Reactions Exam Review. Question 1 Potassium Calcium Sodium Magnesium Aluminum Lead Copper Mercury Silver Which metals would be replaced in a solution.

Unit 7 Reactions Exam Review

Question 1 Potassium Calcium Sodium Magnesium Aluminum Lead Copper Mercury Silver Which metals would be replaced in a solution made from one of their compounds, if a piece of lead metal were added?

Question 1 Potassium Calcium Sodium Magnesium Aluminum Lead Copper Mercury Silver Which metals would be replaced in a solution made from one of their compounds, if a piece of lead metal were added? Copper, Mercury, Silver

Question 2 Potassium Calcium Sodium Magnesium Aluminum Lead Copper Mercury Silver You have a mixture that contains solutions of both Sodium and Aluminum compounds. You wish to ‘recover’ the aluminum but not the sodium. What other metal should you add to this mixture?

Question 2 Potassium Calcium Sodium Magnesium Aluminum Lead Copper Mercury Silver You have a mixture that contains solutions of both Sodium and Aluminum compounds. You wish to ‘recover’ the aluminum but not the sodium. What other metal should you add to this mixture? Magnesium

Question 3 Potassium Calcium Sodium Magnesium Aluminum Lead Copper Mercury Silver Which metals would be replaced in a solution made from one of their compounds, if a piece of sodium metal were added?

Question 3 Potassium Calcium Sodium Magnesium Aluminum Lead Copper Mercury Silver Which metals would be replaced in a solution made from one of their compounds, if a piece of sodium metal were added? All of them except Potassium and Calcium – Sodium and below

Question 4 Potassium Calcium Sodium Magnesium Aluminum Lead Copper Mercury Silver Which of the metals listed above could NOT then be used to remove the mercury from a nitrate solution?

Question 4 Potassium Calcium Sodium Magnesium Aluminum Lead Copper Mercury Silver Which of the metals listed above could NOT then be used to remove the mercury from a nitrate solution? Silver

Question 5 List the types of reactions and write examples of each using the letters A, B, etc.

Question 5 List the types of reactions and write examples of each using the letters A, B, etc. Synthesis

Question 5 List the types of reactions and write examples of each using the letters A, B, etc. SynthesisA + B  AB

Question 5 List the types of reactions and write examples of each using the letters A, B, etc. SynthesisA + B  AB Decomposition

Question 5 List the types of reactions and write examples of each using the letters A, B, etc. SynthesisA + B  AB DecompositionAB  A + B

Question 5 List the types of reactions and write examples of each using the letters A, B, etc. SynthesisA + B  AB DecompositionAB  A + B Single Replacement

Question 5 List the types of reactions and write examples of each using the letters A, B, etc. SynthesisA + B  AB DecompositionAB  A + B Single Replacement AB + C  AC + B

Question 5 List the types of reactions and write examples of each using the letters A, B, etc. SynthesisA + B  AB DecompositionAB  A + B Single Replacement AB + C  AC + B Double Replacement

Question 5 List the types of reactions and write examples of each using the letters A, B, etc. SynthesisA + B  AB DecompositionAB  A + B Single ReplacementAB + C  AC + B Double Replacement AB + CD  AD + CB

Question 5 List the types of reactions and write examples of each using the letters A, B, etc. SynthesisA + B  AB DecompositionAB  A + B Single ReplacementAB + C  AC + B Double Replacement AB + CD  AD + CB Combustion (Complete)

Question 5 List the types of reactions and write examples of each using the letters A, B, etc. SynthesisA + B  AB DecompositionAB  A + B Single ReplacementAB + C  AC + B Double Replacement AB + CD  AD + CB Combustion C x H y + O 2  CO 2 + H 2 O (Complete)

Question 5 List the types of reactions and write examples of each using the letters A, B, etc. SynthesisA + B  AB DecompositionAB  A + B Single ReplacementAB + C  AC + B Double Replacement AB + CD  AD + CB CombustionC x H y + O 2  CO 2 + H 2 O (Complete) Combustion (Incomplete)

Question 5 List the types of reactions and write examples of each using the letters A, B, etc. SynthesisA + B  AB DecompositionAB  A + B Single ReplacementAB + C  AC + B Double Replacement AB + CD  AD + CB CombustionC x H y + O 2  CO 2 + H 2 O (Complete) CombustionC x H y + O 2  CO + H 2 O (Incomplete)

Question 6 Copper metal reacts with silver nitrate solution What type of reaction that took place between the copper & silver nitrate?

Question 6 Copper metal reacts with silver nitrate solution What type of reaction that took place between the copper & silver nitrate? Single Replacement

Question 7 Copper metal reacts with silver nitrate solution What is the skeletal chemical reaction equation?

Question 7 Copper metal reacts with silver nitrate solution What is the skeletal chemical reaction equation? Cu + Ag(NO 3 )  Cu(NO 3 ) 2 + Ag or Cu + Ag(NO 3 )  Cu(NO 3 ) + Ag

Question 8 Copper metal reacts with silver nitrate solution This reaction shows which metal is more reactive?

Question 8 Copper metal reacts with silver nitrate solution This reaction shows which metal is more reactive? Copper

Question 9 Sulfur dioxide is produced from the burning of sulfur. What type of reaction that took place between the sulfur & oxygen gas?

Question 9 Sulfur dioxide is produced from the burning of sulfur. What type of reaction that took place between the sulfur & oxygen gas? Synthesis

Question 10 Sulfur dioxide is produced from the burning of sulfur. What is the skeletal chemical reaction equation?

Question 10 Sulfur dioxide is produced from the burning of sulfur. What is the skeletal chemical reaction equation? S + O 2  SO 2

Question 11 Sulfur dioxide is produced from the burning of sulfur. What is the balanced equation for the reaction?

Question 11 Sulfur dioxide is produced from the burning of sulfur. What is the balanced equation for the reaction? S + O 2  SO 2

Question 12 In a chemical reaction, what is the relationship between the total mass of the reactants and the total mass of the products?

Question 12 In a chemical reaction, what is the relationship between the total mass of the reactants and the total mass of the products? They are the SAME (Law of Conservation of Mass)

Question 13 Which substances are the reactants and which are the products?

Question 13 Which substances are the reactants and which are the products? Reactants: H 2 & O 2 ; products: H 2 O

Question 14 What is the skeletal chemical reaction equation?

Question 14 What is the skeletal chemical reaction equation? H 2 + O 2  H 2 O

Question 15 What is the balanced equation for the reaction?

Question 15 What is the balanced equation for the reaction? 2H 2 + O 2  2H 2 O

Question 16 What type of reaction took place?

Question 16 What type of reaction took place? Decomposition

Question 17 What is the word equation that describes this reaction?

Question 17 What is the word equation that describes this reaction? Hydrogen bromide breaks down into hydrogen gas and bromine gas

Question 18 What are the reactant(s) and product(s)?

Question 18 What are the reactant(s) and product(s)? Reactants HBr; products: H 2 and Br 2

Question 19 What is the balanced equation for this reaction?

Question 19 What is the balanced equation for this reaction? 2HBr  H 2 + Br 2

Question 20 Copper metal is heated in an evaporating dish using a Bunsen burner. After 10 minutes it looses its ‘copper color’ and turns black, indicating it has reacted with the oxygen in the air to make copper oxide. The type of reaction that took place was?

Question 20 Copper metal is heated in an evaporating dish using a Bunsen burner. After 10 minutes it looses its ‘copper color’ and turns black, indicating it has reacted with the oxygen in the air to make copper oxide. The type of reaction that took place was? Synthesis (Cu + O 2  CuO)

Question 21 What are the reactants and products of this reaction?

Question 21 What are the reactants and products of this reaction? Reactants: HCl and NaOH; products: NaCl and H 2 O

Question 22 The type of reaction that took place would BEST be classified as:

Question 22 The type of reaction that took place would BEST be classified as: Double replacement

Question 23 What is the balanced equation for this reaction?

Question 23 What is the balanced equation for this reaction? HCl + NaOH  NaCl + H 2 O (skeletal and balanced are same)

Question 24 Clear lead nitrate solution is added to a test tube containing potassium chloride solution and a white solid immediately begins to form in the bottom of the test tube. The products of this reaction are most likely?

Question 24 Clear lead nitrate solution is added to a test tube containing potassium chloride solution and a white solid immediately begins to form in the bottom of the test tube. The products of this reaction are most likely? Lead chloride and potassium nitrate

Question 25 Clear lead nitrate solution is added to a test tube containing potassium chloride solution and a white solid immediately begins to form in the bottom of the test tube. The type of reaction that took place would BEST be classified as?

Question 25 Clear lead nitrate solution is added to a test tube containing potassium chloride solution and a white solid immediately begins to form in the bottom of the test tube. The type of reaction that took place would BEST be classified as? Double replacement

Question 26 If the reaction rate was increased for a reaction, without changing the products, what can you assume was added to the reaction?

Question 26 If the reaction rate was increased for a reaction, without changing the products, what can you assume was added to the reaction? Catalyst

Question 27 In an equation, the number of molecules of a given substance is indicated by what?

Question 27 In an equation, the number of molecules of a given substance is indicated by what? Coefficient

Question 28 A piece of Calcium metal is placed in a test tube containing hydrochloric acid (HCl) and immediately begins to fizz and ‘disappear’. After a few minutes, the test tube begins to get hot to the touch; when the flaming splint test is preformed a loud popping noise is heard. This reaction can be classified as what?

Question 28 A piece of Calcium metal is placed in a test tube containing hydrochloric acid (HCl) and immediately begins to fizz and ‘disappear’. After a few minutes, the test tube begins to get hot to the touch; when the flaming splint test is preformed a loud popping noise is heard. This reaction can be classified as what? Single replacement

Question 29 A piece of Calcium metal is placed in a test tube containing hydrochloric acid (HCl) and immediately begins to fizz and ‘disappear’. After a few minutes, the test tube begins to get hot to the touch; when the flaming splint test is preformed a loud popping noise is heard. From the flaming splint you can conclude that one of the products is?

Question 29 A piece of Calcium metal is placed in a test tube containing hydrochloric acid (HCl) and immediately begins to fizz and ‘disappear’. After a few minutes, the test tube begins to get hot to the touch; when the flaming splint test is preformed a loud popping noise is heard. From the flaming splint you can conclude that one of the products is? Hydrogen gas [ H 2 (g) ]

Question 30 A piece of Calcium metal is placed in a test tube containing hydrochloric acid (HCl) and immediately begins to fizz and ‘disappear’. After a few minutes, the test tube begins to get hot to the touch; when the flaming splint test is preformed a loud popping noise is heard. Would this reaction be endothermic or exothermic? Explain your answer.

Question 30 A piece of Calcium metal is placed in a test tube containing hydrochloric acid (HCl) and immediately begins to fizz and ‘disappear’. After a few minutes, the test tube begins to get hot to the touch; when the flaming splint test is preformed a loud popping noise is heard. Would this reaction be endothermic or exothermic? Explain your answer. Exothermic; test tube gets “hot to the touch”

Question 31 A piece of Calcium metal is placed in a test tube containing hydrochloric acid (HCl) and immediately begins to fizz and ‘disappear’. After a few minutes, the test tube begins to get hot to the touch; when the flaming splint test is preformed a loud popping noise is heard. The other product is most likely what?

Question 31 A piece of Calcium metal is placed in a test tube containing hydrochloric acid (HCl) and immediately begins to fizz and ‘disappear’. After a few minutes, the test tube begins to get hot to the touch; when the flaming splint test is preformed a loud popping noise is heard. The other product is most likely what? Calcium chloride (CaCl 2 )

Question 32 Methane gas (CH 4 ) is burned and reacts with oxygen from the air… The type of reaction that took place was?

Question 32 Methane gas (CH 4 ) is burned and reacts with oxygen from the air… The type of reaction that took place was? Combustion

Question 33 Methane gas (CH 4 ) is burned and reacts with oxygen from the air… What is the balanced equation for the above reaction?

Question 33 Methane gas (CH 4 ) is burned and reacts with oxygen from the air… What is the balanced equation for the above reaction? CH 4 + 2O 2  CO 2 + 2H 2 O

Question 34 A substance that enters into a chemical reaction is called what?

Question 34 A substance that enters into a chemical reaction is called what? Reactant

Question 35 A substance that is formed by a chemical reaction is called what?

Question 35 A substance that is formed by a chemical reaction is called what? Product

Question 36 In a true chemical reaction a new substance must form. True or False?

Question 36 In a true chemical reaction a new substance must form. True or False? True (forming a new substance is the definition of a chemical reaction)

Question 37 What does the  stand for?

Question 37 What does the  stand for? Yields or Reacts or Forms or Produces

Question 38 What is the chemical equation for “magnesium reacts with chlorine to produce magnesium chloride”?

Question 38 What is the chemical equation for “magnesium reacts with chlorine to produce magnesium chloride”? Mg + Cl 2  MgCl 2

Question 39 The total number of atoms of each element remains the same in a balanced equation. True of False?

Question 39 The total number of atoms of each element remains the same in a balanced equation. True of False? True

Question 40 The activity series of metals ranks elements in order of what?

Question 40 The activity series of metals ranks elements in order of what? Reactivity (Decreasing)

Question 41 CuCl 2 + Mg  Cu + MgCl 2 Which is the more active metal?

Question 41 CuCl 2 + Mg  Cu + MgCl 2 Which is the more active metal? Magnesium (it’s able to displace the copper)

Question 42 What is a catalyst? Name two ways that catalysts can change the nature of a chemical reaction.

Question 42 What is a catalyst? Name two ways that catalysts can change the nature of a chemical reaction. Catalyst is neither reactant nor product. Not used up in reaction. Speeds up reaction rate and/or lowers reaction temperature.

Question 43 How would you show that heat was used during a reaction?

Question 43 How would you show that heat was used during a reaction? Include the word “heat” as one of the reactants.

Question 44 How would you show that platinum was being used as a catalyst?

Question 44 How would you show that platinum was being used as a catalyst? Place the letters “Pt” over the top of the reaction arrow

Question 45 What is the symbol for equilibrium?

Question 46 Predict the products of the following reaction: Pb + Cu(SO 4 )  ______ + ______

Question 46 Predict the products of the following reaction: Pb + Cu(SO 4 )  ______ + ______ Pb + Cu(SO 4 ) ― > Pb(SO 4 ) + Cu

Question 47 N 2 + 3H 2  2NH 3 + Heat In the synthesis of ammonia (NH 3 ), which direction (forward or reverse) would be favored if: Temperature was raised – Hydrogen was decreased – Pressure was increased –

Question 47 N 2 + 3H 2  2NH 3 + Heat In the synthesis of ammonia (NH 3 ), which direction (forward or reverse) would be favored if: Temperature was raised – Reverse Hydrogen was decreased – Pressure was increased –

Question 47 N 2 + 3H 2  2NH 3 + Heat In the synthesis of ammonia (NH 3 ), which direction (forward or reverse) would be favored if: Temperature was raised – Reverse Hydrogen was decreased – Reverse Pressure was increased –

Question 47 N 2 + 3H 2  2NH 3 + Heat In the synthesis of ammonia (NH 3 ), which direction (forward or reverse) would be favored if: Temperature was raised – Reverse Hydrogen was decreased – Reverse Pressure was increased – Forward

Question 48 Draw energy diagrams illustrating endothermic and exothermic reactions, and one showing the impact of adding a catalyst.

Question 48 Endothermic Reactions

Question 48 Exothermic Reactions

Question 48 Impact of adding a Catalyst

Unit 7 Reactions Exam Review. Question 1 Potassium Calcium Sodium Magnesium Aluminum Lead Copper Mercury Silver Which metals would be replaced in a solution.

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Unit 7 Reactions Exam Review. Question 1 Potassium Calcium Sodium Magnesium Aluminum Lead Copper Mercury Silver Which metals would be replaced in a solution.

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