Chapter 9 Test - Livingston Public Schools



Chapter 12 Test – VERSION A Name ___________________________

CP Chemistry Date _____________________________

Part I: Multiple Choice: Write the letter corresponding to the best choice in the space provided.

_____1. In balancing a chemical equation, which of the following are you allowed to do?

a. change subscripts

b. change superscripts

c. add coefficients

d. add new substances

_____2. What number should be written in front of Na to balance the equation:

Na + MgCl2 → NaCl + Mg

a. 1

b. 3

c. 2

d. 4

_____3. What is the standard form for a single-replacement reaction?

a. AX + BY → AY + BX

b. A + B → AB

c. AB → A + B

d. A +BX → AX + B

_____4. How many atoms of oxygen are represented in 2 Ca(NO3)2?

a. 4

b. 10

c. 6

d. 12

_____5. Given the reaction: Mg(s) + 2 HCl(aq) → MgCl2(aq) + H2(g), what state of matter is HCl?

a. solid

b. liquid

c. gas

d. dissolved in water (aqueous)

_____ 6. According to collision theory,

a. All collisions result in some sort of chemical reaction

b. Molecular orientation alone determines the effectiveness of a collision

c. The amount of energy of the particles determines whether a reaction occurs

d. Both molecular orientation and amount of energy must be right for a reaction to occur

_____ 7. What is the general relationship between temperature and reaction rate:

a. The higher the temperature, the higher the reaction rate

b. The higher the temperature, the lower the reaction rate

c. Temperature and rate vary inversely

d. There is no relationship between the two

_____ 8. What factor accounts for the fact that powdered sugar dissolves more quickly than granulated sugar under the same conditions?

a. Temperature

b. Concentration

c. Nature of reactants

d. Surface area

_____ 9. A substance that increases the rate of a reaction without itself being used up is called a(n)

a. Intermediate product

b. Catalyst

c. Inhibitor

d. Activated complex

_____ 10. In an exothermic reaction: (hint: draw the picture!)

a. the heat of the products is equal to the heat of the reactants

b. the heat of the products is greater than the heat of the reactants

c. the heat of the products is less than the heat of the reactants

d. it varies depending on the reaction

_____ 11. Which of the following statements about bonds and energy is correct?

a. Bond breaking and bond formation both require energy

b. Bond breaking and bond formation both release energy

c. Bond breaking requires energy and bond formation releases energy

d. Bond breaking releases energy and bond formation requires energy

_____ 12. Endothermic reactions are reactions that:

a. Absorb heat

b. Release heat

c. Do not involve heat

d. Take place instantaneously

Your answers must be written in the space provided for the following question.

[pic]

Reaction Progress

1. Given the above diagram, determine the: (include units)

a. Heat of the products: ______________

b. Heat of the reactants: ______________

c. Activation energy: ______________

d. ΔH: ______________

PART II: For each of the following reactions:

1. Label the type of reaction on the line to the left.

Reaction types include:

single displacement, double displacement, synthesis, decomposition, combustion of a hydrocarbon.

2. Balance the equation. (1 point – no partial credit)

___________________________1. ___ K + ___ FeCl3 → ___KCl + ___Fe

___________________________2. ___ HNO3 → ___H2O + ___N2O5

___________________________3. ___C3H8 + ___O2 → ___CO2 + ___H2O

___________________________4. ___H2SO4 + ___NaOH → ___H2O + ___Na2SO4

___________________________5. ___NaCl + ___O2 → ___NaClO3

PART III: WORD EQUATIONS – Write and balance the equation for each chemical reaction below:

1. chlorine + potassium bromide ( potassium chloride + bromine

2. hydrobromic acid + sodium hydroxide ( water + sodium bromide

3. aluminum carbonate ( aluminum oxide + carbon dioxide

4. strontium metal reacts with water to form strontium hydroxide and hydrogen gas.

Part IV: Predicting Products:

Reaction types include:

single displacement, double displacement, synthesis, decomposition, combustion of a hydrocarbon.

# 1 -3: Label the type of reaction, predict the products and balance the equation. (3 points for writing reaction, 1 point for balancing, 1 point for reaction type)

_______________________1. Ba + P →

_______________________2. Ca + Al(ClO3)3 →

_______________________3. C2H4 + O2 →

For #4-5: Label the type of reaction, predict the products and balance the equation.

_______________________4. potassium metal is placed in sulfuric acid (

_______________________5. lead (II) nitrate solution mixes with potassium iodide solution (

Chapter 12 Test – VERSION A Name ___________________________

CP Chemistry Date _____________________________

Part I: Multiple Choice: Write the letter corresponding to the best choice in the space provided.

__C___1. In balancing a chemical equation, which of the following are you allowed to do?

a. change subscripts

b. change superscripts

c. add coefficients

d. add new substances

__C___2. What number should be written in front of Na to balance the equation:

Na + MgCl2 → NaCl + Mg

a. 1

b. 3

c. 2

d. 4

__D___3. What is the standard form for a single-replacement reaction?

a. AX + BY → AY + BX

b. A + B → AB

c. AB → A + B

d. A +BX → AX + B

__D___4. How many atoms of oxygen are represented in 2 Ca(NO3)2?

a. 4

b. 10

c. 6

d. 12

__D___5. Given the reaction: Mg(s) + 2 HCl(aq) → MgCl2(aq) + H2(g), what state of matter is HCl?

a. solid

b. liquid

c. gas

d. dissolved in water (aqueous)

_H____ 6. According to collision theory,

e. All collisions result in some sort of chemical reaction

f. Molecular orientation alone determines the effectiveness of a collision

g. The amount of energy of the particles determines whether a reaction occurs

h. Both molecular orientation and amount of energy must be right for a reaction to occur

__E___ 7. What is the general relationship between temperature and reaction rate:

e. The higher the temperature, the higher the reaction rate

f. The higher the temperature, the lower the reaction rate

g. Temperature and rate vary inversely

h. There is no relationship between the two

__H___ 8. What factor accounts for the fact that powdered sugar dissolves more quickly than granulated sugar under the same conditions?

e. Temperature

f. Concentration

g. Nature of reactants

h. Surface area

___F__ 9. A substance that increases the rate of a reaction without itself being used up is called a(n)

e. Intermediate product

f. Catalyst

g. Inhibitor

h. Activated complex

__G___ 10. In an exothermic reaction: (hint: draw the picture!)

e. the heat of the products is equal to the heat of the reactants

f. the heat of the products is greater than the heat of the reactants

g. the heat of the products is less than the heat of the reactants

h. it varies depending on the reaction

__G___ 11. Which of the following statements about bonds and energy is correct?

e. Bond breaking and bond formation both require energy

f. Bond breaking and bond formation both release energy

g. Bond breaking requires energy and bond formation releases energy

h. Bond breaking releases energy and bond formation requires energy

__E___ 12. Endothermic reactions are reactions that:

e. Absorb heat

f. Release heat

g. Do not involve heat

h. Take place instantaneously

Your answers must be written in the space provided for the following question.

[pic]

Reaction Progress

1. Given the above diagram, determine the: (include units)

a. Heat of the products: ___40kJ_______

b. Heat of the reactants: ___10kJ_______

c. Activation energy: ___50kJ______

d. ΔH: _____30kj______

PART II: For each of the following reactions:

3. Label the type of reaction on the line to the left.

Reaction types include:

single displacement, double displacement, synthesis, decomposition, combustion of a hydrocarbon.

4. Balance the equation. (1 point – no partial credit)

____single displacement_______1. _3__ K + ___ FeCl3 → __3_KCl + ___Fe

_____decomposition ______2. _2_ HNO3 → ___H2O + ___N2O5

__combustion of a hydrocarbon_3. ___C3H8 + _5_O2 → _3__CO2 + __4_H2O

__double displacement________4. ___H2SO4 + _2__NaOH → __2_H2O + ___Na2SO4

____synthesis_______________5. _2__NaCl + __3_O2 → __2_NaClO3

PART III: WORD EQUATIONS – Write and balance the equation for each chemical reaction below:

5. chlorine + potassium bromide ( potassium chloride + bromine

Cl2 + 2KBr ( 2 KCl + Br2

6. hydrobromic acid + sodium hydroxide ( water + sodium bromide

HBr + NaOH ( H2O + NaBr

7. aluminum carbonate ( aluminum oxide + carbon dioxide

Al2(CO3)3 ( Al2O3 + 3 CO2

8. strontium metal reacts with water to form strontium hydroxide and hydrogen gas.

Sr + 2 H2O ( Sr(OH)2 + H2

Part IV: Predicting Products:

Reaction types include:

single displacement, double displacement, synthesis, decomposition, combustion of a hydrocarbon.

# 1 -3: Label the type of reaction, predict the products and balance the equation. (3 points for writing reaction, 1 point for balancing, 1 point for reaction type)

____synthesis___________ 1. 3 Ba + 2 P → Βa3P2

___single displacement_____2. 3 Ca + 2 Al(ClO3)3 → 3 Ca(ClO3)2 + 2 Al

Combustion of a hydrocarbon

_______________________3. C2H4 + 3 O2 → 2 CO2 + 2 H2O

For #4-5: Label the type of reaction, predict the products and balance the equation.

___single displacement____4. potassium metal is placed in sulfuric acid (

2 K + H2SO4 ( K2SO4 + H2

____double displacement__5. lead (II) nitrate solution mixes with potassium iodide solution (

Pb(NO3)2 + 2 KI ( PbI2 + 2 KNO3

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