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Physical Science - Unit 4 Extra Credit

Total questions: 65

Worksheet time: 5hrs 25mins

Name
Class
Date
1.

In the reaction between calcium metal and chlorine gas to produce calcium chloride. How would chlorine gas be represented?

a)

C

b)

Cl

c)

Cl₂

d)

C₂

2.

LT1 Lead Nitrate + Sodium Iodide ----> Sodium Nitrate + Lead Iodide What are the reactants in the above equation?

a)

lead nitrate, sodium iodide

b)

sodium nitrate, lead iodide

c)

sodium iodide, lead iodide

d)

lead nitrate, sodium nitrate

3.

Which statement about endothermic reactions is correct?

a)

Energy is always created in the form of heat.

b)

Energy is transferred from the surroundings to the reactants.

c)

Energy is used to force electrons to move to higher energy levels.

d)

Energy is transferred from the reactants to the surroundings.

4.

In an exothermic reaction

a)

the products have more energy than the reactants.

b)

the reactants have more energy than the products.

c)

the energy of the reactants and products is equal.

d)

the activation energy is greater than the energy of the products.

5.

According to the Law of Conservation of Mass, in a balanced chemical equation, the mass of the reactants is equal to the

a)

atoms in a molecule.

b)

volume of the reactants.

c)

atomic mass of the elements.

d)

mass of the products.

6.

LT2 The law of conservation of mass can be demonstrated by a chemical reaction. Which of the following models of a chemical reaction best represents the law of conservation of mass?

(a)  

7.

According to the law of conservation of mass, if two atoms of copper are used in the reactant, how many atoms of copper must be a part of the product?

a)

0

b)

1

c)

2

d)

4

8.

How many iodine atoms are in 4 CrI₃?

a)

3

b)

9

c)

12

d)

36

9.

How many Dinitrogen trioxide molecules are represented by “6 N₂O₃”?

a)

1

b)

2

c)

6

d)

12

10.

The following equations represent chemical reactions. Which equation shows that the total mass during a chemical reaction stays the same?

a)

Equation 1

b)

Equation 2

c)

Equation 3

d)

Equation 4

11.

In Antoine Lavoisier's classic experiment, mercuric (II) oxide is heated in a sealed container. The solid red powder is changed into silver liquid mercury and oxygen gas. If Lavoisier heated 50 grams of powdered mercuric oxide to produce 46.5 grams of liquid mercury, how much oxygen would be released?

a)

3.5 grams

b)

4 grams

c)

5 grams

d)

3 grams

12.

A physical science group wants to design a lab to compare the mass of reactants versus the mass of products for a chemical reaction between baking soda and vinegar. Which is the most appropriate procedure to gather relevant data?

a)

Measure 3.5 g of baking soda into a cup. Pour 2.5 g of vinegar into a bag. Pour the baking soda into the bag. Seal the bag closed. Measure the mass of the bag after the reaction is complete.

b)

Measure the masses of an empty bag and an empty cup. Measure 3.5 g of baking soda into a cup. Pour the baking soda into the bag. Seal the bag closed. Measure the mass of the bag after the reaction is complete.

c)

Measure 3.5 g of baking soda into a cup. Pour 2.5 g of vinegar into the same cup. Measure the mass of the cup after the reaction is complete.

d)

Measure the masses of an empty bag and an empty cup. Measure 3.5 g of baking soda into a cup. Place vinegar in bag. Place the cup inside the bag and seal the bag closed. Pour the baking soda onto the vinegar. Measure the mass of the bag after the reaction is complete.

13.

During science lab, Mr. Smith’s students tested the reactivity of aluminum in copper II chloride. When aluminum was added to a solution of copper II chloride, bubbles were produced. Based on the Law of Conservation of Matter, if 45 grams of aluminum are added to 45 grams of copper II chloride to produce 12 grams of copper, how much aluminum chloride would also be produced? The formula for the chemical reaction is as follows: Al + CuCl₂ → AlCl₃ + Cu

a)

102 grams

b)

57 grams

c)

78 grams

d)

90 grams

14.

A physical science group wants to analyze lab data to compare the mass of reactants versus the mass of products for a chemical reaction between baking soda and vinegar. Which is the most appropriate procedure to make meaningful conclusions? Measurements before the reaction: - Mass of empty bag: 8.85 g - Mass of empty cup: 2.20 g - Mass of cup with baking soda: 5.7 g - Mass of bag with vinegar: 11.35 g Measurements after the reaction: - Mass of bag with cup and products: 17.05 g

a)

Compare the total mass of reactants before the reaction to the total mass of products after the reaction.

b)

Measure the temperature change during the reaction.

c)

Analyze the color change of the reactants and products.

d)

Use a pH indicator to measure acidity before and after the reaction

15.

A synthesis reaction is a reaction between at least two different chemicals in which:

a)

one compound is decomposed by an electric current.

b)

one compound burns in the presence of oxygen.

c)

one compound breaks down into at least two new products.

d)

one new, more complex compound is formed.

16.

Classify the following reaction: Sulfur dioxide reacts with carbon to yield sulfur and carbon monoxide

a)

Single Replacement

b)

Double Replacement

c)

Synthesis

d)

Decomposition

17.

Which of the following equations is NOT balanced?

a)

KOH + HCl → KCl + H2O

b)

2Ca + O2 → 2CaO

c)

NaCl + H2SO4 → Na2SO4 + HCl

d)

Fe + S → FeS

18.

Which of the following correctly represents the word equation: Carbon and aluminum oxide react to form aluminum and carbon dioxide.

a)

C + Al2O3 --> Al + CO2

b)

C + AlO --> Al + CO2

c)

AlO3 --> Al + CO2

d)

C + Al2O3 --> Al + CO2

19.

LT5 Students were asked to balance the equation below. Evaluate their responses. Which statement is correct? Original Equation: Zn + HCl → ZnCl2 + H2 Student Answers: Student A: Zn + H2Cl2 → ZnCl2 + H2 Student B: Zn +2HCl → ZnCl2 + H2 Student C: Zn + HCl → ZnCl + H

a)

All of the students are correct because there are the same number of Zn, H, and Cl atoms on both sides of the equations.

b)

Student B is correct because he used the correct subscripts to have the same number of Zn, H, and Cl atoms on both sides of the equations.

c)

Student B is incorrect because he used a coefficient to have the same number of Zn, H, and Cl atoms on both sides of the equations.

d)

Student C is incorrect because he changed the subscripts to have the same number of Zn, H, and Cl atoms on both sides of the equations.

20.
_P4+_O2 →  _P2O3
a)
3 P4+1 O2 → 2 P2O3
b)
1 P4+1 O2 → 2 P2O3
c)
1 P4+ 3 O2 → 2 P2O3
d)
1 P4+ 2 O2 → 3 P2O3
21.
_AgNO3 + _Cu →_Cu(NO3)2 + _Ag
a)
2 AgNO3 + 2 Cu → 3 Cu(NO3)2 + 1 Ag
b)
2 AgNO3 + 1 Cu → 1 Cu(NO3)2 + 2 Ag
c)
1 AgNO3 + 2 Cu → 2 Cu(NO3)2 + 1 Ag
d)
3 AgNO3 + 2 Cu → 3 Cu(NO3)2 + 2 Ag
22.
_BaS + _PtF2 → _BaF2 + _PtS
a)
1 BaS + 1 PtF2 → 1 BaF2 + 1 PtS
b)
4 BaS + 2 PtF2 → 1 BaF2 +  1 PtS
c)
1 BaS + 2 PtF2→ 2 BaF2 +  2 PtS
d)
1 BaS + 3 PtF2 →1 BaF2 +  2 PtS
23.
_AlBr3 + _K2SO4 → _KBr + _Al2(SO4)3
a)
6 AlBr3 + 1 K2SO4 → 6 KBr + 1 Al2(SO4)3
b)
2 AlBr3 + 3 K2SO4 → 6 KBr + 1 Al2(SO4)3
c)
1 AlBr3 + 1 K2SO4 → 2 KBr + 3 Al2(SO4)3
d)
2 AlBr3 + 3 K2SO4 → 1 KBr + 2 Al2(SO4)3
24.
_SO2 + _Li2Se →_SSe2 + _Li2O
a)
1 SO2 + 2 Li2Se → 1 SSe2 + 2 Li2O
b)
1 SO2 + 1 Li2Se → 2 SSe2 + 2 Li2O
c)
2 SO2 + 2 Li2Se → 2 SSe2 +  2 Li2O
d)
2 SO2 + 2 Li2Se → 1 SSe2 + 1 Li2O
25.
_Al + _HCl →_H2 + _AlCl3
a)
2 Al + 2 HCl → 2 H2 + 6 AlCl3
b)
3 Al + 3 HCl → 6 H2 + 2 AlCl3
c)
1 Al + 1 HCl → 3 H2 + 1 AlCl3
d)
2 Al + 6 HCl → 3 H2 + 2 AlCl3
26.
_K + _Cl2 →_KCl
a)
2 K + 16 Cl2 → 8 KCl
b)
2 K + 1 Cl2 → 2 KCl
c)
3 K + 4 Cl2 → 3 KCl
d)
1 K + 1 Cl2 →1 KCl
27.
_NaF + _Br2 →_NaBr + _F2
a)
1NaF + 2 Br2 →1 NaBr + 2 F2
b)
2NaF + 2 Br2 → 2 NaBr + 2 F2
c)
2 NaF + 3 Br2 → 1 NaBr + 2 F2
d)
2 NaF + 1 Br2 → 2 NaBr + 1 F2
28.
Balance this equation,            Al2O3 ---> Al + O2 
a)
Cannot be balanced
b)
2Al2O3 ---> 2Al + 3O2 
c)
2Al2O3 ---> 4Al + 3O2 
d)
3Al2O3 ---> 2Al + O2 
29.
Balance this equation:  H2 + N2 → NH3
a)
 H2 + 4N2 → NH3
b)
 H2 + 3N2 → 2NH3
c)
 3H2 + N2 → 2NH3
d)
 2H2 + 2N2 → 2NH3
30.
How many total atoms are represented?         4Al2O3
a)
2
b)
8
c)
5
d)
20
31.
Substances that enter into a chemical reaction (found to the left side of the arrow) 
a)
product
b)
reactant
c)
chemical
d)
balanced equation
32.
The large number in front of a chemical formula or compound is the ___________. 
a)
coefficient
b)
product
c)
physical
d)
chemical
33.
In every balanced chemical equation, each side of the equation has the same number of ____.  
a)
coefficients
b)
moles
c)
molecules
d)
atoms of each element
34.
Is the following equation balanced or unbalanced?
Fe + S --> FeS
a)
balanced
b)
unbalanced
35.
When balancing equations what does
 -->
mean?
a)
subscript
b)
equals
c)
it is just an arrow
d)
yield
36.
What is the part of the chemical equation in green called? 
Fe + S --> FeS
a)
products
b)
reactants
c)
yield
d)
chemical formula
37.
How many atoms of aluminum are on each side of the following equation: 4Al + 3O2 --> 2Al2 O3
a)
2
b)
6
c)
1
d)
4
38.
How many atoms are there TOTAL in:
H2SO4
a)
6
b)
5
c)
7
d)
3
39.
___________________ are the elements or compounds that are formed in a chemical
reaction.
a)
Polymers
b)
Bonds
c)
Reactants
d)
Products
40.
Matter can not be created nor destroyed: it can only be
a)
Destroyed a little bit
b)
Invisible
c)
Transformed, changed
d)
None of the above
41.
If reaction starts with 20g of reactants it should produce 
a)
a total of 40g of products
b)
a total of 10g of products
c)
a total of 80 g of products
d)
a total of 20g of products
42.

The Law of Conservation of Mass States

a)

Energy cannot be created nor destroyed, it can only change form.

b)

Mass cannot be created nor destroyed, it can only change form.

c)

Mass can be created or destroyed, it cannot change form.

43.

Which of the models of a chemical reaction best represents the Law of Conservation of Mass?

a)

A

b)

B

c)

C

d)

D

44.

Which of the models of a chemical reaction best represents the Law of Conservation of Mass?

a)

A

b)

B

c)

C

d)

D

45.

Which of the models of a chemical reaction best represents the Law of Conservation of Mass?

a)

A

b)

B

c)

C

d)

D

46.

A student pours hydrochloric acid (HCl) into an open beaker that contains a piece of magnesium (Mg). A chemical reaction occurs, and the data for the reaction is shown in the image. Was there a total mass increase or a total mass decrease for this experiment?

a)

There was a increase in mass.

b)

There was a decrease in mass.

c)

There was no change in mass.

47.

A student heated a 10 gram sample of a chemical in an open container. A chemical reaction occurred, and the mass of the sample was measured again. The mass of the sample was found to be less than before the reaction. Which of the following best explains the decrease in mass of the sample?

a)

The heat caused the chemical to become less dense.

b)

The reaction gave off more heat than was added.

c)

Some of the lighter particles were destroyed.

d)

Some of the particles escaped as a gas formed.

48.

A student dissolved 25 grams of salt into 1,000 grams of water. What should the mass of the saltwater mixture be?

a)

975 grams

b)

1,000 grams

c)

1,025 grams

d)

2,500 grams

49.

A student measures the mass of an iron nail to be 25 grams. The student heats the nail over a bunsen burner and measures the mass of the nail afterwards. The mass of the nail is found to be greater after burning. Which of the following best explains the increase in mass of the nail?

a)

The heat caused the compound to become more dense.

b)

The reaction gave off less heat than was added.

c)

Some of the heavier particles multiplied inside the nail.

d)

Extra particles from the air were added to the nail during burning.

50.

What type of reaction is Fe + Cl2 → FeCl3

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Combustion

e)

None of these

51.

What type of reaction is C2H2 + O2 → CO2 + H2O

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Combustion

e)

None of these

52.

What type of reaction is BF3 + Li2SO3 → B2(SO3)3 + LiF

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Combustion

e)

None of these

53.

What type of reaction is Ag2O → Ag + O2

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Combustion

e)

None of these

54.

What type of reaction is C5H10 + O2 → CO2 + H2O

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Combustion

e)

None of these

55.

What type of reaction is Zn + HCl → H2 + ZnCl2

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Combustion

e)

None of these

56.

What type of reaction is H2 + N2 → NH3

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Combustion

e)

None of these

57.

What type of reaction is (NH2)3PO4 + Pb(NO3)4 → NH4NO3 + Pb3(PO4)4

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Combustion

e)

None of these

58.

What type of reaction is FeBr3 + H2SO4 → HBr + Fe2(SO4)3

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Combustion

e)

None of these

59.

What type of reaction is Fe + H2SO4 → H2 + FeSO4

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Combustion

e)

None of these

60.

What type of reaction is Mg + Br2 → MgBr2

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Combustion

e)

None of these

61.

What type of reaction is KClO3 → KCl + O2

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Combustion

e)

None of these

62.

What type of reaction is K2CO3 → K2O + CO2

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Combustion

e)

None of these

63.

What type of reaction is CH4 + O2 → CO2 + H2O

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Combustion

e)

None of these

64.

What type of reaction is NaOH + HCl → H2O + NaCl

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Combustion

e)

None of these

65.

What type of reaction is SeCl6 + O2 → SeO2 + Cl2

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Combustion

e)

None of these

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