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NAME ______________________________
DATE _________
PERIOD _______
CHEMISTRY (Honors) – TEST
Chemical Reactions and Stoichiometry
Choose the best answer for the following statements:
1.
A chemical reaction is a process in which
a) reactants change into products.
b) substances with new chemical and physical properties are formed.
c) the law of conservation of mass applies.
d) all of the above.
2.
What happens to the bonds between atoms in a substance that undergoes a
chemical reaction?
a) All single covalent bonds become double covalent bonds.
b) Some existing bonds will weaken while others will strengthen.
c) existing bonds are broken, atoms are rearrange, and new bonds form.
d) Bonds between atoms are unaffected during a chemical reaction.
3.
The numbers chosen to balance a chemical equation are called
a) superscripts
b) subscripts
c) coefficients
d) formula units
4.
Which of the following types of reactions results in many reactants forming a single
product?
a) synthesis reaction
b) decomposition reaction
c) single-replacement reaction
d) double-replacement reaction
5.
A double-replacement reaction is likely to occur when
a) a metal, such as zinc, is placed in a concentrated acid.
b) a hydrocarbon is burned in the presence of oxygen.
c) two ionic compounds are dissolved in water.
d) a compound breaks down into its elemental components.
6.
A combustion reaction usually involves
a) the production of a radioactive solid.
b) something being burned.
c) the synthesis of a hydrocarbon.
d) the production of no new substances.
7.
The type and number of atoms found in a molecule is shown by the
a) molecular formula
b) empirical formula
c) chemical formula
d) structural formula
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NAME ______________________________
DATE _________
PERIOD _______
8.
Stoichiometry is the study of
a) the qualitative relationships that exist in chemical reactions.
b) the quantitative relationships that exist in chemical reactions.
c) energy changes in chemical reactions.
d) the balance of nature in chemistry.
9.
The number of moles of each reactant taking part in a chemical reaction is
indicated by
a) the molar mass of each substance.
b) the subscripts in the chemical formulas.
c) the type of reaction.
d) the coefficients in the balanced equation.
10.
In the balanced equation 2H2 + O2  2H2O,
a) 2 moles of hydrogen react with 1 mole of oxygen.
b) 4 moles of hydrogen react with 1 mole of oxygen.
c) 2 moles of hydrogen react with 2 moles of oxygen.
d) 4 moles of water are produced.
11.
How many moles of hydrogen react with 1 mole of nitrogen in the
following reaction: N2 + 3H2  2NH3?
a) 1
b) 2
c) 3
d) 6
12.
After translating the names of the reactants and products into chemical symbols,
what value should be checked for accuracy immediately before balancing the
equation?
a) coefficients
b) charges
c) subscripts
d) moles
13.
The limiting reactant in a chemical reaction
a) will have some amount unchanged, or leftover, after the reaction.
b) is completely used up in the reaction.
c) cannot be calculated without performing the reaction.
d) has no effect on the amount of product formed.
14.
The ratio of the actual amount of product to the theoretical amount of product in a
chemical reaction is called the
a) true yield
b) expected yield c) actual yield
d) percent yield
15.
The calculated amount of product that should be produced in a chemical reaction
is called the
a) true yield
b) theoretical yield c) actual yield
d) percent yield
16.
A particular reaction is expected to produce 2.6 L of oxygen gas. In reality, the
reaction only produces 2.4 L of oxygen gas. The percent yield of the reaction is
a) 42 %
b) 73 %
c) 92 %
d) 137 %
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NAME ______________________________
DATE _________
PERIOD _______
Solve the following problems. Show your calculations for credit.
17.
Translate and balance the following reaction.
When methane (CH4) reacts with oxygen, carbon dioxide and water are produced.
a) Calculate the theoretical yield when 54 g of methane reacts with excess oxygen.
How many grams of water are formed?
b) If 90 g of water are actually formed, calculate the percent yield of this reaction.
c) If 54 g of methane are reacted with 190 g of oxygen, which is the limiting reactant?
Justify through calculation. Lucky guesses won’t count.
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NAME ______________________________
CHEMISTRY (Honors) – Chemical Reactions
 Predict the product for each reaction.
 Balance the equation.
 Classify the type of reaction that occurred.
1.
Cu (NO3)2 
Ca +
a. Type of reaction: ____________________
2.
Na2SO4 
BaCl2 +
a. Type of reaction: ____________________
3.
C3H8
+
O2 
a. Type of reaction: ____________________
4.
Mg +
O2 
a. Type of reaction: ____________________
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DATE _________
PERIOD _______
NAME ______________________________
DATE _________
PERIOD _______
Reference the Reactivity Series to predict products. Balance the reaction if one
occurs. If no reaction occurs, record “No Reaction”.
Zn+2
+
AgNO3
 __________ + _____________
Zn+2
+
Pb(C2H3O2)2
 __________ + _____________
Zn+2
+
ZnSO4
 __________ + _____________
Zn+2
+
CuSO4
 __________ + _____________
Reference the equation below to answer the following prompts.
3 Ca3N2 (s) +
6 H2O (l) 
3 Ca(OH)2 (aq) + 2 NH3 (aq)
5. Put a star * over any coefficient on the reactant side.
6. Name the reactants (not the formulas!):
a. _____________________
b. _____________________
7. Circle any subscript on the product side.
8. Calculate the total atoms on the product side. ________________
9. Name the products (not the formulas!):
a. ____________________
b. _____________________
10. Calculate the molar mass of each product. Write your answer under each compound.
11. Calculate the total atoms on the product side. ________________
12. Does the equation support or break the Law of Conservation of Mass? Justify.
_______________________________________________________________________
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