Ch 11 final exam guide

Question 1

What does a chemical equation represent?

Answer 1

A chemical equation is the symbolic representation of a chemical reaction in the form of symbols and formulae,

Question 2

Where are the reactants located in a chemical equation?

Answer 2

Reactants are located on the left side of the arrow

Question 3

Where are the products located in a chemical equation?

Answer 3

Products are located on the right side of the arrow.

Question 4

Give 3 examles of symbols used in chemical equations, and what they mean.

Answer 4

+ used to separate one reactant or product from another
–> used to separate the reactants from the products - it is pronounced “yields” or “produces” when the equation is read
(two arrows overlapping) used when the reaction can proceed in both directions - this is called an equilibrium arrow and will be used later in the course
(g) indicates that the substance is in a gaseous state
(arrow up) an alternative way of representing a substance in a gaseous state
(s) indicates that the substance is in a solid state
(arrow down) an alternative way of representing a substance in a solid state
(aq) indicates that the substance is dissolved in water - the aq comes from aqueous
indicates that heat is applied to make the reaction proceed

Question 5

balance the following equation

NaClO3 = NaCl + O2

Answer 5

2 NaClO3 = 2 NaCl + 3 O2

Question 6

balance:

Mg + H3PO4 = Mg3 (PO4)2 + H2

Answer 6

3 Mg + 2 H3PO4 = Mg3(PO4)2 + 3 H2

Question 7

balance

(NH4)2CO3 + NaOH = Na2CO3 + NH3 + H2O

Answer 7

(NH4)2CO3 + 2 NaOH = Na2CO3 + 2 NH3 + 2 H2O

Question 8

balance

C3H6 + O2 = CO + H2O

Answer 8

C3H6 + 3 O2 = 3 CO + 3 H2O

Question 9

what is a Synthesis reaction?

Answer 9

Two or more reactants combine to make 1 new product.

Question 10

Classify these two reactions:
C(s) + O2(g) → CO2(g)
H2O(l) + SO3(g) → H2SO4(aq)

Answer 10

Synthesis reactions

Two or more reactants combine to make 1 new product.

Question 11

Classify the type of reaction in these two equations:

H2CO3(aq) → H2O(l) + CO2(g)
CaCO3(s) → CaO(s) + CO2(g)

Answer 11

decomposition reactions

because a single reactant breaks down to form 2 or more products.

Question 12

what is a decomposition reaction?

Answer 12

A single reactant breaks down to form 2 or more products.

Question 13

What is a single replacement reaction?

Answer 13

A single element replaces a similar element of an adjacent reactant compound.

Question 14

Classify this type of reaction:

Zn(s) + CuSO4(aq) → ZnSO4(aq) + Cu(s)

Answer 14

Single Replacement Reaction because a single element replaced a similar element of an adjacent reactant compound

Question 15

What is a Double-replacement reaction?

Answer 15

Two ionic compounds exchange ions, producing 2 new ionic compounds.

Question 16

Classify this type of reaction in these two examples:
NaCl(aq) AgNO3(aq) → NaNO3(aq) + AgCl(s)
HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l)

Answer 16

Double-replacement reactions because two ionic compounds exchange ions, producing 2 new ionic compounds

Question 17

what are the 5 types to classify chemical reactions?

Answer 17

(SDSDC to remember)

synthesis, decomposition, single replacement, double replacement, or a combustion reaction

Question 18

what is a combustion reaction?

Answer 18

A single element or compound combines with oxygen gas releasing energy. This rapid oxidation is called burning.

Question 19

classify these two reactions:
Examples:
C(s) + O2(g) → CO2(g) + energy
2Mg(s) + O2(g) → 2MgO(s) + energy

Answer 19

Combustion reactions

A single element or compound combines with oxygen gas releasing energy. This rapid oxidation is called burning.