Welcome to
Jeopardy
Unit 9 – Concepts of Acids & Bases
Unit 10 - Thermochemistry
Chemical
Reactions
Got it all
Acid
AND ?
Enthalpy
/Energy
EXO /
ENDO
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Which of the following chemical reactions
will produce a precipitate?
A. 3KBr + AlPO4 → K3PO4 + AlBr3
B. ZnCl2 + Mg2SO4 → ZnSO4 + MgCl2
C. Na2CO3 + CaCl2 → CaCO3 + 2NaCl
D. NH4OH + KCl → KOH + NH4Cl
c
Zn(s) + 2H+(aq) → Zn2+(aq) + H2(g)
Which of the following statements best explains why
the chemical reaction shown above is an oxidationreduction reaction?
F. Zn reacts under basic conditions.
G. Zn dissolves in an aqueous solution.
H. Zn and H+ undergo a change of state.
J. Zn loses electrons and H+ gains electrons.
j
The reaction below shows carbon monoxide
burning in oxygen.
2 CO + O2 → 2 CO2
What is the change in the oxidation number of
carbon for this reaction?
A. +2 to +1
B. +2 to +4
C. +4 to +1
D. +4 to +2
b
Copper (II) nitrate and sodium hydroxide solutions react in
a test tube as shown below.
Cu(NO3)2(aq) + 2NaOH(aq)→ Cu(OH)2(s) + 2NaNO3(aq)
If nitric acid is added to the test tube, the amount of solid
precipitate decreases. The best explanation for this is that
the acidF. Will dissolve most solids, including sodium nitrate.
G. Dilutes the solution making the precipitate dissolve.
H. Reacts with the copper (II) nitrate, pulling the
equilibrium to the left.
J. Will react with the copper (II) hydroxide to form water
and soluble copper(II) nitrate.
j
Consider this balanced chemical equation:
Zn (s) + 2 HCl (aq) → ZnCl2 (aq) + H2 (g)
Which is the oxidation half-reaction?
A. Zn → Zn2+ + 2eB. Zn + 2e- → Zn2+
C. 2H+ → H2 + 2eD. 2H+ + 2e- → H2
A
Which of the following reaction shows an acidbase reaction?
F. Na2CO3 + CaCl2 → CaCO3 + 2NaCl
G. HCl + NaOH → H2O +NaCl
H. CH4 + O2 → CO2 + H2O
J. Mg +HCl → MgCl2 + H2
g
What is the pH of a substance with
6.0 × 10–8 M [H3O+]?
F. 1.89
G. 2.63
H. 4.90
J. 7.22
j
Grapefruit juice has a pOH of approximately
11.0. What is the pH of grapefruit juice?
A. 3.0
B. 5.0
C. 9.0
D. 11.0
a
A solution of a metal hydroxide is prepared by
placing 1 mole of the compound in water and
stirring. Less than 1% of the solid dissolves.
Which of the following is the most likely value of
the pH of the solution?
A. 1
B. 6
C. 8
D. 14
c
10. Which energy conversion occurs during
the operation of an electrolytic cell?
A. Chemical energy to electrical energy
B. Electrical energy to chemical energy
C. Nuclear energy to electrical energy
D. Electrical energy to nuclear energy
b
An 18.0 g piece of an unidentified metal was
heated from 21.5°C to 89.0°C. If 292 J of heat
energy was absorbed by the metal in the
heating process, what was the identity of the
metal?
F. Calcium
G. Copper
H. Silver
J. Iron
h
Which energy conversion occurs during the
operation of an electrolytic cell?
A. Chemical energy to electrical energy
B. Electrical energy to chemical energy
C. Nuclear energy to electrical energy
D. Electrical energy to nuclear energy
b
Which of the following is one of the products of the
reaction between sulfuric acid and sodium
hydroxide?
F. Sodium hydride
H. Sulfur dioxide
G. Sodium sulfate
J. Hydrogen
g
The diagram below shows the structure of a common pain
reliever.
Which of the highlighted atoms or group of atoms
makes aspirin a Brønsted-Lowry acid?
F. 1
G. 2
H. 3
J. 4
g
In the reaction represented by this equation,
which substance(s) act as a Brønsted-Lowry
acid?
CH3COOH + H2O H3O+ + CH3COO
A.H2O only
B. CH3COOH only
C. CH3COOH and H3O+
D. H2O and CH3COOC
c
Hydrochloric acid is a strong acid.
How will it dissociate in water?
F. It will partially dissociate in water.
G. It will fully dissociate in water.
H. It will not dissociate in water.
J. It will not mix with water.
g
As a rock rolls down a hill, its potential energy is
converted into kinetic energy, sound energy, and even
thermal energy. What is true about the total energy of
this system?
A. Energy is lost as the rock moves down the hill.
B. Energy is gained as the rock moves down the hill.
C. The total energy remains the same as the rock
moves down the hill
D. The total energy is constantly changing as the
rock moves down the hill.
C
The temperature of a sample of water changes
from 10°C to 20°C when the sample absorbs
418 joules of heat. What is the mass of the
sample?
F. 100 g
G. 10 g
H. 1000 g
J. 1 g
g
Which enthalpy diagram shows that the reaction A2(g) +
X2(g) → 2AX(g) is an exothermic reaction that produces 550
kJ of heat?
A.
B.
C.
D.
A
For the reaction shown below, calculate the enthalpy of
reaction for decomposition of hydrogen peroxide into
oxygen and water and determine if the reaction is
exothermic or endothermic
.
2H2O2(l) → O2(g) + 2H2O(g)
ΔHf of reactants: ΔHf H2O2 (l) =-187.8 kJ/mol
ΔHf of products: ΔHf O2 (g) = 0.00 kJ/mol
ΔHf H2O(g) =-285.8 kJ/mol
F. 196 kJ/mol, endothermic
G. -196 kJ/mol, exothermic
H. 474 kJ/mol, exothermic
J. -474 kJ/mol, endothermic
g
In the figure of molecules shown below, what is
occurring?
A. Energy is removed from a solid to form a
liquid.
B. Energy is removed from a liquid to form a
solid.
C. Energy is added to a solid to form a liquid.
D. Energy is added to a liquid to form a solid.
c
How do you set up the enthalpy change for the reaction
shown below?
C2H4 (g) + 3O2 (g) → 2CO2 (g) + 2H2O (l)
Enthalpies: C2H4 (g) = 52.26 kJ/mol
O2 (g) = 0 kJ/mol
CO2 (g) = –393.5 kJ/mol
H2O (l) = –285.8 kJ/mol
F. [2(–393.5 kJ/mol) + 2(–285.8 kJ/mol)]– [(52.26 kJ/mol)
+ 3(0 kJ/mol)]
G. –[2(–393.5 kJ/mol) + 2(–285.8 kJ/mol)]– [(52.26
kJ/mol) + 3(0 kJ/mol)]
H. [(52.26 kJ/mol) + 3(0 kJ/mol)] +[2(–393.5 kJ/mol) +
2(–285.8 kJ/mol)]
J. [(52.26 kJ/mol) + 3(0 kJ/mol)] –[2(–393.5 kJ/mol) +
2(–285.8 kJ/mol)]
f
As heat is slowly added to a glass of ice water,
the temperature remains at 0°C. Which of the
following statements explains why the
temperature of the mixture of ice and water
remains constant as heat is added?
A. Heat is stored in the solid ice.
B. Heat is stored in the liquid water.
C. Heat is used to turn the solid ice into liquid
water.
D. Heat is absorbed equally by the solid ice and
the liquid water.
c
The diagram below shows a heating curve for a substance.
Between points X and Y, which of the following would be
observed?
A. Solid and liquid will be
present as the temperature
remains constant.
B. Liquid and vapor will be
present as the temperature
remains constant.
C. Only vapor will be present
as the temperature gradually increases.
D. Only liquid will be present as the temperature gradually
increases.
B
Which of the following statements describes all
exothermic reactions?
F. Exothermic reactions form gases.
G. Exothermic reactions require a catalyst.
H. The energy of the reactants is lower than the
energy of the products.
J. The energy of the reactants is higher than the
energy of the products.
j
Black powder has been used as a propellant for
fireworks for centuries. One of the components of
black powder is potassium nitrate (KNO3). A sample
of black powder containing 1 mol of KNO3 releases
289 kJ of heat during combustion. The molar mass
of KNO3 is 101 g/mol. How much heat is released if
a firework contains 250 g of KNO3?
A. 117 kJ
B. 715 kJ
C. 29,189 kJ
D. 72,250 kJ
b
A sample was burned in a calorimeter that has a
3000 mL water bath. The temperature of the water
rose from 22°C to 46°C. How much heat was
produced by the reaction? (Specific heat of water
is 4.184 J/g K)
A. 301 J
B. 12.5 kJ
C. 301 kJ
D. 577 kJ
c
Which equation represents an exothermic
reaction at 298 K?
A. N2(g) + O2(g) → 2NO(g)
B. C(s) + O2(g) → CO2(g)
C. KNO3(s) → K+(aq) + NO3-(aq)
D. NH4Cl(s) → NH4+(aq) + Cl-(aq)
b
Given the balanced equation representing a phase
change:
C6H4Cl2 (s) + energy → C6H4Cl2 (g)
Which statement describes this change?
F. It is endothermic, and entropy decreases.
G. It is endothermic, and entropy increases.
H. It is exothermic, and entropy decreases.
J. It is exothermic, and entropy increases.
.
g
Which is always true of an endothermic
reaction?
A. Chemical bonds are broken.
B. Energy is absorbed.
C. Energy is released.
D. Light is created.
B