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ACP Chemistry Semester 1 Final Exam
Name: ______________________ Period: ____ Date: ___________________
This exam is worth 100 points. Only those exams completed in black ink
will be graded. Good luck!
1) Dalton's Atomic Theory states
A) that all elements have several isotopes.
B) that matter is composed of small indestructible particles.
C) that the properties of matter are determined by the properties of atoms.
D) that energy is neither created nor destroyed during a chemical reaction.
E) that an atom is predominantly empty space.
2) Define thermal energy.
A) energy associated with the temperature of an object
B) energy associated with the motion of an object
C) energy associated with the force of an object
D) energy associated with the gravity of an object
E) All the above are true for thermal energy
3) Which of the following are examples of extensive properties?
A) mass
B) color
C) density
D) temperature
E) taste
4) Which of the following is an example of the law of multiple proportions?
A) A sample of chlorine is found to contain three times as much Cl-35 as Cl-37.
B) Two different compounds formed from carbon and oxygen have the following mass
ratios:
1.33 g O: 1 g C and 2.66 g O: 1 g C.
C) Two different samples of table salt are found to have the same ratio of sodium to
chlorine.
D) The atomic mass of bromine is found to be 79.90 amu.
E) Nitrogen dioxide always has a mass ratio of 2.28 g O: 1 g N.
5) How many neutrons are in arsenic?
A) 33
B) 41
C) 42
D) 41.9
E) 75
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6) An ionic bond is best described as
A) the sharing of electrons.
B) the transfer of electrons from one atom to another.
C) the attraction that holds the atoms together in a polyatomic ion.
D) the attraction between 2 nonmetal atoms.
E) the attraction between 2 metal atoms.
7) Determine the name for aqueous HBr.
A) bromic acid
B) bromous acid
C) hydrobromous acid
D) hydrogen bromate
E) hydrobromic acid
8) Give the name for PBr3.
A) phosphorus tribromide
B) potassium tribromide
C) phosphorus (III) bromide
D) phosphorus (II) bromide
E) phosphorus bromide
9) Determine the theoretical yield of HCl if 60.0 g of BCl3 and 37.5 g of H2O are reacted
according to the following balanced reaction. A possibly useful molar mass is BCl3 =
117.16 g/mol.
BCl3(g) + 3 H2O(l) → H3BO3(s) + 3 HCl(g)
A) 75.9 g HCl
B) 132 g HCl
C) 187 g HCl
D) 56.0 g HCl
E) 25.3 g HCl
10) What mass (in g) of AgCl is formed from the reaction of 75.0 mL of a 0.078 M
AgC2H3O2 solution with 55.0 mL of 0.109 M MgCl2 solution?
2 AgC2H3O2(aq) + MgCl2(aq) → 2 AgCl(s) + Mg(C2H3O2)2(aq)
A) 0.838 g
B) 1.72 g
C) 0.859 g
D) 2.56 g
E) 1.70 g
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11) Which of the following pairs of aqueous solutions will form a precipitate when
mixed?
A) NH4NO3 + Li2CO3
B) Hg2(NO3)2 + LiI
C) NaCl + Li3PO4
D) AgC2H3O2 + Cu(NO3)2
E) None of the above solution pairs will produce a precipitate.
12) Give the net ionic equation for the reaction (if any) that occurs when aqueous
solutions of Na2CO3 and HCl are mixed.
A) 2 H+(aq) + CO32-(aq) → H2CO3(s)
B) 2 Na+(aq) + CO32-(aq) + 2 H+(aq) + 2 Cl-(aq) → H2CO3(s) + 2 NaCl(aq)
C) 2 H+(aq) + CO32-(aq) → H2O(l) + CO2(g)
D) 2 Na+(aq) + CO32-(aq) + 2 H+(aq) + 2 Cl-(aq) → H2CO3(s) + 2 Na+(aq) + 2 Cl-(aq)
E) No reaction occurs.
13) The titration of 25.0 mL of an unknown concentration H2SO4 solution requires 83.6
mL of 0.12 M LiOH solution. What is the concentration of the H2SO4 solution (in M)?
A) 0.20 M
B) 0.40 M
C) 0.10 M
D) 0.36 M
E) 0.25 M
14) Determine the oxidizing agent in the following reaction.
Ni(s) + 2 AgClO4(aq) → Ni(ClO4)2(aq) + 2 Ag(s)
A) Ag
B) Ni
C) Cl
D) O
E) This is not an oxidation-reduction reaction.
15) The volume of a gas is proportional to the temperature of a gas is known as
A) Avogadro's Law
B) Ideal Gas Law
C) Charles's Law
D) Boyle's Law
E) Dalton's Law
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16) If a sample of 0.29 moles of Ar occupies 3.8 L under certain conditions, what volume
will 0.66 moles occupy under the same conditions?
A) 12 L
B) 8.6 L
C) 17 L
D) 5.0 L
E) 15 L
17) What is the volume of 9.783 x 1023 atoms of He at 9.25 atm and 512K?
A) 7.38 L
B) 3.69 L
C) 1.85 L
D) 15.4 L
E) 30.8 L
18) Which of the following gas samples would be most likely to behave ideally under the
stated conditions?
A) Ne at STP
B) CO at 200 atm and 25°C
C) SO2 at 2 atm and 0 K
D) N2 at 1 atm and -70°C
E) O2 at 400 atm and 25°C
19) Using the graph below, determine the gas that has the lowest density at STP.
A) A
B) B
C) C
D) D
E) All of the gases have the same density at STP.
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20) A mixture of 0.220 moles CO, 0.350 moles H2 and 0.640 moles He has a total
pressure of 2.95 atm. What is the pressure of CO?
A) 1.86 atm
B) 0.649 atm
C) 0.536 atm
D) 1.54 atm
E) 0.955 atm
21) Determine the volume of SO2 (at STP) formed from the reaction of 96.7 g of FeS2
and 55.0 L of O2 (at 398 K and 1.20 atm). The molar mass of FeS2 is 119.99 g/mol.
4 FeS2(s) + 11 O2(g) → 2 Fe2O3(s) + 8 SO2(g)
A) 36.1 L
B) 45.3 L
C) 18.1 L
D) 27.6 L
E) 32.9 L
22) Which of the following compounds will behave LEAST like an ideal gas at low
temperatures?
A) He
B) SO2
C) H2
D) N2
E) F2
23) Which of the following samples will have the greatest average speed at 355 K?
A) Ne
B) C2H4
C) Cl2
D) CH4
E) All of these samples will have the same average speed at the same temperature.
24) Which of the following is a Bronsted-Lowry base?
A) CH4
B) HCN
C) NH3
D) Cl2
E) None of the above are Bronsted-Lowry bases.
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25) The stronger the acid, then which of the following is TRUE?
A) The stronger the conjugate acid.
B) The stronger the conjugate base.
C) The weaker the conjugate base.
D) The weaker the conjugate acid.
E) None of the above.
26) What is the pH of pure water at 40.0°C if the Kw at this temperature is 2.92 × 10-14?
A) 6.767
B) 0.465
C) 7.000
D) 7.233
E) 2.067
27) Which of the following acids is the WEAKEST? The acid is followed by its Ka
value.
A) HC2H3O2, 1.8 × 10-5
B) HIO, 2.3 × 10-11
C) HBrO, 2.3 × 10-9
D) HClO, 2.9 × 10-8
E) C6H5CO2H, 6.3 × 10-5
28) Determine the pH of a 0.188 M NH3 solution at 25°C. The Kb of NH3 is 1.76 × 10-5.
A) 5.480
B) 2.740
C) 8.520
D) 11.260
E) 12.656
29) Which one of the following will form an acidic solution in water?
A) NH4Cl
B) NaF
C) LiI
D) KNO3
E) None of the above solutions will be acidic.
30) Identify the strongest acid.
A) H2O
B) H2S
C) H2Se
D) H2Te
E) not enough information is available
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31) Determine the pH of a 0.18 M H2CO3 solution. Carbonic acid is a diprotic acid
whose Ka1 = 4.3 × 10-7 and Ka2 = 5.6 × 10-11.
A) 11.00
B) 10.44
C) 5.50
D) 4.31
E) 3.56
32) Define specific heat capacity.
A) the quantity of heat required to raise the temperature of 1 mole of a substance by 1°C
B) the quantity of heat required to change a system's temperature by 1°C
C) the quantity of heat required to raise the temperature of 1 gram of a substance by 1°C
D) the quantity of heat required to raise the temperature of 1 gram of a substance by 1°F
E) the quantity of heat required to raise the temperature of 1 liter of a substance by 1°C
33) A 21.8 g sample of ethanol (C2H5OH) is burned in a bomb calorimeter, according to
the following reaction. If the temperature rises from 25.0 to 62.3°C, determine the heat
capacity of the calorimeter. The molar mass of ethanol is 46.07 g/mol.
C2H5OH(l) + 3 O2(g) → 2 CO2(g) + 3 H2O(g)
ΔH°rxn = -1235 kJ
A) 4.99 kJ/°C
B) 5.65 kJ/°C
C) 63.7 kJ/°C
D) 33.1 kJ/°C
E) 15.7 kJ/°C
34)According to the following reaction, how much energy is evolved during the reaction
of 32.5 g B2H6 and 72.5 g Cl2? The molar mass of B2H6 is 27.67 g/mol.
B2H6(g) + 6 Cl2(g) → 2 BCl3(g) + 6 HCl(g)
A) 1640 kJ
B) 238 kJ
C) 1430 kJ
D) 3070 kJ
E) 429 kJ
ΔH°rxn = -1396 kJ
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35)Use the standard reaction enthalpies given below to determine ΔH°rxn for the
following reaction:
P4(g) + 10 Cl2(g) → 4PCl5(s) ΔH°rxn = ?
Given:
PCl5(s) → PCl3(g) + Cl2(g)
ΔH°rxn= +157 kJ
P4(g) + 6 Cl2(g) → 4 PCl3(g)
ΔH°rxn
= -1207 kJ
A) -1835 kJ
B) -1364 kJ
C) -1050. kJ
D) -1786 kJ
E) -2100. kJ
36)Use the ΔH°f and ΔH°rxn information provided to calculate ΔH°f for IF:
ΔH°f (kJ/mol)
IF7(g)
-941
IF5(g)
-840
IF7(g) + I2(g) → IF5(g) + 2 IF(g) ΔH°rxn = -89 kJ
A) 101 kJ/mol
B) -146 kJ/mol
C) -190. kJ/mol
D) -95 kJ/mol
E) 24 kJ/mol
37) Which of the following processes have a ΔS > 0?
A) CH3OH(l) → CH3OH(s)
B) N2(g) + 3 H2(g) → 2 NH3(g)
C) CH4(g) + H2O (g) → CO(g) + 3 H2(g)
D) Na2CO3(s) + H2O(g) + CO2(g) → 2 NaHCO3(s)
E) All of the above processes have a ΔS > 0.
38) Consider a reaction that has a positive ΔH and a positive ΔS. Which of the following
statements is TRUE?
A) This reaction will be spontaneous only at high temperatures.
B) This reaction will be spontaneous at all temperatures.
C) This reaction will be nonspontaneous at all temperatures.
D) This reaction will be nonspontaneous only at high temperatures.
E) It is not possible to determine without more information.
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39) Consider a reaction that has a positive ΔH and a negative ΔS. Which of the following
statements is TRUE?
A) This reaction will be spontaneous only at high temperatures.
B) This reaction will be spontaneous at all temperatures.
C) This reaction will be nonspontaneous at all temperatures.
D) This reaction will be nonspontaneous only at high temperatures.
E) It is not possible to determine without more information.
40) Above what temperature does the following reaction become nonspontaneous?
FeO(s) + CO(g) → CO2(g) + Fe(s)
ΔH = -11.0 kJ; ΔS = -17.4 J/K
A) 632 K
B) 298 K
C) 191 K
D) This reaction is nonspontaneous at all temperatures.
E) This reaction is spontaneous at all temperatures.
41) Identify the statement that is FALSE.
A) The entropy of a gas is greater than the entropy of a liquid.
B) Entropy generally increases with increasing molecular complexity.
C) Free atoms have greater entropy than molecules.
D) Entropy increases with dissolution.
E) For noble gasses, entropy increases with size.
42) Calculate ΔS°rxn for the following reaction. The S° for each species is shown below
the reaction.
C2H2(g) + H2(g) → C2H4(g)
S°(J/mol∙K) 200.9
130.7
219.3
A) +112.3 J/K
B) +550.9 J/K
C) -112.3 J/K
D) +337.1 J/K
E) -550.9 J/K
43) Give the name of the reaction that achieves the theoretical limits with respect to free
energy in thermodynamics.
A) reversible reaction
B) forward reaction
C) reverse reaction
D) equilibrium reaction
E) irreversible reaction
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44) Given the following equation,
N2O(g) + NO2(g) → 3 NO(g) ΔG°rxn = -23.0 kJ
Calculate ΔG°rxn for the following reaction.
9 NO(g) → 3N2O(g) + 3NO2(g)
A) -23.0 kJ
B) 69.0 kJ
C) -69.0 kJ
D) -7.67 kJ
E) 23.0 kJ
45) Determine ΔG°rxn using the following information.
CaCO3(s) → CaO(s) + CO2(g)
ΔH°= +179.2 kJ; ΔS°= +160.2 J/K
A) -607.0 kJ
B) +112 .0 kJ
C) -89.3 kJ
D) +131.4 kJ
E) +228.1 kJ
46) Use Hess's law to calculate ΔG°rxn using the following information.
NO(g) + O(g) → NO2(g)
ΔG°rxn = ?
2 O3(g) → 3 O2(g)
O2(g) → 2 O(g)
NO(g) + O3(g) → NO2(g) + O2(g)
A) +753.5 kJ
B) +277.0 kJ
C) -676.0 kJ
D) -1152.5 kJ
E) -225.7 kJ
ΔG°rxn = +489.6 kJ
ΔG°rxn = +463.4 kJ
ΔG°rxn = - 199.5 kJ
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47) Calculate ΔGrxn at 298 K under the conditions shown below for the following
reaction.
2 Hg(g) + O2(g) → 2 HgO(s)
ΔG° = -180.8 kJ
P(Hg) = 0.025 atm, P(O2) = 0.037 atm
A) +207 kJ
B) -154.4 kJ
C) -26.5 kJ
D) -164 kJ
E) +60.7 kJ
48) Choose the statement below that is TRUE.
A) K > 1, ΔG°rxn is positive.
B) K < 1, ΔG°rxn is negative.
C) ΔG°rxn = 0 at equilibrium.
D) ΔGrxn = 0 at equilibrium.
E) None of the above statements are true.
49) Determine the equilibrium constant for the following reaction at 298 K.
Cl(g) + O3(g) → ClO(g) + O2(g)
ΔG° = - 34.5 kJ
A) 5.66 × 105
B) 0.986
C) 8.96 × 10-7
D) 4.98 × 10-4
E) 1.12 × 106
50) Isotopes differ in the number of what particle?
A) beta particles
B) protons
C) electrons
D) neutrons
E) gamma particles