AP CHEMISTRY Scoring Guide
Unit 4 MCQ
1. 10 HI + 2 KMnO4 + 3 H2SO4 → 5 I2 + 2 MnSO4 + K2SO4 + 8 H2O
According to the balanced equation above, how many moles of HI would be necessary to produce 2.5 mol of I2,
starting with 4.0 mol of KMnO4 and 3.0 mol of H2SO4 ?
(A) 20.
(B) 10.
(C) 8.0
(D) 5.0
(E) 2.5
2. 2 Al(s) + 6 HCl(aq) → 2 AlCl3(aq) + 3 H2(g)
According to the reaction represented above, about how many grams of aluminum (atomic mass 27 g) are necessary
to produce 0.50 mol of hydrogen gas at 25ºC and 1.00 atm?
(A) 1.0 g
(B) 9.0 g
(C) 14 g
(D) 27 g
(E) 56 g
3.
2 H2O(l) + 4 MnO4-(aq) + 3 ClO2-(aq) → 4 MnO2(s) + 3 ClO4-(aq) + 4 OH-(aq)
According to the balanced equation above, how many moles of ClO2-(aq) are needed to react completely with 20.
mL of 0.20 M KMnO4 solution?
(A) 0.0030 mol
(B) 0.0053 mol
(C) 0.0075 mol
(D) 0.013 mol
(E) 0.030 mol
4.
2 KClO3(s) → 2 KCl(s) + 3 O2(g)
What is the percentage yield of O2 if 12.3 g of KClO3 (molar mass 123 g) is decomposed to produce 3.2 g of O2
(molar mass 32 g) according to the equation above?
AP Chemistry Page 1 of 42
Scoring Guide
Unit 4 MCQ
(A) 100%
(B) 67%
(C) 50%
(D) 33%
(E) 10%
5.
According to the equation above, how many moles of potassium chlorate, KClO3 , must be decomposed to generate
1.0 L of O2 gas at standard temperature and pressure?
(A) mol
(B) mol
(C) mol
(D) mol
(E) mol
6.
2 MnO4-(aq) + 5 C2O42-(aq) + 16 H+(aq) → 2 Mn2+(aq) + 10 CO2(g) + 8 H2O(l)
Permanganate and oxalate ions react in an acidified solution according to the balanced equation above. How many
moles of CO2(g) are produced when 20. mL of acidified 0.20 M KMnO4 solution is added to 50. mL of 0.10 M
Na2C2O4 solution?
(A) 0.0040 mol
(B) 0.0050 mol
(C) 0.0090 mol
(D) 0.010 mol
(E) 0.020 mol
7.
2 N2H4(g) + N2O4(g) → 3 N2(g) + 4 H2O(g)
When 8.0 g of N2H4 (32 g mol-1) and 92 g of N2O4 (92 g mol-1) are mixed together and react according to the
equation above, what is the maximum mass of H2O that can be produced?
Page 2 of 42 AP Chemistry
Scoring Guide
Unit 4 MCQ
(A) 9.0 g
(B) 18 g
(C) 36 g
(D) 72 g
(E) 144 g
8. 2 SO2(g) + O2(g) → 2 SO3(g)
A mixture of gases containing 0.20 mol of SO2 and 0.20 mol of O2 in a 4.0 L flask reacts to form SO3. If the
temperature is 25ºC, what is the pressure in the flask after reaction is complete?
(A)
(B)
(C)
(D)
(E)
9. 3 Ag(s) + 4 HNO3 → 3 AgNO3 + NO(g) + 2 H2O
The reaction of silver metal and dilute nitric acid proceeds according to the equation above. If 0.10 mole of
powdered silver is added to 10. milliliters of 6.0–molar nitric acid, the number of moles of NO gas that can be
formed is
(A) 0.015 mole
(B) 0.020 mole
(C) 0.030 mole
(D) 0.045
(E) 0.090
10. 5 Fe2+ + MnO4– + 8 H+ ⇄ 5 Fe3+ + Mn2+ + 4 H2O
In a titration experiment based on the equation above, 25.0 milliliters of an acidified Fe2+ solution requires 14.0
milliliters of standard 0.050–molar MnO4– solution to reach the equivalence point. The concentration of Fe2+ in the
original solution is
(A) 0.0010 M
(B) 0.0056 M
(C) 0.0028 M
(D) 0.0090 M
(E) 0.14 M
AP Chemistry Page 3 of 42
Scoring Guide
Unit 4 MCQ
At 27°C, five identical rigid 2.0 L vessels are filled with N2(g) and sealed. Four of the five vessels also contain a 0.050
mol sample of NaHCO3(s), NaBr(s), Cu(s), or I2(s), as shown in the diagram above. The volume taken up by the solids is
negligible, and the initial pressure of N2(g) in each vessel is 720 mm Hg. All four vessels are heated to 127°C and allowed
to reach a constant pressure.
11. At 127°C, the entire sample of I2 is observed to have vaporized. How does the mass of vessel 5 at 127°C compare to
its mass at 27°C?
(A) The mass is less, since the I2 is in the vapor phase.
(B) The mass is the same, since the number of each type of atom in the vessel is constant.
(C) The mass is greater, since the I2 will react with N2 to form NI3 , which has a greater molar mass.
(D) The mass is greater, since the pressure is greater and the particles have a higher average kinetic energy.
12. At 127°C, the pressure in vessel 1 is found to be higher than that in vessel 2. Which of the following reactions best
accounts for the observation?
(A) NaHCO3(s) → Na(s) + HCO3(s)
(B) NaHCO3(s) → NaH(s) + CO3(s)
(C) 2 NaHCO3(s) → Na2CO3(s) + CO2(g) + H2O(g)
(D) 2 NaHCO3(s) + N2(g) → 2 NaNO3(s) + C2H2(g)
13. A 1.0 L sample of an aqueous solution contains 0.10 mol of NaCl and 0.10 mol of CaCl2. What is the minimum
number of moles of AgNO3 that must be added to the solution in order to precipitate all of the Cl- as AgCl(s) ?
(Assume that AgCl is insoluble.)
(A) 0.10 mol
(B) 0.20 mol
(C) 0.30 mol
(D) 0.40 mol
(E) 0.60 mol
Page 4 of 42 AP Chemistry
Scoring Guide
Unit 4 MCQ
14. A 20.0–milliliter sample of 0.200–molar K2CO3 solution is added to 30.0 milliliters of 0.400–molar Ba(NO3)2
solution. Barium carbonate precipitates. The concentration of barium ion, Ba2+, in solution after reaction is
(A) 0.150 M
(B) 0.160 M
(C) 0.200 M
(D) 0.240 M
(E) 0.267 M
15. Addition of sulfurous acid (a weak acid) to barium hydroxide (a strong base) results in the formation of a
precipitate. The net ionic equation for this reaction is
(A) 2 H+(aq) + 2 OH-(aq) ⇄ 2 H2O(l)
(B) H2SO3(aq) + Ba2+(aq) + 2 OH-(aq) ⇄ BaSO3(s) + 2 H2O(l)
(C) 2 H+(aq) + SO32-(aq) + Ba2+(aq) + 2 OH-(aq) ⇄ BaSO3(s) + 2 H2O(l)
(D) H2SO3(aq) + Ba2+(aq) + 2 OH-(aq) ⇄ Ba2+(aq) + SO32-(aq) + 2 H2O(l)
(E) H2SO3(aq) + Ba(OH)2(aq) ⇄ BaSO3(s) + 2 H2O(l)
16.
When a student adds 30.0 mL of 1.00 M HCl to 0.56 g of powdered Fe, a reaction occurs according to the equation
above. When the reaction is complete at 273 K and 1.0 atm, which of the following is true?
(A) HCl is in excess, and 0.100 mol of HCl remains unreacted.
(B) HCl is in excess, and 0.020 mol of HCl remains unreacted.
(C) 0.015 mol of FeCl2 has been produced.
(D) 0.22 L of H2 has been produced.
The reaction represented above goes essentially to completion. The reaction takes place in a rigid, insulated vessel that is
initially at 600 K
17. A sample of CH3OH(g) is placed in the previously evacuated vessel with a pressure of P1 at 600 K. What is the
final pressure in the vessel after the reaction is complete and the contents of the vessel are returned to 600 K?
AP Chemistry Page 5 of 42
Scoring Guide
Unit 4 MCQ
(A) P1 / 9
(B) P1 / 3
(C) P1
(D) 3P1
18. A student pipetted five 25.00–milliliter samples of hydrochloric acid and transferred each sample to an Erlenmeyer
flask, diluted it with distilled water, and added a few drops of phenolphthalein to each. Each sample was then
titrated with a sodium hydroxide solution to the appearance of the first permanent faint pink color. The following
results were obtained.
Volumes of NaOH Solution
First Sample.....35.22 mL
Second Sample.....36.14 mL
Third Sample.....36.13 mL
Fourth Sample .....36.15 mL
Fifth Sample.....36.12 mL
Which of the following is the most probable explanation for the variation in the student’s results?
(A) The burette was not rinsed with NaOH solution.
(B) The student misread a 5 for a 6 on the burette when the first sample was titrated.
(C) A different amount of water was added to the first sample.
(D) The pipette was not rinsed with the HCI solution.
(E) The student added too little indicator to the first sample.
A sample of was placed in a solution of , where it reacted completely.
19. In another experiment, a small piece of is weighed, then placed in a flask containing excess
. The student wants to determine number of moles of gas produced. Which of the following is the best way to
conduct the experiment for accurate data collection?
(A) Conducting the experiment at different temperatures to see which generates the most gas
Completing the entire reaction in a large Erlenmeyer flask of known volume to measure the volume of
(B)
the gas collected
(C) Collecting the gas in a eudiometer tube and measuring the volume of the gas collected
(D) Conducting the reaction in a graduated cylinder and measuring the volume of the gas collected
20. Which of the following equations best represents the reacting species in the reaction described above?
Page 6 of 42 AP Chemistry
Scoring Guide
Unit 4 MCQ
(A)
(B)
(C)
(D)
21. . . . C10H12O4S(s) + . . . O2(g) → . . . CO2(g) + . . . SO2(g) + . . . H2O(g)
When the equation above is balanced and all coefficients are reduced to their lowest whole-number terms, the
coefficient for O2(g) is
(A) 6
(B) 7
(C) 12
(D) 14
(E) 28
22.
C3H8(g) + 4 Cl2(g) → C3H4Cl4(g) + 4 HCl(g)
A 6.0 mol sample of C3H8(g) and a 20. mol sample of Cl2(g) are placed in a previously evacuated vessel, where
they react according to the equation above. After one of the reactants has been totally consumed, how many moles
of HCl(g) have been produced?
(A) 4.0 mol
(B) 8.0 mol
(C) 20. mol
(D) 24 mol
23. C3H8(g) + 5 O2(g) → 3 CO2(g) + 4 H2O(l)
In the reaction represented above, what is the total number of moles of reactants consumed when 1.00 mole of
CO2(g) is produced?
(A) 0.33 mol
(B) 1.33 mol
(C) 1.50 mol
(D) 2.00 mol
(E) 6.00 mol
AP Chemistry Page 7 of 42
Scoring Guide
Unit 4 MCQ
24. ...C3H8(g) + ...O2(g) → ...H2O(g) + ...CO2(g)
When the equation for the reaction represented above is balanced and all coefficients are reduced to the lowest
whole-number terms, the coefficient for O2(g) is
(A) 1
(B) 2
(C) 3
(D) 5
(E) 6
25. . . . Ca3(PO4)2(s) + . . . H3PO4(l) → . . . Ca(H2PO4)2(s)
When the equation above is balanced and all coefficients are reduced to lowest whole-number terms, what is the
coefficient for H3PO4(l) ?
(A) 1
(B) 2
(C) 3
(D) 4
(E) 5
Reaction 1: CaC2(s) + 2 H2O(l) → C2H2(g) + Ca(OH)2(s)
Reaction 2: NaOCl(aq) + 2 HCl(aq) → Cl2(g) + NaCl(aq) + H2O(l)
Reaction 3: C2H2(g) + Cl2(g) → C2H2Cl2(g)
26. Reaction 2 occurs when an excess of 6 M HCl(aq) solution is added to 100. mL of NaOCL(aq) of unknown
concentration. If the reaction goes to completion and 0.010 mol of Cl2(g) is produced, then what was the molarity of
the NaOCL(aq) solution?
(A) 0.0010 M
(B) 0.010 M
(C) 0.10 M
(D) 1.0 M
Page 8 of 42 AP Chemistry
Scoring Guide
Unit 4 MCQ
27.
A sample of reacts with excess according to the equation above. If the reaction is
repeated with excess but with of , which of the following is correct?
(A) The amount of produced is doubled.
(B) The amount of produced is halved.
(C) The amount of produced remains the same.
(D) The amount of produced is doubled.
28. Which of the following describes the changes in forces of attraction that occur as H2O changes phase from a liquid
to a vapor?
(A) H – O bonds break as H – H and O – O bonds form.
(B) Hydrogen bonds between H2O molecules are broken.
(C) Covalent bonds between H2O molecules are broken.
(D) Ionic bonds between H+ ions and OH- ions are broken.
(E) Covalent bonds between H+ ions and H2O molecules become more effective.
29.
Mass of empty crucible
Mass of crucible and sample before heating
Mass of crucible and sample after heating
A student places a sample of a pure metal in a crucible and heats it strongly in air. Data from the experiment are
given in the table above. The final mass was determined after the sample was cooled to room temperature. Which of
the following statements related to the experiment is correct?
The mass of the sample decreased, so physical changes occurred as the metal first melted and then
(A)
boiled out of the crucible.
The mass of the sample increased, so a chemical change occurred when bonds formed between the metal
(B)
and another substance.
(C) There was nothing for the metal to react with, so only a physical change could have occurred.
(D) The sample was only heated, so neither a physical nor a chemical change occurred.
30. If equal masses of the following compounds undergo complete combustion, which will yield the greatest mass of
CO2?
(A) Benzene, C6H6
(B) Cyclohexane, C6H12
(C) Glucose, C6H12O6
(D) Methane, CH4
AP Chemistry Page 9 of 42
Scoring Guide
Unit 4 MCQ
31.
CS2(l) + 3 O2(g) → CO2(g) + 2 SO2(g)
What volume of O2(g) is required to react with excess CS2(l) to produce 4.0 L of CO2(g)? (Assume all gases are
measured at 0°C and 1 atm.)
(A) 12 L
(B) 22.4 L
(C) L
(D) 2 22.4 L
(E) 3 22.4 L
Page 10 of 42 AP Chemistry
Scoring Guide
Unit 4 MCQ
32.
A group of students was asked to recover Cu(s) from a blue-green aqueous solution containing an unknown
concentration of Cu2+(aq) . The students took a 100.0 mL sample of the solution and added an excess of 1.0 M
Na3PO4(aq), causing the Cu2+(aq) to precipitate as Cu3(PO4)2(s), as shown in step 1 below.
Step 1
The Cu3(PO4)2(s) was filtered, dried, and weighed. Then the Cu3(PO4)2(s) was dissolved in a 3.0 M HCl(aq)
solution, as shown in step 2 below.
Step 2
The students added a strip of Zn(s) to the solution to recover the Cu(s), as shown in step 3 below.
Step 3
AP Chemistry Page 11 of 42
Scoring Guide
Unit 4 MCQ
Finally, the Cu(s) was filtered, dried, and weighed.
If 4.6 g of Cu3(PO4)2(s) was recovered from step 1, what was the approximate [Cu2+] in the original solution? (The
molar mass of Cu3(PO4)2 is 381 g/mol.)
(A) 0.040 M
(B) 0.12 M
(C) 0.36 M
(D) 1.5 M
33. A student mixes of white crystals with distilled water in a beaker. After the mixture was stirred, no
crystals are visible and the solution is clear. After several days, all of the water evaporates and white crystals are
found in the beaker. Which of following pieces of experimental evidence would best help the student to confirm that
a new compound had not been made and that only a physical change occurred?
(A) The solution does not change color after stirring.
(B) The crystals are no longer visible after mixing with water.
(C) There is a temperature change in the solution during the dissolving process.
(D) After the water has evaporated, the white crystals in the beaker have a mass of .
34.
A sample of and a sample of were combined, and
precipitated, as shown by the equation above. If the experiment is repeated using solutions of the
same molarity, which of the following changes in volume will double the amount of produced?
(A) Using the same volume of but twice the volume of
(B) Using twice the volume of but half the volume of
(C) Using twice the volume of but the same volume of
(D) Using twice the volume of and twice the volume of
Page 12 of 42 AP Chemistry
Scoring Guide
Unit 4 MCQ
35. Potassium hydrogen phthalate, KHP, is used as a primary standard for determining the concentration of a solution
of NaOH by titration. If the KHP has not been dried before weighing, the calculated molarity of
the NaOH would be
(A) higher than the actual value, since water is included in the apparent mass of KHP
(B) higher than the actual value, since the presence of water requires a larger volume of titrant
(C) lower than the actual value, since NaOH absorbs water
(D) unaffected, since KHP is a strong acid
(E) unaffected, since water is routinely added before the titration
An experiment was performed to investigate the reaction between metal and at different concentrations.
Because the ion is green, the extent of the reaction was determined using spectrophotometric analysis. Four
standard solutions of were prepared by dissolving (molar mass ) in
water. The absorbance of each solution was measured; the results are shown both in the table below and in the following
plot of the absorbance data.
Solution Absorbance
36. Which of the following equations best represents the reacting species in the reaction between metal and
?
AP Chemistry Page 13 of 42
Scoring Guide
Unit 4 MCQ
(A)
(B)
(C)
(D)
37. Which species is being oxidized in the reaction between metal and ?
(A)
(B)
(C)
(D)
38.
H2 + F2 → 2 HF
In the reaction represented above, what mass of HF is produced by the reaction of 3.0 x 1023 molecules of H2 with
excess F2 ? (Assume the reaction goes to completion.)
(A) 1.0 g
(B) 4.0 g
(C) 10. g
(D) 20. g
(E) 40. g
2 H2O2(aq) → 2 H2O(l) + O2(g) ΔH° = −196 kJ/molrxn
The decomposition of H2O2(aq) is represented by the equation above. A student monitored the decomposition of a 1.0 L
sample of H2O2(aq) at a constant temperature of 300. K and recorded the concentration of H2O2 as a function of time.
The results are given in the table below.
Page 14 of 42 AP Chemistry
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Unit 4 MCQ
39. The O2(g) produced from the decomposition of the 1.0 L sample of H2O2(aq) is collected in a previously evacuated
10.0 L flask at 300. K. What is the approximate pressure in the flask after 400. s? (For estimation purposes, assume
that 1.0 mole of gas in 1.0 L exerts a pressure of 24 atm at 300. K.)
(A) 1.2 atm
(B) 2.4 atm
(C) 12 atm
(D) 24 atm
40. Which of the following identifies the element(s) being oxidized and reduced in the reaction?
(A) Hydrogen is oxidized and oxygen is reduced.
(B) Oxygen is oxidized and hydrogen is reduced.
(C) Oxygen is both oxidized and reduced.
(D) No elements are oxidized or reduced; the reaction is not a redox reaction.
41.
. . . LiHCO3(aq) + . . . H2SO4(aq) → . . . Li2SO4(aq) + . . . H2O(l) + . . . CO2(g)
When the equation above is balanced and the coefficients are reduced to lowest whole-number terms, what is the
coefficient of H2O(l) ?
(A) 1
(B) 2
(C) 3
(D) 4
(E) 5
42. A student finds the mass of a pure sample of a metal chloride hydrate. The student heats the sample several times,
reaching a constant mass that contains mole of anhydrous metal chloride. Which of the following questions
about the hydrated metal chloride substance is most likely to be answered by the results of the experiment?
(A) How many moles of water are in one mole of the substance?
(B) How many moles of the metal cation are in one mole of the substance?
(C) What is the identity of the metal cation in the formula of the substance?
(D) What is the melting point of the substance?
AP Chemistry Page 15 of 42
Scoring Guide
Unit 4 MCQ
43.
A student had two dilute, colorless solutions, and , which were at the same temperature. The
student combined the solutions, and the reaction represented above occurred. Which of the following results would
be evidence that a chemical reaction took place?
(A) The resulting solution is colorless.
(B) The temperature of the reaction mixture increases.
(C) The total volume of the mixture is approximately equal to the sum of the initial volumes.
(D) The resulting solution conducts electricity.
44. If 0.40 mol of H2 and 0.15 mol of O2 were to react as completely as possible to produce H2O, what mass of reactant
would remain?
(A) 0.20 g of H2
(B) 0.40 g of H2
(C) 3.2 g of O2
(D) 4.0 g of O2
(E) 4.4 g of O2
Refer to the following.
PCl5(g) ⇄ PCl3(g) + Cl2(g)
PCl5(g) decomposes into PCl3(g) and Cl2(g) according to the equation above. A pure sample of PCl5(g) is placed in a
rigid, evacuated 1.00 L container. The initial pressure of the PCl5(g) is 1.00 atm. The temperature is held constant until
the PCl5(g) reaches equilibrium with its decomposition products. The figures below show the initial and equilibrium
conditions of the system.
45. If the decomposition reaction were to go to completion, the total pressure in the container would be
(A) 1.4 atm
(B) 2.0 atm
(C) 2.8 atm
(D) 3.0 atm
Page 16 of 42 AP Chemistry
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Unit 4 MCQ
K(s) + Cl2(g) → KCl(s) ΔH° = −437 kJ/molrxn
The elements K and Cl react directly to form the compound KCl according to the equation above. Refer to the information
above and the table below to answer the questions that follow.
46. What remains in the reaction vessel after equal masses of K(s) and Cl2(g) have reacted until either one or both of
the reactants have been completely consumed?
(A) KCl only
(B) KCl and K only
(C) KCl and Cl2 only
(D) KCl , K, and Cl2
AP Chemistry Page 17 of 42
Scoring Guide
Unit 4 MCQ
K(s)+ ½ Cl2(g) → KCl(s) ΔH° = -437kJ/molrxn
The elements K and Cl react directly to form the compound KCl according to the equation above. Refer to the information
above and the table below to answer the questions that follow.
47. What remains in the reaction vessel after equal masses of K(s) and Cl2(g) have reacted until either one or both of
the reactants have been completely consumed?
(A) KCl only
(B) KCl and K only
(C) KCl and Cl2 only
(D) KCl, K, and Cl2
48. When a buret is rinsed before a titration, which of the techniques below is the best procedure?
(A) Rinse the buret one time with some of the titrant solution.
(B) Rinse the buret one time with some of the titrant solution and then dry the buret in an oven.
(C) Rinse the buret two times: once with some of the titrant solution, then once with distilled water.
(D) Rinse the buret two times: each time with some of the titrant solution.
(E) Rinse the buret two times: each time with distilled water.
Page 18 of 42 AP Chemistry
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Unit 4 MCQ
A 0.35 g sample of Li(s) is placed in an Erlenmeyer flask containing 100 mL of water at 25°C. A balloon is placed over
the mouth of the flask to collect the hydrogen gas that is generated.
After all of the Li(s) has reacted with H2O(l), the solution in the flask is added to a clean, dry buret and used to titrate an
aqueous solution of a monoprotic acid. The pH curve for this titration is shown in the diagram below
49. Which of the following is the balanced net-ionic equation for the reaction between Li(s) and water?
(A) 2 Li(s) + 2 H+(aq) + 2 OH−(aq) → 2 Li+(aq) + 2 OH−(aq) + H2(g)
(B) 2 Li(s) + 2 H2O(l) → 2 Li+(aq) + 2 OH−(aq) + H2(g)
(C) 2 Li(s) + 2 H2O(l) → 2 LiOH(s) + H2(g)
(D) 2 Li(s) + 2 H2O(l) → 2 LiH(s) + H2(g)
Due to the presence of as an impurity, the combustion of some types of coal results in the formation of ,
as represented by the equation above. Also, can react with to form , as represented by the
equation below.
50. Which of the following statements is correct when of reacts with of ?
AP Chemistry Page 19 of 42
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Unit 4 MCQ
(A) is the limiting reactant and of is formed.
(B) is the limiting reactant and of is formed.
(C) is the limiting reactant and of is formed.
(D) is the limiting reactant and of remains unreacted.
51. What mass of Au is produced when 0.0500 mol of Au2S3 is reduced completely with excess H2?
(A) 9.85 g
(B) 19.7 g
(C) 24.5 g
(D) 39.4 g
(E) 48.9 g
52.
Extraction of from pyrite, , is a two-step process, as represented above. The maximum amount of
that could be extracted from of (molar mass ) is approximately
(A)
(B)
(C)
(D)
53.
In a one-person spacecraft, an astronaut exhales of (molar mass ) per day. To
prevent the buildup of in the spacecraft, a device containing is used to remove the ,
as represented by the equation above. What mass of (molar mass ) is needed to react with
all of the produced by an astronaut in one day
(A)
(B)
(C)
(D)
54. A student was asked to formulate a hypothesis about what would happen if of at
was combined with of at . Which of the following hypotheses indicates
that the student thought a chemical change would occur?
Page 20 of 42 AP Chemistry
