AP Chemistry Chapter 4
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. 1/3 ×22.4 D. 2 ×22.4 L E. 3 ×22.4 L
A. 12 L
The diagram above represents H2(g) and N2(g) in a closed container. Which of the following diagrams would represent the results if the reaction shown below were to proceed as far as possible? N2(g) + 3 H2(g) → 2 NH3(g)
D
The reaction between aqueous strontium chloride (SrCl2) and aqueous potassium sulfate (K2SO4) forms a precipitate of strontium sulfate (SrSO4). Which of the following represents the net ionic equation for the reaction? A Cl−(aq)+K+(aq)→KCl(aq)Cl−(aq)+K+(aq)→KCl(aq) B Sr2+(aq)+SO42−(aq)→SrSO4(s)Sr2+(aq)+SO42−(aq)→SrSO4(s) C Sr2+(aq)+2Cl−(aq)+SO42−(aq)+2K+(aq)→SrSO4(s)+2Cl−(aq)+2K+(aq)Sr2+(aq)+2Cl−(aq)+SO42−(aq)+2K+(aq)→SrSO4(s)+2Cl−(aq)+2K+(aq) D SrCl2(aq)+K2SO4(aq)→SrSO4(s)+2KCl(aq)
B Sr2+(aq)+SO42−(aq)→SrSO4(s)Sr2+(aq)+SO42−(aq)→SrSO4(s)
2F2(g)+2NaOH(aq)→OF2(g)+2NaF(aq)+H2O(l) A 2mol sample of F2(g) reacts with excess NaOH(aq) according to the equation above. If the reaction is repeated with excess NaOH(aq) but with 1 mol of F2(g), which of the following is correct? A The amount of OF2(g)OF2(g) produced is doubled. B The amount of OF2(g)OF2(g) produced is halved. C The amount of NaF(aq)NaF(aq) produced remains the same. D The amount of NaF(aq)NaF(aq) produced is doubled.
B The amount of OF2(g)OF2(g) produced is halved.
Ni(s)→Ni2+(aq)+2e− Ag+(aq)+e−→Ag(s) Which of the following is the balanced net ionic equation for an oxidation-reduction reaction between Ag+(aq) and Ni(s) based on the half-reactions represented above? A Ag+(aq)+Ni(s)→Ag(s)+Ni2+(aq)Ag+(aq)+Ni(s)→Ag(s)+Ni2+(aq) B 2Ag+(aq)+Ni(s)→Ag(s)+2Ni2+(aq)2Ag+(aq)+Ni(s)→Ag(s)+2Ni2+(aq) C Ag+(aq)+2Ni(s)→Ag(s)+2Ni2+(aq)Ag+(aq)+2Ni(s)→Ag(s)+2Ni2+(aq) D 2Ag+(aq)+Ni(s)→2Ag(s)+Ni2+(aq)
D 2Ag+(aq)+Ni(s)→2Ag(s)+Ni2+(aq)
A beaker was half filled with freshly distilled H2O and placed on a hot plate. As the temperature of the water reached 100°C, vigorous bubbling was observed in the beaker. The gaseous contents of the bubbles were analyzed. The presence of which of the following substances would support the claim that the observed phenomenon was a physical change? A H2(g)H2(g) B O2(g)O2(g) C CO2(g)CO2(g) D H2O(g)H2O(g)
D H2O(g)H2O(g)
HCl(aq)+H2O(l)→H3O+(aq)+Cl−(aq) For the dissolution of HCl in water represented above, which of the following pairs includes the Brønsted-Lowry bases? A HCl(aq)HCl(aq) and Cl−(aq)Cl−(aq) B HCl(aq)HCl(aq) and H3O+(aq)H3O+(aq) C H2O(l)H2O(l) and H3O+(aq)H3O+(aq) D H2O(l)H2O(l) and Cl−(aq)
D H2O(l)H2O(l) and Cl−(aq)
Which of the following is the correct net ionic equation of the neutralization reaction between hydrofluoric acid and sodium hydroxide in aqueous solution? A HF(aq)+NaOH(aq)→H2O(l)+NaF(aq)HF(aq)+NaOH(aq)→H2O(l)+NaF(aq) B HF(aq)+NaOH(aq)→NaH(aq)+FOH(aq)HF(aq)+NaOH(aq)→NaH(aq)+FOH(aq) C H+(aq)+OH−(aq)→H2O(l)H+(aq)+OH−(aq)→H2O(l) D HF(aq)+OH−(aq)→H2O(l)+F−(aq)
D HF(aq)+OH−(aq)→H2O(l)+F−(aq)
Zn(s)+2HCl(aq)→ZnCl2(aq)+H2(g) When the reaction represented above proceeds, heat is produced. Which of the following best describes the reaction? A It is a combustion reaction because heat is produced by the reaction. B It is a double replacement reaction because 2Cl2Cl atoms are added to ZnZn. C It is an acid-base reaction because HClHCl is an acid that is capable of exchanging H+H+. D It is an oxidation-reduction reaction because zinc is oxidized and hydrogen is reduced.
D It is an oxidation-reduction reaction because zinc is oxidized and hydrogen is reduced.
MgCl2(aq)+2NaOH(aq)→2NaCl(aq)+Mg(OH)2(s) A 100mL sample of 0.1MMgCl2(aq) and a 100mL sample of 0.2MNaOH(aq) were combined, and Mg(OH)2(s) 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 Mg(OH)2(s) produced? A Using the same volume of MgCl2(aq)MgCl2(aq) but twice the volume of NaOH(aq)NaOH(aq) B Using twice the volume of MgCl2(aq)MgCl2(aq) but half the volume of NaOH(aq)NaOH(aq) C Using twice the volume of MgCl2(aq)MgCl2(aq) but the same volume of NaOH(aq)NaOH(aq) D Using twice the volume of MgCl2(aq)MgCl2(aq) and twice the volume of NaOH(aq)
D Using twice the volume of MgCl2(aq)MgCl2(aq) and twice the volume of NaOH(aq)
Cu(s)+2AgNO3(aq)→Cu(NO3)2(aq)+2Ag(s) The reaction between solid copper and aqueous silver nitrate produces solid silver and a blue solution, as represented by the balanced equation shown above. Based on the balanced equation, which of the following identifies the oxidation and reduction half-reactions?
Oxidation Half-reaction Cu(s)→Cu2+(aq)+2e− Reduction Half-reaction Ag+(aq)+e−→Ag(s)
f 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
A 0.20 g of H2
NH4NO3(s) → N2O(g) + 2 H2O(g) A 0.03 mol sample of NH4NO3(s) is placed in a 1 L evacuated flask, which is then sealed and heated. The NH4NO3(s) decomposes completely according to the balanced equation above. The total pressure in the flask measured at 400 K is closest to which of the following? (The value of the gas constant, R, is 0.082 L atm mol-1 K-1.) A 3 atm B 1 atm C 0.5 atm D 0.1 atm E 0.03 atm
A 3 atm
A student was studying physical and chemical changes. The student carried out some procedures in the laboratory and recorded observations. For one of the procedures, the student concluded that a physical change took place, but not a chemical change. Which of the following could have been the results of the procedure? A A cube of metal was changed into a flat sheet of metal. B When two liquids at room temperature were combined in a beaker, the beaker became hot. C When two clear liquids were combined, the resulting mixture was cloudy. D When a colorless liquid was added to a blue liquid, the resulting solution was yellow.
A A cube of metal was changed into a flat sheet of metal.
A student combines a solution of NaCl(aq) with a solution of AgNO3(aq), and a precipitate forms. Which of the following is the balanced net ionic equation for the formation of the precipitate? A Ag+(aq)+Cl−(aq)→AgCl(s)Ag+(aq)+Cl−(aq)→AgCl(s) B Na+(aq)+NO3−(aq)→NaNO3(s)Na+(aq)+NO3−(aq)→NaNO3(s) C NaCl(aq)+AgNO3(aq)→NaNO3(s)+AgCl(aq)NaCl(aq)+AgNO3(aq)→NaNO3(s)+AgCl(aq) D NaCl(aq)+AgNO3(aq)→NaNO3(aq)+AgCl(s)
A Ag+(aq)+Cl−(aq)→AgCl(s)Ag+(aq)+Cl−(aq)→AgCl(s)
f 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
A Benzene, C6H6
Na2CO3(aq)+2HCl(aq)→2NaCl(aq)+H2O(l)+CO2(g) A student combined two colorless aqueous solutions. One of the solutions contained Na2CO3 as the solute and the other contained HCl. The chemical reaction that took place is represented by the equation above. What experimental result would be evidence that a chemical reaction took place when the solutions were combined? A Bubbles formed when the two solutions were combined. B The total volume of the mixture is close to the sum of the initial volumes. C The resulting solution is colorless. D The resulting solution conducts electricity.
A Bubbles formed when the two solutions were combined.
Zn(s)+CuSO4(aq)→Cu(s)+ZnSO4(aq) When a zinc plate is placed in an aqueous solution of copper sulfate, elemental copper forms, as represented by the equation above. Which of the following represents the reduction half-reaction of the reaction? A Cu2+(aq)+2e−→Cu(s) B Cu(s)→Cu2+(aq)+2e− C Zn(s)+2e−→Zn2−(aq) D Zn(s)→Zn2+(aq)+2e−
A Cu2+(aq)+2e−→Cu(s)
Based on the Brønsted-Lowry theory of acids and bases, which of the following species can act as both a conjugate acid and a conjugate base? A HS− B CH3COO− C H3O+ D NH4+
A HS−
2Mg(s)+SiCl4(l)→2MgCl2(s)+Si(s) Which of the following statements about the reaction represented above is correct? A It is an oxidation-reduction reaction, and Mg is oxidized. B It is an oxidation-reduction reaction, and electrons are transferred from SiCl4SiCl4 to Mg C It is an oxidation-reduction reaction, and the oxidation number of Cl changes from +4+4 to +2+2. D It is not an oxidation-reduction reaction because none of the oxidation numbers change.
A It is an oxidation-reduction reaction, and Mg is oxidized. B
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
A. 0.015 mole
What is the maximum number of moles of Al2O3 that can be produced by the reaction of 0.40 mol of Al with 0.40 mol of O2 ? A 0.10 mol B 0.20 mol C 0.27 mol D 0.33 mol E 0.40 mol
B 0.20 mol
Al(s)→Al3+(aq)+3e− Zn2+(aq)+2e−→Zn(s) The half-reactions for the oxidation-reduction reaction between Al(s) and Zn2+(aq) are represented above. Based on the half-reactions, what is the coefficient for Al(s) if the equation for the oxidation-reduction reaction is balanced with the smallest whole-number coefficients? A 1 B 2 C 3 D 4
B 2
C6H5COOH(aq)+NaOH(aq)→C6H5COONa(aq)+H2O(l) Which of the following identifies a conjugate acid-base pair in the reaction represented above?
B Acid C6H5COOH Conjugate base C6H5COO−
5Fe2+(aq)+MnO4−(aq)+8H+(aq)→5Fe3+(aq)+Mn2+(aq)+4H2O(l) Which of the following represents the oxidation half-reaction based on the balanced ionic equation shown above? A Fe2+(aq)+e−→Fe3+(aq) B Fe2+(aq)→Fe3+(aq)+e− C MnO4−(aq)→Mn2+(aq)+5e− MnO4−(aq)+5e−→Mn2+(aq)
B Fe2+(aq)→Fe3+(aq)+e−
H2C2O4(aq) + H2O(l) ⇄ H3O+(aq) + HC2O4-(aq) HC2O4-(aq) + H2O(l) ⇄ H3O+(aq) + C2O42-(aq) H2O(l) + H2O(l) ⇄ H3O+(aq) + OH- (aq) All the reactions represented above occur in an aqueous solution of oxalic acid. Which of the following represent a Brønsted-Lowry conjugate acid-base pair? A H2C2O4(aq) and C2O42-(aq) B HC2O4−(aq) and C2O42-(aq) C HC2O4-(aq) and H2O(aq) D H3O+(aq) and OH−(aq)
B HC2O4−(aq) and C2O42-(aq)
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.
B Hydrogen bonds between H2O molecules are broken.
Which of the following best describes the process represented above that takes place when NH3 is added to water? A It is a single replacement reaction in which an electron pair on NN is replaced with an HH atom. B It is an acid-base reaction in which a proton is exchanged from H2OH2O to NH3NH3. C It is a precipitation reaction in which NH4OHNH4OH, an insoluble solid, is produced. D It is an oxidation-reduction reaction in which the oxidation number of NN changes from −3−3 to −4−4.
B It is an acid-base reaction in which a proton is exchanged from H2OH2O to NH3NH3.
Which of the following is the conjugate acid of NH2- ? A NH2- B NH3 C H+ D NH4+ E H2O
B NH3
NH3(aq) + HCl(aq) ⇄ NH4+(aq) + Cl-(aq) The Brønsted-Lowry bases in the reaction represented above are A NH3(aq) and NH4+(aq) B NH3(aq) and Cl-(aq) C NH3(aq) and HCl(aq) D HCl(aq) and NH4+(aq) E HCl(aq) and Cl-(aq)
B NH3(aq) and Cl-(aq)
Which of the following is the correct net ionic equation of the reaction that occurs when aqueous solutions of ammonia and hydrochloric acid are combined? A NH3(aq)+HCl(aq)→NH4Cl(aq)NH3(aq)+HCl(aq)→NH4Cl(aq) B NH3(aq)+H+(aq)→NH4+(aq)NH3(aq)+H+(aq)→NH4+(aq) C NH3(aq)+HCl(aq)→NH4+(aq)+Cl−(aq)NH3(aq)+HCl(aq)→NH4+(aq)+Cl−(aq) D NH3(aq)+H+(aq)+Cl−(aq)→NH4+(aq)+Cl−(aq)
B NH3(aq)+H+(aq)→NH4+(aq)NH3(aq)+H+(aq)→NH4+(aq)
Which of the following particulate diagrams best shows the formation of water vapor from hydrogen gas and oxygen gas in a rigid container at 125C?
C
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
D. 2.00 mol
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
D. 20. g
HC2H3O2(aq)+OH−(aq)→C2H3O2−(aq)+H2O(l) A student carried out a titration using HC2H3O2(aq) and NaOH(aq). The net ionic equation for the neutralization reaction that occurs during the titration is represented above. The NaOH(aq) was added from a buret to the HC2H3O2(aq) in a flask. The equivalence point was reached when a total of 20.0mL of NaOH(aq) had been added to the flask. How does the amount of HC2H3O2(aq) in the flask after the addition of 5.0mL of NaOH(aq) compare to the amount of HC2H3O2(aq) in the flask after the addition of 1.0mL of NaOH(aq), and what is the reason for this result? A It is less because more HC2H3O2(aq)HC2H3O2(aq) reacted with the base. B It is the same because the half-equivalence point has not been reached. C It is the same because all of the coefficients in the neutralization equation are 1. D It is greater because HC2H3O2(aq)HC2H3O2(aq) is a proton donor.
A It is less because more HC2H3O2(aq)HC2H3O2(aq) reacted with the base.
C6H12O6+6O2→6CO2+6H2O The reaction between C6H12O6 and O2 is represented by the balanced equation above. In an experiment, 0.30mol of CO2 was produced from the reaction of 0.05mol of C6H12O6 with excess O2. The reaction was repeated at the same temperature and in the same container, but this time 0.60mol of CO2 was produced. Which of the following must be true? A The initial amount of C6H12O6C6H12O6 in the container must have been 0.10mol0.10mol. B Exactly 0.30mol0.30mol of C6H12O6C6H12O6 must have reacted because CC atoms were conserved. C Exactly 0.40mol0.40mol of O2O2 of must have reacted because the temperature and container volume are the same. D More than 0.60mol0.60mol of O2O2 must have reacted because it was present in excess.
A The initial amount of C6H12O6C6H12O6 in the container must have been 0.10mol0.10mol.
A student was given two clear liquids; a colorless liquid and a dark-blue liquid. The student was asked to combine the liquids in a beaker and record observations. Which of the following results, if true, would provide the best evidence that a chemical change took place when the liquids were combined? A The resulting mixture was cloudy. B The total volume of the mixture was equal to the sum of the initial volumes. C The resulting liquid was light blue. D The liquids formed two separate layers in the beaker.
A The resulting mixture was cloudy.
In the reaction between C5H5N(aq) and HCl(aq) represented above, C5H5N acts as A a Brønsted-Lowry base B a Brønsted-Lowry acid C the conjugate base of HClHCl D the conjugate acid of [C5H5NH]+
A a Brønsted-Lowry base
Mass of empty crucible-12.0g Mass of crucible and sample before heating-14.4g Mass of crucible and sample after heating- 16.0g 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? A The mass of the sample decreased, so physical changes occurred as the metal first melted and then boiled out of the crucible. B The mass of the sample increased, so a chemical change occurred when bonds formed between the metal 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.
B The mass of the sample increased, so a chemical change occurred when bonds formed between the metal and another substance.
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? A. 100% B. 67% C. 50% D. 33% E. 10%
B. 67%
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
B. 9.0 g
Al(s)→Al3+(aq)+3e− Sn2+(aq)+2e−→Sn(s) Based on the half-reactions represented above, which of the following is the balanced ionic equation for the oxidation-reduction reaction between Al(s) and Sn2+(aq) ? A Al(s)+Sn2+(aq)→Al3+(aq)+Sn(s)+e− B 3Al(s)+2Sn2+(aq)→3Al3+(aq)+2Sn(s) C 2Al(s)+3Sn2+(aq)→2Al3+(aq)+3Sn(s) D Al(s)+Sn2+(aq)+2e−→Al3+(aq)+Sn(s)+3e−
C 2Al(s)+3Sn2+(aq)→2Al3+(aq)+3Sn(s)
When students added 2.0g of NaI crystals to 100.mL of Pb(NO3)2(aq), a yellow precipitate formed. After the solution was filtered, the yellow solid was dried and weighed. Data from the experiment are shown in the table above. Which of the following claims is best supported by the observations? A A physical change occurred when a new yellow compound was formed. B A physical change occurred when the color of the NaI solid added changed to yellow when mixed with water. C A chemical change occurred when a yellow, insoluble compound with a larger mass than the original NaI formed. D A chemical change occurred when covalent bonds between the yellow solid and water were broken during drying.
C A chemical change occurred when a yellow, insoluble compound with a larger mass than the original NaI formed.
The particle diagram above represents an aqueous solution of a weak monoprotic acid. The white circles represent H atoms. Which of the following shows the species that act as a Brønsted-Lowry base and its conjugate acid, in that order, in the solution?
D
A chemistry teacher carried out several demonstrations, and students recorded their observations. For one of the demonstrations, a student concluded that a physical change took place, but not a chemical change. Which of the following observations could the student have made of the results of the demonstration? A Two colorless solutions were combined, and the resulting solution was pink. B When a solid was added to a liquid, sparks were produced. C One piece of solid substance was changed into small pieces. D When two solutions were combined, a precipitate formed.
C One piece of solid substance was changed into small pieces.
A student combines a solution of NaCl(aq) with a solution of AgNO3(aq), and a precipitate forms. Which of the following is evidence that ionic bonds formed during the precipitation? A The resulting solution is colorless. B The resulting solution conducts electricity. C The precipitate has a high melting point. D The temperature of the solution did not change significantly during the precipitation
C The precipitate has a high melting point.
A student was asked to formulate a hypothesis about what would happen if 100.mL of 0.1MNaOH(aq) at 25°C was combined with 100.mL of 0.1MMgCl2(aq) at 25°C. Which of the following hypotheses indicates that the student thought a chemical change would occur? A The volume of the resulting solution will be equal to the sum of the volumes of the original solutions. B The mass of the resulting solution will be equal to the sum of the masses of the original solutions. C The resulting solution would contain a precipitate. D The resulting solution will be clear.
C The resulting solution would contain a precipitate.
K2SO3(aq)+2HNO3(aq)→2KNO3(aq)+SO2(g)+H2O(l) According to the balanced chemical equation above, when 100.0mL of 0.100MK2SO3(aq) is mixed with 100.0mL of 0.200MHNO3(aq) at 30°C and 1 atm, the volume of SO2 gas produced is 0.24 L. If it is assumed that the reaction goes to completion, which of the the following changes would double the volume of SO2 produced at the same temperature and pressure? (For each change, assume that the other solutions and volumes remain the same.) A Using 200.0mL200.0mL of the 0.100MK2SO3(aq)0.100MK2SO3(aq), because it then becomes the reactant in excess B Using 200.0mL200.0mL of the 0.200MHNO3(aq)0.200MHNO3(aq), because the volume of SO2SO2 produced is inversely proportional to the number of moles at constant temperature and pressure C Using 200.0mL200.0mL of 0.100MK2SO3(aq)0.100MK2SO3(aq) and 200.0mL200.0mL of 0.200MHNO3(aq)0.200MHNO3(aq), because these are the required stoichiometric amounts D Using 400.0mL400.0mL of 0.100MK2SO3(aq)0.100MK2SO3(aq) and 200.0mL200.0mL of 0.200MHNO3(aq)0.200MHNO3(aq), because this provides the same number of moles of each reactant
C Using 200.0mL200.0mL of 0.100MK2SO3(aq)0.100MK2SO3(aq) and 200.0mL200.0mL of 0.200MHNO3(aq)0.200MHNO3(aq), because these are the required stoichiometric amounts
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
C. 20. mol
A student combines a solution of NaCl(aq) with a solution of AgNO3(aq), and a precipitate forms. Assume that 50.0mL of 1.0MNaCl(aq) and 50.0mL of 1.0MAgNO3(aq) were combined. According to the balanced equation, if 50.0mL of 2.0MNaCl(aq) and 50.0mL of 1.0MAgNO3(aq) were combined, the amount of precipitate formed would A double, because all of the coefficients are 1 B double, because the amount of one of the reactants was doubled C not change, because all of the coefficients are 1 D not change, because the amount of AgNO3(aq)AgNO3(aq) did not change
D not change, because the amount of AgNO3(aq)AgNO3(aq) did not change
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
D. 5
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
D. 5.0