CHEM043 Summit High School Redox Equation Chemistry Questions

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CHEM043

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2 units, multiple choice. See attached.

I really need to get an A on these. Please help! I am so stuck.
I submitted this earlier this morning, and someone got the answers back to me, but I received a low C on 2 of the units and an F on the third unit. So many of the answers were wrong, I didn't learn anything when studying the questions. And I have to take a final Thursday, so not having correct answers on the 3 units is not allowing me the ability to study.

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UNIT 7 1. In the following equation, what is the reducing agent? TiCl4(l) + O2(g) → TiO2(s) + 2Cl2(g) a. b. c. d. TiCl4 O2 Cl2 TiO2 2. After balancing the redox equation ClO- + OH- + N2O4 → ClO2-+H2O + NO2-, what are the coefficients, in order from left to right? a. 1, 2, 1, 1, 1, 1 b. 1, 2, 1, 1, 1, 2 c. 2, 2, 1, 1, 2, 2 d. 1, 2, 2, 1, 1, 2 3. Determine the oxidation number of S in Al2S3. a. +6 b. -2 c. -3 d. +3 4. Which of the following is true in redox reactions? a. The reducing agent is the substance reduced. b. Both oxidizing and reducing agents are oxidized. c. The oxidizing agent is the substance oxidized. d. The oxidizing agent is the substance reduced. 5. Consider the following reaction: Ba(s) + F2(g) → BaF2. Which of the following statements is true? a. The fluorine atom is gaining electrons; therefore, it is reduced. b. The barium atom is losing electrons; therefore, it is reduced. c. The fluorine atom is losing electrons; therefore, it is reduced. d. The barium atom is gaining electrons; therefore, it is oxidized. 6. What takes place at the cathode: a. Reduction b. The electrode loses mass c. Loss of electrons d. Oxidation 7. Determine the oxidation number of S in SO2. a. +4 b. -2 c. +2 d. -4 8. When the following redox equation is correctly balanced in acid, what is the coefficient of the NO3–? H3PO3 + NO3– → PO43– + N2O4 a. b. c. d. 1 4 3 2 9. How many electrons are being exchanged in the balanced redox equation Ga + Ag+→ Ga+ + Ag? a. b. c. d. 3 4 2 1 10. In the reaction represented by the equation: Ni → Ni2+ + 2e–, what happens to the species Ni? a. It is oxidized. b. It is reduced. c. It is neutralized. d. It is made disproportionate. 11. Determine the oxidation number of Cr in Cr2O7-2. a. +2 b. +3 c. 0 d. +6 12. What is the purpose of the wire in an electrochemical cell a. Is the physical barrier between the anode and the cathode b. Acts as the pathway for electrons to travel from one electrode to the other c. allows ions to move between the two half-cells d. Balances the pH of the two solutions 13. Determine the oxidation number of Pd in Pd(NO2)4. a. +4 b. +3 c. 0 d. +2 14. Determine the oxidation number of Mn in KMnO4. a. +1 b. +7 c. –2 d. +6 15. In the following equation, which species is reduced? TiCl4(l) + O2(g) → TiO2(s) + 2Cl2(g) a. b. c. d. Ti Cl O TiO2 16. In cell diagram notation, which half is the site of reduction? a. Left b. Neither side c. Both sides d. Right 17. A species whose oxidation number decreases in a reaction is said to be which of the following? a. oxidized b. elcotrolized c. reduced d. autooxidized 18. What species is oxidized in the following oxidation-reduction equation? H+ + I– + Cr2O72–→ Cr3+ + I2 + H2 O a. b. c. d. O Cr I H 19. What species is reduced in the following oxidation-reduction equation? H+ + I– + Cr2O72–→ Cr3+ + I2 + H2 O a. b. c. d. Cr O I H 20. Which of the following statements correctly describes the redox equation 6H+ + MnO4- + 5CO → 5CO2 + Mn2+ + 3H2O? a. It is correctly balanced. b. It is correctly balanced for charge but not for the number of atoms. c. It is correctly balanced for the number of atoms but not for charge. d. It is not balanced for the number of atoms or charge. 21. What is the most common oxidation number of oxygen when combined with metal elements other than itself? a. -2 b. +1 c. +2 d. 0 22. In a voltaic cell with electrodes made from nickel and cobalt, the cobalt is plated onto the electrode as Co from the Co+2 solution. What is the cobalt electrode called? a. oxidizing electrode b. metal electrode c. anode d. cathode 23. What takes place at the anode: a. Oxidation b. Gain of electrons c. The electrode gains mass d. Reduction 24. What does the algebraic sum of the oxidation numbers of the atoms in a neutral compound always equal? a. 0 b. –1 c. +1 d. any whole number 25. In a dry cell battery discussed in this lesson, the sides and bottom of the casing are made of which metal? a. zinc b. chromium c. gold d. nickel 26. When balancing redox equations, you need to balance the charge. What would you use to balance the charge if the equation were being balanced in acid? a. H+ b. H2 O c. OHd. none of these 27. When the following redox equation is balanced correctly in acid, what is the coefficient of the HNO3? HNO3 + H3PO3→ H3PO4 + NO a. b. c. d. 4 3 2 1 28. All free elements have oxidation numbers equal to what? a. the number of electrons b. zero c. the number of protons d. their charge 29. In a correctly balanced redox equation, if the oxidation reaction lost five electrons how many electrons did the reduction reaction take? a. No relationship exists between the two numbers. b. 4 c. 5 d. 6 30. When an automobile battery is starting a car, which of the following occurs? a. Energy as heat is converted to energy of motion. b. Chemical energy is converted to electrical energy. c. Electrical energy is converted to chemical energy. d. Energy of motion is converted to energy as heat. Unit 8 1. What is nuclear fission? a. When an unstable nucleus emits radiation to become a new element b. When chemical bonds are broken and reformed in new combinations c. When a large nucleus is split into two intermediate sized nuclei d. When two smaller nuclei combine to form a larger nucleus 2. What is the correct nuclear symbol for an isotope that has 82 protons, 127 neutrons, and 78 electrons? a. b. c. d. 3. What does the 101 in represent? a. the number of neutrons b. the nuclide number c. the atomic number d. the mass number 4. What is the correct order of increasing energy (lowest to highest) for the following waves: red, green, violet, yellow? a. violet, green, red, yellow b. violet, green, yellow, red c. red, yellow, green, violet d. violet, red, yellow, green 5. The isotope 206Po has a half-life of 8.8 days. If you have 5.68 x 1025 atoms of this isotope, how long will it take for the sample to decay to 3.55 x 1024 atoms? a. 26.4 days b. 35.2 days c. 2.20 days d. 141 days 6. Complete this nuclear equation: 58Mn → +10e + ___. a. 57Cr b. 57Fe c. 58Fe d. 58Cr 7. Complete this nuclear equation: 135Cs → β–+ ___. a. 134Ba b. 135Ba c. 134Cs d. 135Rn 8. Which of the illustrations below represents a fission reaction? a b c d 9. Which of the following radioactive decay processes does not reduce the atomic number of a nuclide? a. alpha decay b. electron capture c. beta decay d. positron decay 10. Which of the following is the symbol for an alpha particle? a. b. c. d. 11. Which is a source of radiation we are exposed to during our lifetime? a. bricks b. airport security c. smoke detectors d. all of the above 12. What type of wave has the highest frequency? a. microwaves b. infrared c. x-rays d. radio 13. Many foods contain a small amount of potassium-40. Its decay product is chlorine-36. Identify the emission particle from potassium-40. a. beta-plus particle b. alpha particle c. beta-minus particle d. electron capture 14. If the particle that starts a nuclear reaction is also one of the products, the process is a a. chain reaction. b. nuclear fusion. c. neutron bombardment. d. neutron emission. 15. Balance the following equation: a. b. c. + ____ → d. 16. Write a balanced nuclear equation for the formation of from beta-minus emission. a b c d 17. What type of wave has the longest wavelength? a. green b. blue c. yellow d. red 18. Complete this nuclear equation: 228Ra → β- + ___ ? a. 228Fr b. 228Ac c. 227Fr d. 227Ac 19. Which of the following forms of radiation has the greatest penetrating power? a. beta particles b. positrons c. gamma rays d. alpha particles 20. What does the 2 in represent? a. the number of protons and neutrons b. the atomic number c. the mass number d. the number of neutrons 21. Balance the following equation: + → + ___ a. b. c. d. 22. What type of radiation is used in chemotherapy and radiation therapy to treat cancer? a. positrons b. gamma rays c. alpha particles d. beta minus 23. Of the following forms of radioactivity, select all that would penetrate paper. 1. positrons 2. gamma rays 3. alpha particles 4. beta minus particles a. 1 and 2 b. 3 and 4 c. 2 and 4 d. 2, 3, and 4 e. 1, 2 and 4 24. You are performing an experiment that uses 113Ag. 113Ag is radioactive, decays by beta-minus emission and has a half-life of 5.3 hours. It requires 42.4 hours to ship the material from the warehouse to your laboratory. How many grams should you order if the experiment requires that you have 4 grams to begin the experiment? a. 32 g b. 1.56 x 10-2 g c. 1.02 x 103 g d. 510 g 25. Which of the following lists ranks nuclear radiation from most massive to least massive? a. alpha, beta, and gamma b. beta, gamma, and alpha c. gamma, alpha, and beta d. gamma, beta, and alpha 26. Alpha particles are a. electromagnetic waves b. neutrons c. helium nuclei d. electrons 27. The iodine-131 nuclide has a half-life of 8.0 days. If you originally have a 123 g sample, after 24 days how much will you have? a. 48 g b. less than 1 g c. 41 g d. 15.4 g 28. Which are not products of the fission of promethean? a. energy b. neutrons c. alpha particles d. medium-weight nuclei 29. Which of the following particles has the same mass as an electron but a positive charge and is sometimes emitted from the nucleus during radioactive decay? a. alpha particle b. positron c. gamma ray d. beta particle 30. Complete this nuclear equation: 222Rn →4He + ___. a. 218Po b. 226Po c. 218Ra d. 226Ra Review 2 0% F The following formulas may be helpful: 1. When an automobile battery is charging, which of the following is accurate? Electrical energy is converted to chemical energy. Energy as heat is converted to energy of motion. Energy of motion is converted to energy as heat. Chemical energy is converted to electrical energy. 2. The molecular weight of nitrogen gas (N2) is 28 g/mol. What is the mass of a single nitrogen atom? 1.17 x 10–23 g 4.65 x 10–23 g 3.13 x 10–1 g 2.33 x 10–23 g 3. Is the following reaction endothermic or exothermic? 2 H2 + O2 --> 2 H2O H= -571.6 kJ exothermic endothermic 4. A student is given a soluble sodium salt containing one of eight possible anions (negative ions): acetate, chloride, bromide, iodide, sulfide, sulfate, and phosphate. The student adds some BaCl2 solution to the salt solution. A precipitate forms. Which anions could be present? CH3COO– only S2–, SO42–and PO43– Br– only Cl–, Br–, and I– 5. At what temperature will 35 g of KClO3 dissolve? 30°C 60°C 75°C 70°C 6. Which of the following is a strong acid? HF HNO2 H2SO3 HI 7. What is the atomic particle that has a mass of 0 amu and a charge of –1? a neutron an electron an alpha particle a proton 8. In the reaction represented by the equation Brönsted-Lowry acid Arrhenius Brönsted-Lowry base Lewis base 9. Which is a source of radiation we are exposed to during our lifetime? airplanes x-rays food all of the above 10. What are alpha particles? protons helium nuclei neutrons electrons 11. What is the oxidation number of phosphorous in H2PO4– ? +6 +5 –1 0 , what is H2O? 12. What is the correct equilibrium constant expression for the equation 2A2B + 3CD ⇄ A4D + C3B2? 13. In which of the following do we find acetic acid? apples lemons vinegar sour milk 14. What is the oxidizing agent in the oxidation-reduction equation H2PO2–+ SbO2– → H3PO3 + Sb? H3PO3 SbO2– H2PO2– Sb 15. What is the molarity of a solution that contains 0.202 mol KCl in 7.98 L solution? 0.0132 M 0.459 M 0.0253 M 1.363 M 16. What is the symbol used in chemistry for the unit called a mole? mo m mol ml 17. The iodine-131 nuclide has a half-life of 8.0 days. If you originally have a 123 g sample, after 24 days how much will you have? less than 1 g 41 g 15.4 g 48 g 18. Convert the pressure 1.30 atm to kPa. 132 kPa 115 kPa 245 kPa 2 kPa 19. What is the conjugate acid of HPO42- ? OHH2O H2PO4PO4320. Which of the following generally have the lowest penetrating ability? gamma rays beta particles alpha particles all have the same penetrating ability 21. How many moles of air are there in a 125 mL flask if the pressure is 739 torr and the temperature is 18°C? 8.22 x 10–2 mol 5.09 mol 197 mol 5.09 x 10–3 mol 22. Which of the following equations represents an oxidation-reduction reaction? HCl + NaBr → HBr + NaCl H2→ 2H H2 + Cl2 → 2HCl 23. Why does a can collapse when a vacuum pump removes air from inside the can? The vacuum pump creates a force that crushes the can. The inside and outside forces balance out and crush the can. The atmosphere exerts pressure on the inside of the can and crushes it. The unbalanced outside force from atmospheric pressure crushes the can. 24. Which of the following is true about the redox equation ? It is correctly balanced for charge but not for number of atoms. It is not balanced for number of atoms or charge. It is correctly balanced. It is correctly balanced for number of atoms but not for charge. 25. Balance the following equation: → ____ + . 26. What is the oxidation number for C in table sugar, C12H22O11? +2 +3 1 0 27. The expression P = kT is a statement of which of the following laws? Boyle’s law Avogadro’s law Gay-Lussac’s law Charles’s law 28. Which of the illustrations below represents a fission reaction? a b c d 29. Which of the following affects reaction rate? the nature of reactants surface area of reactants temperature all of the above 30. A gas has a volume of 5 L at a certain pressure. How must the pressure be changed to double the volume of the gas at constant temperature? The pressure must be doubled. The pressure must be quadrupled. The pressure must be halved. There is not enough information to decide. 31. Balance the following equation: + ____→ + 32. Convert 14.2 grams Pb(NO3)2 (MW = 331 g/mol) to molecules Pb(NO3)2. 7.12 x 10–26 molecules 2.85 molecules 7.81 x 1021 molecules 2.58 x 1022 molecules 33. What is the OH– concentration of an aqueous solution with a pH of 4.45? 7.1x10–5 M 9.55 M 3.5x10–5 M 2.8x10–10 M 34. What type of wave has the longest wavelength? red blue green yellow 35. After balancing the redox equation FeCl3 + Zn → ZnCl2 + Fe, what are the coefficients, in order from left to right? 1, 1, 1, 1 2, 3, 3, 2 4, 3, 3, 4 2, 2, 1, 2 36. According to the Arrhenius definition, a base is substance that when dissolved in water increases the concentration of which of the following? hydroxide ion protons hydronium ion electrolytes 37. Which statement about nuclear reactions is not true? Nuclear power plants use fission of uranium. In fission, the total mass of the reactants equals the total mass of the products. Heat and light in the sun are produced by hydrogen fusion reactions. In fission, nuclei are split, and in fusion, nuclei are combined. 38. What does 46 represent in the symbol ? the sum of the protons and neutrons the number of electrons number of protons the number of neutrons 39. The volume of a gas is 15 L when the temperature is 20°C. If the temperature is increased to 40°C without changing the pressure, what is the new volume? 7.5 L 30 L 16 L 14 L 40. In which system does a spontaneous redox reaction produce electrical energy? electrolytic cell half-cell electroplating cell electrochemical cell 41. In the equation shown, what represents the concentrations of the reactants? [Y] and [Z] [W] and [X] 42. Convert 414°C to K. 687 K –229 K 141 K 317 K 43. What is the pH of a solution at 25°C in which [OH–]= 3.8 x 10–5 M? 4.42 11.08 4.79 9.58 44. If the pressure on the equilibrium system N2(g) + O2(g) ⇄ 2NO(g) decreases, which of the following will occur? the quantity of NO(g) will increase the quantity of N2(g) will decrease the quantity of NO(g) will decrease the quantities in the system will not change 45. Which of the following is perchloric acid? HClO HClO2 HClO4 HClO3 46. If solutions of Co(NO3)3 and KOH are mixed, how many precipitation reactions will occur? three zero one two 47. Laughing gas, or nitrous oxide (N2O), is often used by a dentist to put you to sleep during a painful dental procedure. What is the molecular weight of nitrous oxide? 44 g/mol 78 g/mol 52 g/mole 30 g/mol 48. What is the term for the substance that is dissolved when a solution is formed? solvent solute nonelectrolyte electrolyte 49. Which of the following compounds are not soluble in water? Co(CH3COO)3 (NH4)3PO4 NaNO3 Hg2Cl2 50. Raising the temperature of reactants in a system does which of the following? increases the average kinetic energy of the molecules has no effect on the average kinetic energy of molecules decreases the average kinetic energy of the molecules decreases the rate of collision of molecules 51. What is the approximate boiling point of CCl4 if the atmospheric pressure on the surface of the liquid is 90 kPa? 95°C 20°C 101.3°C 80°C 52. When a solute is placed in a solvent each of the following occur except which of the following? The osmotic pressure is increased. The freezing point is increased. The boiling point is increased. The vapor pressure is lowered.
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Running Head: CHEMISTRY QUESTIONS

1

Chemistry questions
Name
Tutor
Institution
Date

CHEMISTRY QUESTIONS

UNIT 7
1. In the following equation, what is the reducing agent?
TiCl4(l) + O2(g) → TiO2(s) + 2Cl2(g)
a. TiCl4
b. O2
c. Cl2
d. TiO2
Answer = c, Cl2 is the reducing agent since it undergoes oxidation process.
2. After balancing the redox equation ClO- + OH- + N2O4 → ClO2-+H2O + NO2-, what are the
coefficients, in order from left to right?
a. 1, 2, 1, 1, 1, 1
b. 1, 2, 1, 1, 1, 2
c. 2, 2, 1, 1, 2, 2
d. 1, 2, 2, 1, 1, 2
Answer = b , 1,2,1,1,1,2
3 Determine the oxidation number of S in Al2S3.
a. +6
b. -2
c. -3
d. +3
Answer =b
4 Which of the following is true in redox reactions?
a. The reducing agent is the substance reduced.
b. Both oxidizing and reducing agents are oxidized.
c. The oxidizing agent is the substance oxidized.
d. The oxidizing agent is the substance reduced.

2

CHEMISTRY QUESTIONS
Answer = d, the oxidizing agent is the substance reduced
5 Consider the following reaction: Ba(s) + F2(g) → BaF2. Which of the following statements is
true?
a. The fluorine atom is gaining electrons; therefore, it is reduced.
b. The barium atom is losing electrons; therefore, it is reduced.
c. The fluorine atom is losing electrons; therefore, it is reduced.
d. The barium atom is gaining electrons; therefore, it is oxidized.
answer = a, the fluorine atom is gaining electrons; therefore, it is reduced
6 What takes place at the cathode:
a. Reduction
b. The electrode loses mass
c. Loss of electrons
d. Oxidation
Answer= a, reduction.
7 Determine the oxidation number of S in SO2.
a. +4
b. -2
c. +2
d. -4
Answer = a, +4
8 When the following redox equation is correctly balanced in acid, what is the coefficient of the
NO3–?
H3PO3 + NO3– → PO43– + N2O4
a. 1
b. 4
c. 3
d. 2
Answer =c 3

9 How many electrons are being exchanged in the balanced redox equation
Ga + Ag+→ Ga+ + Ag?
a. 3
b. 4
c. 2

3

CHEMISTRY QUESTIONS

4

d. 1
Answer = d , 1
10 In the reaction represented by the equation: Ni → Ni2+ + 2e–, what happens to the species Ni?
a. It is oxidized.
b. It is reduced.
c. It is neutralized.
d. It is made disproportionate.
Answer =a, It is oxidized
11 Determine the oxidation number of Cr in Cr2O7-2.
a. +2
b. +3
c. 0
d. +6
Answer =d.+6
12 What is the purpose of the wire in an electrochemical cell
a. Is the physical barrier between the anode and the cathode
b. Acts as the pathway for electrons to travel from one electrode to the other
c. allows ions to move between the two half-cells
d. Balances the pH of the two solutions
Answer = b, Acts as the pathway for electrons to travel from one electrode to the other
13 Determine the oxidation number of Pd in Pd(NO2)4.
a. +4
b. +3
c. 0
d. +2
Answer = a, +4
14 Determine the oxidation number of Mn in KMnO4.
a. +1
b. +7
c. –2
d. +6
Answer = , b +7
15 In the following equation, which species is reduced?
TiCl4(l) + O2(g) → TiO2(s) + 2Cl2(g)
a. Ti
b. Cl

CHEMISTRY QUESTIONS
c. O
d. TiO2
Answer = C, O
16 In cell diagram notation, which half is the site of reduction?
a. Left
b. Neither side
c. Both sides
d. Right
Answer = d, right side
17 A species whose oxidation number decreases in a reaction is said to be which of the
following?
a. Oxidized
b. elcotrolized
c. reduced
d. autooxidized
Answer = c, reduced
18 What speacies is oxidized in the following oxidation-reduction equation?
H+ + I– + Cr2O72–→ Cr3+ + I2 + H2 O
a. O
b. Cr
c. I
d. H
Answer = c ,I.
19 What species is reduced in the following oxidation-reduction equation?
H+ + I– + Cr2O72–→ Cr3+ + I2 + H2 O
a. Cr
b. O
c. I
d. H
Answer= a, Cr.
20 Which of the following statements correctly describes the redox equation 6H+ + MnO4- +
5CO → 5CO2 + Mn2+ + 3H2O?
a. It is correctly balanced.
b. It is correctly balanced for charge but not for the number of atoms.

5

CHEMISTRY QUESTIONS
c. It is correctly bal...


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