General Organic And Biological Chemistry 2nd Edition By Laura D. Frost- Test Bank Instant Download - Complete Test Bank With Answers Sample Questions Are Posted Below Chapter 5: Chemical Reactions 1. The law of conservation of mass states that A) Atoms cannot be created or destroyed in a chemical …
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General Organic And Biological Chemistry 2nd Edition By Laura D. Frost- Test Bank
Instant Download – Complete Test Bank With Answers
Sample Questions Are Posted Below
Chapter 5: Chemical Reactions
| 1. | The law of conservation of mass states that | |
| A) | Atoms cannot be created or destroyed in a chemical reaction. | |
| B) | Molecules cannot be created or destroyed in a chemical reaction. | |
| C) | Compounds cannot be created or destroyed in a chemical reaction. | |
| D) | Heat cannot be created or destroyed in a chemical reaction. | |
| Ans: A Difficulty: Easy | ||
| 2. | The Greek letter delta (D) may be written over the reaction arrow in a chemical equation to indicate that | |
| A) | Heat is generated when the reaction occurs. | |
| B) | A catalyst is needed for the reaction to occur. | |
| C) | Water is needed for the reaction to occur. | |
| D) | Heat is needed for the reaction to occur. | |
| Ans: D Difficulty: Easy | ||
| 3. | Which chemical equation is properly balanced? | |||
| A) | SO2 + O2 + H2O ® H2SO4 | C) | 4 SO2 + O2 + 4 H2O ® 4 H2SO4 | |
| B) | 2 SO2 + O2 + 2 H2O ® 2 H2SO4 | D) | SO2 + O2 + 4 H2O ® 2 H2SO4 | |
| Ans: B Difficulty: Easy | ||||
| 4. | In the chemical equation 2 Co(NO3)3 + 3 (NH4)2S ® Co2S3 + 6 NH4NO3 , how many nitrogen atoms are on each side of the equation? |
| A) 2 B) 3 C) 6 D) 12 E) 16 | |
| Ans: D Difficulty: Medium |
| 5. | Write a balanced chemical equation for the reaction of acetone (C3H6O) with oxygen (O2) to form carbon dioxide (CO2) and water (H2O). | |||
| A) | C3H6O + O2 ® CO2 + H2O | C) | 6 C3H6O + 8 O2 ® 6 CO2 + 6 H2O | |
| B) | C3H6O + 4 O2 ® 3 CO2 + 3 H2O | D) | 3 CO2 + 3 H2O ® C3H6O + 4 O2 | |
| Ans: B Difficulty: Medium | ||||
| 6. | How many carbon atoms are in 3.85 mol of carbon? | |||
| A) | 3.85 carbon atoms | D) | 2.32 × 1024 carbon atoms | |
| B) | 23.2 carbon atoms | E) | 6.40 × 10–24 carbon atoms | |
| C) | 6.02 × 1023 carbon atoms | |||
| Ans: D Difficulty: Easy | ||||
| 7. | How many iron atoms are in 0.32 mol of Fe2O3? | |||
| A) | 3.9 × 1023 iron atoms | D) | 1.1 × 10–24 iron atoms | |
| B) | 1.9 × 1023 iron atoms | E) | 6.02 × 1023 iron atoms | |
| C) | 3.9 iron atoms | |||
| Ans: A Difficulty: Medium | ||||
| 8. | How many moles of chloroethylene (C2H3Cl) contain 5.47 × 1026 molecules? | |||
| A) | 3.29 × 1050 mol of C2H3Cl | C) | 909 mol of C2H3Cl | |
| B) | 5.47 × 1026 mol of C2H3Cl | D) | 5450 mol of C2H3Cl | |
| Ans: C Difficulty: Medium | ||||
| 9. | What is the formula weight of KCl? |
| A) 74.55 amu B) 66.42 amu C) 36.00 amu D) 1386 amu | |
| Ans: A Difficulty: Easy |
| 10. | What is the formula weight of Co(NO3)3? |
| A) 88.94 amu B) 244.96 amu C) 216.94 amu D) 148.96 amu | |
| Ans: B Difficulty: Medium |
| 11. | What is the mass of 3.81 mol of PH3? |
| A) 34.0 g B) 3.81 g C) 8.92 g D) 130. g | |
| Ans: D Difficulty: Medium |
| 12. | How many moles of carbon dioxide are in 211 g of carbon dioxide? | |||
| A) | 929 mol of CO2 | C) | 167 mol of CO2 | |
| B) | 4.79 mol of CO2 | D) | 0.209 mol of CO2 | |
| Ans: B Difficulty: Medium | ||||
| 13. | Aspartic acid is an amino acid used to synthesize proteins. What is the molar mass of aspartic acid shown below?
|
| A) 121.09 g/mol B) 133.11 g/mol C) 132.09 g/mol D) 117.0 g/mol | |
| Ans: B Difficulty: Easy |
| 14. | Which sample contains the largest number of molecules? |
| A) 100 g of CO2 B) 100 g of CH4 C) 100 g of CBr4 D) 100 g of CHBr3 | |
| Ans: B Difficulty: Difficult |
| 15. | How many moles of sulfur trioxide are formed from 3 moles of sulfur dioxide using the given balanced equation?
2 SO2 + O2 ® 2 SO3 |
|||
| A) | 1 mol of SO3 | D) | 5 mol of SO3 | |
| B) | 2 mol of SO3 | E) | 6 mol of SO3 | |
| C) | 3 mol of SO3 | |||
| Ans: C Difficulty: Easy | ||||
| 16. | How many moles of sulfur trioxide are formed from 3 moles of oxygen using the given balanced equation?
2 SO2 + O2 ® 2 SO3 |
|||
| A) | 1 mol of SO3 | D) | 5 mol of SO3 | |
| B) | 2 mol of SO3 | E) | 6 mol of SO3 | |
| C) | 3 mol of SO3 | |||
| Ans: E Difficulty: Medium | ||||
| 17. | Consider the reaction: 2 Al(OH)3 + 3 H2SO4 ® Al2(SO4)3 + 6 H2O. How many grams of Al2(SO4)3 are generated when 152 g of H2SO4 reacts? | |||
| A) | 530. g of Al2(SO4)3 | D) | 43.6 g of Al2(SO4)3 | |
| B) | 1590 g of Al2(SO4)3 | E) | 131 g of Al2(SO4)3 | |
| C) | 177 g of Al2(SO4)3 | |||
| Ans: C Difficulty: Difficult | ||||
| 18. | A balanced chemical equation tells the number of _____ of each reactant that combine and the number of _____ of each product formed. |
| A) Grams, grams B) Grams, moles C) Moles, grams D) Moles, moles | |
| Ans: D Difficulty: Easy |
| 19. | Suppose the theoretical yield in a reaction is 10.5 g and the percent yield is 75.5%. What is the actual yield of product obtained? |
| A) 793 g B) 7.93 g C) 13.9 g D) 0.139 g | |
| Ans: B Difficulty: Medium |
| 20. | Consider the oxidation of sodium metal to sodium oxide described by the balanced equation:
4 Na + O2 ® 2 Na2O. What is the theoretical yield of Na2O in grams from 9.0 mol of O2? |
|||
| A) | 11 g of Na2O | D) | 280 g of Na2O | |
| B) | 410 g of Na2O | E) | 560 g of Na2O | |
| C) | 1,100 g of Na2O | |||
| Ans: C Difficulty: Difficult | ||||
| 21. | Consider the oxidation of sodium metal to sodium oxide described by the balanced equation:
4 Na + O2 ® 2 Na2O. If 2.55 mol of sodium reacts, and 75.0 g of Na2O is produced, what is the percent yield? |
| A) 94.9% yield B) 34.0% yield C) 47.5% yield D) 190.% yield | |
| Ans: A Difficulty: Difficult |
| 22. | If a synthesis has four steps and each step has a 75% yield (0.75 written as a decimal), what is the overall percent yield? |
| A) 75% B) 19% C) 56% D) 32% E) 42% | |
| Ans: D Difficulty: Medium |
| 23. | Potassium metal (K) reacts violently when added to water according to the balanced equation:
2 K(s) + 2 H2O(l) ® 2 KOH(aq) + H2(g). How many moles of H2O are needed to react completely with 7.54 mol of K? |
|||
| A) | 2 mol of H2O | C) | 15.1 mol of H2O | |
| B) | 7.54 mol of H2O | D) | 3.77 mol of H2O | |
| Ans: B Difficulty: Medium | ||||
| 24. | Tin (II) fluoride can be made by the following reaction: Sn(s) + 2 HF(g) ® SnF2(s) + H2(g). What is the maximum amount of SnF2 that can be produced when 0.480 moles of Sn are mixed with 0.720 moles of HF? | |||
| A) | 0.360 moles of SnF2 | D) | 0.720 moles of SnF2 | |
| B) | 0.480 moles of SnF2 | E) | 1.20 moles of SnF2 | |
| C) | 0.600 moles of SnF2 | |||
| Ans: A Difficulty: Difficult | ||||
| 25. | Identify the species that is oxidized and the species that is reduced in the reaction:
2 I– + Cl2 ® 2 Cl– + I2 |
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| A) | I– is oxidized and Cl2 is reduced. | D) | I2 is oxidized and Cl– is reduced. | |
| B) | Cl2 is oxidized and I– is reduced. | E) | Cl2 is oxidized and Cl– is reduced. | |
| C) | I2 is oxidized and I– is reduced. | |||
| Ans: A Difficulty: Medium | ||||
| 26. | What are the two half reactions that show how many electrons are gained or lost by each species in the reaction:
Ni2+(aq) + Mg(s) ® Ni(s) + Mg2+(aq)? |
|
| A) | Ni2+(aq) + e– ® Ni(s) and Mg(s) ® Mg2+(aq) + e– | |
| B) | Ni2+(aq) + 2 e– ® Ni(s) and Mg(s) ® Mg2+(aq) + 2 e– | |
| C) | Ni2+(aq) ® Ni(s) + 2 e– and Mg(s) + 2 e– ® Mg2+(aq) | |
| D) | Ni2+(aq) ® Ni(s) + e– and Mg(s) + e– ® Mg2+(aq) | |
| E) | Ni2+(aq) + 2 e– ® Ni(s) and Mg(s) + 2 e– ® Mg2+(aq) | |
| Ans: B Difficulty: Medium | ||
| 27. | Which quantity has the greatest mass? | |
| A) | 2.0 mol of Na | |
| B) | 2.0 mol of Na2O | |
| C) | 2.0 mol of NaCl | |
| D) | 2.0 mol of O2 | |
| E) | All of these quantities have the same mass. | |
| Ans: B Difficulty: Medium | ||
| 28. | How many moles of sodium chloride (table salt, NaCl, molar mass 58.44 g/mol) are contained in a 1.00 lb box of table salt? | |||
| A) | 26,500 mol of NaCl | D) | 7.77 mol of NaCl | |
| B) | 4.68 × 1024 mol of NaCl | E) | 0.129 mol of NaCl | |
| C) | 58.44 mol NaCl | |||
| Ans: D Difficulty: Medium | ||||
| 29. | In the balanced redox reaction: 2 Cu(s) + S(s) ® Cu2S(s), how many electrons are gained or lost by each copper atom? | |
| A) | Each copper atom gains two (2) electrons | |
| B) | Each copper atom gains one (1) electron | |
| C) | Each copper atom loses one (1) electron | |
| D) | Each copper atom loses two (2) electrons | |
| Ans: C Difficulty: Difficult | ||
| 30. | Consider the mixture of Cl2 and F2 in a closed container as illustrated below. What will the contents of the container look like if the molecules undergo the reaction:
Cl2(g) + 3 F2(g) ® 2 ClF3(g)?
|
|||
| A) | C) | |||
| B) | D) | |||
| Ans: B Difficulty: Difficult | ||||
| 31. | In the balanced redox reaction: 2 C2H6(g) + 7 O2(g) ® 4 CO2(g) + 6 H2O(g), which species is oxidized? |
| A) C2H6(g) B) O2(g) C) CO2(g) D) H2O(g) | |
| Ans: A Difficulty: Medium |
| 32. | In the balanced redox reaction: 2 C2H6(g) + 7 O2(g) ® 4 CO2(g) + 6 H2O(g), which species is reduced? |
| A) C2H6(g) B) O2(g) C) CO2(g) D) H2O(g) | |
| Ans: B Difficulty: Medium |
| 33. | How many grams of oxygen gas are required to completely react with 77.28 g of ethane (C2H6) in the balanced redox reaction: 2 C2H6(g) + 7 O2(g) ® 4 CO2(g) + 6 H2O(g)? | |||
| A) | 77.28 g of O2(g) | D) | 143.9 g of O2(g) | |
| B) | 8.995 g of O2(g) | E) | 287.8 g of O2(g) | |
| C) | 23.50 g of O2(g) | |||
| Ans: E Difficulty: Difficult | ||||
| 34. | How many carbon atoms are in 77.28 g of ethane (C2H6)? | |||
| A) | 2.570 carbon atoms | D) | 1.238 × 1025 carbon atoms | |
| B) | 1.548 × 1024 carbon atoms | E) | 3.094 × 1024 carbon atoms | |
| C) | 5.140 carbon atoms | |||
| Ans: E Difficulty: Difficult | ||||
| 35. | What is the molar mass of the compound show below?
|
|||
| A) | 90.13 amu | D) | 91.14 g/mol | |
| B) | 93.13 g/mol | E) | 93.13 amu | |
| C) | 90.13 g/mol | |||
| Ans: D Difficulty: Easy | ||||
| 36. | What is the mass of 3.4 × 1020 molecules of ethanol (C2H6O) expressed in milligrams? | |||
| A) | 0.026 mg of ethanol | C) | 26,000 mg of ethanol | |
| B) | 0.012 mg of ethanol | D) | 26 mg of ethanol | |
| Ans: D Difficulty: Difficult | ||||
| 37. | The chemical equation: KClO3(s) ® KCl(s) + O2(g) is not balanced. Balance this equation, then select the statement that best describes the balanced equation. | |
| A) | The balanced equation will have six atoms of oxygen on each side of the equation. | |
| B) | The balanced equation will have one atom of chlorine on each side of the equation. | |
| C) | The balanced equation will have an O3 on the product side of the equation. | |
| D) | The balanced equation will have a coefficient of 1 in front of KCl. | |
| Ans: A Difficulty: Easy | ||
| 38. | Sodium fluoride can be produced from the reaction between sodium metal and fluorine gas. Which of the following represents the balanced chemical equation for this reaction? | |||
| A) | 2 Na(s) + F2(g) ® 2 NaF(s) | C) | Na+(s) + F–(g) ® NaF(s) | |
| B) | Na(s) + F2(g) ® NaF2(s) | D) | 2 Na(s) + F2(g) ® Na2F2(s) | |
| Ans: A Difficulty: Medium | ||||
| 39. | The conversion factor shown below was obtained from the balanced chemical equation: 4 KO2(s) + 2 CO2(g) ® 2 K2CO3(s) + 3 O2(g). This conversion factor would be used to calculate which of the following?
|
|
| A) | The amount of KO2 required to react with a certain amount of O2 | |
| B) | The amount of O2 that can react with a certain amount of KO2 | |
| C) | The amount of O2 that can be produced from a certain amount of KO2 | |
| D) | The amount of KO2 that is required to produce a certain amount of O2 | |
| Ans: D Difficulty: Medium | ||
| 40. | Blimps are essentially very large helium filled balloons. If a blimp contains 536 kg of helium, how many helium atoms are present inside the blimp? | |||
| A) | 134,000 He atoms | C) | 8.9 x 10-19 He atoms | |
| B) | 8.06 x 1028 He atoms | D) | 3.23 x 1026 He atoms | |
| Ans: B Difficulty: Difficult | ||||
| 41. | Beaker A contains 1 mole of iron atoms, and Beaker B contains 1 mole of lead atoms. Which statement concerning these two samples is known with certainty?
|
|
| A) | Beakers A and B contain samples with the same molar mass. | |
| B) | Beakers A and B contain an equal number of atoms. | |
| C) | Beakers A and B contain an equal volume of atoms. | |
| D) | Beakers A and B contain equal masses of atoms. | |
| Ans: B Difficulty: Medium | ||
| 42. | A student runs the reaction: LiOH + CO2 ® LiHCO3. The reaction consumes 45.0 g LiOH and produces 72.8 g of LiHCO3. Which of the statements concerning this reaction is true? | |
| A) | The actual yield of the product is 72.8 g LiHCO3. | |
| B) | The theoretical yield of the product is 72.8 g LiHCO3. | |
| C) | The theoretical yield of the product is 117.8 g LiHCO3. | |
| D) | The percent yield of the reaction is 61.8%. | |
| Ans: A Difficulty: Easy | ||
| 43. | Assume that the mixture of substances in Figure 1 undergoes a chemical reaction. Which diagram represents a product mixture that is consistent with the Law of Conservation of Mass?
|
|
| A) | ||
| B) | ||
| C) | ||
| D) | It is impossible to predict based on the information given. | |
| Ans: A Difficulty: Medium | ||
| 44. | The subscripts in chemical formulas are changed in order to balance a chemical equation. |
| A) True B) False | |
| Ans: B Difficulty: Easy |
| 45. | A chemical equation is balanced by adding coefficients in front of some formulas so that the number of atoms of each element is equal on both sides of the equation. |
| A) True B) False | |
| Ans: A Difficulty: Easy |
| 46. | A mole of copper atoms has more atoms than a mole of lead atoms. |
| A) True B) False | |
| Ans: B Difficulty: Easy |
| 47. | One mole of oxygen molecules contains more atoms than one mole of lead atoms. |
| A) True B) False | |
| Ans: A Difficulty: Medium |
| 48. | The molar mass of CaCO3 is greater than the molar mass of Ca(NO3)2. |
| A) True B) False | |
| Ans: B Difficulty: Easy |
| 49. | The actual yield is the amount of product expected from a given amount of reactant based on the coefficients in the balanced chemical equation. |
| A) True B) False | |
| Ans: B Difficulty: Medium |
| 50. | In calculating the percent yield, both the actual yield and theoretical yield must be in units of grams. |
| A) True B) False | |
| Ans: B Difficulty: Medium |
| 51. | Oxidation is the gain of electrons by an atom. |
| A) True B) False | |
| Ans: B Difficulty: Easy |
| 52. | All chemical reactions convert one substance into another. |
| A) True B) False | |
| Ans: A Difficulty: Medium |
| 53. | In the reaction: Ni2+(aq) + Mg(s) ® Ni(s) + Mg2+(aq), the oxidizing agent is Ni2+(aq). |
| A) True B) False | |
| Ans: A Difficulty: Medium |
| 54. | In the reaction: Ni2+(aq) + Mg(s) ® Ni(s) + Mg2+(aq), the species that undergoes reduction is Mg(s). |
| A) True B) False | |
| Ans: B Difficulty: Medium |
| 55. | Combustion reactions are redox reactions. |
| A) True B) False | |
| Ans: A Difficulty: Medium |
| 56. | The balanced reaction: 4 NO2 + O2 + 2 H2O ® 4 HNO3 states that four moles of nitrogen dioxide react with each mole of oxygen. |
| A) True B) False | |
| Ans: A Difficulty: Easy |
| 57. | The balanced reaction: 4 NO2 + O2 + 2 H2O ® 4 HNO3 states that four grams of nitrogen dioxide reacts with each gram of oxygen. |
| A) True B) False | |
| Ans: B Difficulty: Easy |
| 58. | The balanced reaction: 4 Fe(s) + 3 O2(g) ® 2 Fe2O3(s) is an oxidation-reduction reaction. |
| A) True B) False | |
| Ans: A Difficulty: Medium |
| 59. | A mole is a quantity that contains 6.02 × 10–23 atoms, molecules, or ions. |
| A) True B) False | |
| Ans: B Difficulty: Easy |
| 60. | The formula weight of a compound is the sum of the atomic weights of all the atoms in a compound, reported in atomic mass units. |
| A) True B) False | |
| Ans: A Difficulty: Easy |
| 61. | When the mass of a substance produced in a reaction must be calculated, first its number of moles is determined using mole ratios, and then Avogadro’s number is used to convert moles to grams. |
| A) True B) False | |
| Ans: B Difficulty: Easy |
| 62. | The actual yield of a product in a chemical reaction should not exceed its theoretical yield. |
| A) True B) False | |
| Ans: A Difficulty: Easy |
| 63. | In redox reactions, metals tend to undergo oxidation. |
| A) True B) False | |
| Ans: A Difficulty: Medium |
| 64. | The electric current generated in batteries used for portable electronic devices and pacemakers results from redox reactions. |
| A) True B) False | |
| Ans: A Difficulty: Easy |
| 65. | The reaction: Mg(s) + 2 HBr(aq) ® MgBr2(s) + H2(g) is an oxidation-reduction reaction. |
| A) True B) False | |
| Ans: A Difficulty: Medium |
| 66. | Consider the balanced reaction: 4 NO2 + O2 + 2 H2O ® 4 HNO3. If 100. g of NO2 is placed in a reaction vessel the theoretical yield of nitric acid (HNO3) collected will be 137 g. |
| A) True B) False | |
| Ans: A Difficulty: Difficult |
| 67. | In a chemical reaction, the actual yield of a product may be reduced by side reactions. |
| A) True B) False | |
| Ans: A Difficulty: Easy |
| 68. | 2 Co(NO3)3(aq) + 3 (NH4)2S(aq) ® Co2S3(s) + 3 NH4NO3(aq) is a properly balanced chemical equation. |
| A) True B) False | |
| Ans: B Difficulty: Medium |
| 69. | To determine the overall percent yield in a synthesis that has more than one step, subtract the percent yield for each step from 100% yield. |
| A) True B) False | |
| Ans: B Difficulty: Medium |
| 70. | Consider the balanced reaction: 2 A + B ® C, where the molar mass of B is less than the molar mass of A. It requires a smaller mass of A to completely react with given mass of B. |
| A) True B) False | |
| Ans: B Difficulty: Difficult |
| 71. | In the reaction: Ni2+(aq) + Mg(s) ® Ni(s) + Mg2+(aq), two electrons are transferred from Ni2 to Mg. |
| A) True B) False | |
| Ans: B Difficulty: Medium |
| 72. | A 100-g sample of the compound below contains greater than one mole of molecules.
|
| A) True B) False | |
| Ans: A Difficulty: Medium |
| 73. | A 100-g sample of the compound below contains less than 6.02 × 1023 molecules.
|
| A) True B) False | |
| Ans: B Difficulty: Medium |
| 74. | One term in a balanced chemical equation contains the coefficient 4 in front of the formula Mg3(PO4)2. This term represents that there are 12 Mg atoms, 4 P atoms and 16 O atoms in this term. |
| A) True B) False | |
| Ans: B Difficulty: Medium |
| 75. | To multiply two numbers in scientific notation, multiply the coefficients together and multiply the exponents in the powers of 10. |
| A) True B) False | |
| Ans: B Difficulty: Medium |
| 76. | The molar mass of dibromomethane (CH2Br2) is larger than the molar mass of dichloromethane (CH2Cl2). |
| A) True B) False | |
| Ans: A Difficulty: Easy |
| 77. | A 200.-mg ibuprofen (C13H18O2) tablet contains greater than one mole of ibuprofen molecules. |
| A) True B) False | |
| Ans: B Difficulty: Medium |
| 78. | Consider the unbalanced chemical equation: NH3 + O2 ® NO + H2O. It requires 55.4 g of NH3 to completely react with 156 g of O2. |
| A) True B) False | |
| Ans: B Difficulty: Difficult |
| 79. | The mass of one ethanol (C2H6O) molecule is 7.65 × 10–23 grams. |
| A) True B) False | |
| Ans: A Difficulty: Medium |
| 80. | A chemical change alters the chemical composition of a substance, and therefore a new substance is produced. |
| A) True B) False | |
| Ans: A Difficulty: Easy |
| 81. | A chemical equation is an expression that uses chemical formulas and other symbols to illustrate what _____ constitute the starting materials in a reaction and what _____ are formed. | |
| Ans: | reactants, products | |
| Difficulty: Easy | ||
| 82. | When calculating the number of moles of calcium hydroxide formed from each mole of sodium hydroxide in the balanced reaction: CaCl2 + 2 NaOH ® Ca(OH)2 + 2 NaCl, the necessary conversion factor is _____. | |
| Ans: | ||
| Difficulty: Easy | ||
| 83. | A redox reaction involves the transfer of _____ from one element to another. | |
| Ans: | electrons | |
| Difficulty: Easy | ||
| 84. | A compound that gains electrons in a redox reaction while causing another compound to be oxidized is called a(n) _____ agent. | |
| Ans: | oxidizing | |
| Difficulty: Medium | ||
| 85. | _____ results in the loss of oxygen atoms or the gain of hydrogen atoms. | |
| Ans: | Reduction | |
| Difficulty: Medium | ||
| 86. | In a redox reaction, the _____ agent is the substance that gets oxidized. | |
| Ans: | reducing | |
| Difficulty: Medium | ||
| 87. | In a two-step synthesis where the first reaction has a 55% yield and the second reaction has a 24% yield, the overall percent yield of the reaction is _____% yield. | |
| Ans: | 13 | |
| Difficulty: Medium | ||
| 88. | In the balanced reaction: 2 I– + Cl2 ® 2 Cl– + I2, _____ is the reducing agent and _____ is the oxidizing agent. | |
| Ans: | I–, Cl2 | |
| Difficulty: Medium | ||
| 89. | Aluminum metal and oxygen gas are obtained when aluminum oxide is heated at high temperature. The reactant(s) in this chemical reaction is(are) _____. | |
| Ans: | aluminum oxide | |
| Difficulty: Easy | ||
| 90. | The combustion of hexane (C6H14), a component of gasoline, is represented by the balanced chemical equation: 2 C6H14(l) + 19 O2(g) ® 12 CO2(g) + 14 H2O(g). If 1.0 mole of hexane undergoes combustion, _____ moles of O2 are required. | |
| Ans: | 9.5 | |
| Difficulty: Medium | ||
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