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Study Resources (Chemistry)

31) 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. 32) A beaker contains 0.50 mol of potassium bromide in 600 mL of water.  An additional 600 mL of water is added.  The number.
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9.2   Algorithmic Questions 1) Which of the following solutions will have the highest concentration of chloride ions? A) 0.10 M NaCl B) 0.10 M MgCl2 C) 0.10 M AlCl3 D) 0.05 M CaCl2 E) All of these solutions have the same concentration of chloride ions. 2) How many milliliters of a 0.184 M RbNO3 solution contain 0.113.
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71) Identify NaCl. A) weak acid B) weak electrolyte C) strong acid D) strong electrolyte E) nonelectrolyte 72) Which one of the following compounds is insoluble in water? A) K2SO4 B) NaNO3 C) Pb SO4 D) Rb2CO3 73) Which one of the following compounds is soluble in water? A) Ca3(PO4)2 B) HgS C) Ni(NO3)2 D) MgCO3 74) Which pair of compounds is soluble in water?.
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11) Identify HCl. A) strong electrolyte, weak acid B) weak electrolyte, weak acid C) strong electrolyte, strong acid D) weak electrolyte, strong acid E) nonelectrolyte 12) Choose the statement below that is true. A) A weak acid solution consists of mostly nonionized acid molecules. B) The term "strong electrolyte" means that the substance is extremely reactive. C) A strong.
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61) Use the ΔH°f and ΔH°rxn information provided to calculate ΔH°f for SO3(g)  ΔH°f (kJ/mol)2 SO2(g) + O2(g) → 2 SO3(g)ΔH°rxn = -198 kJ SO2(g)-297 A) -792 kJ/mol B) -248 kJ/mol C) -495 kJ/mol D) -578 kJ/mol E) -396 kJ/mol 62) Use the information provided to determine ΔH°rxn for the following reaction   ΔH°f (kJ/mol)CH4(g) + 4 Cl2(g).
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9.4   Short Answer Questions 1) How would the concentration change if a 1.0 L flask of 1.0 M NaCl were left uncapped on a laboratory bench for several days.  Why? 2) Define an electrolyte. 3) Explain the difference between a strong and weak electrolyte.  Give an example of each. 4) Give the name for.
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81) The mixing of which pair of reactants will result in a precipitation reaction? A) Mg(NO3)2(aq) + Na2CO3(aq) B) K2SO4(aq) + Cu(NO3)2(aq) C) NaClO4(aq) + (NH4)2S(aq) D) NH4Br(aq) + NH4I(aq) 82) What reagent could be used to separate Br- from N O3- when added to an aqueous solution containing both? A) AgNO3(aq) B) Ba(OH)2(aq) C) CuSO4(aq) D).
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10.3  Matching Questions Match the following. A) energy flows out of system into the surroundings B) thermal energy C) kinetic energy D) chemical energy E) potential energy   1) energy associated with the motion of an object Diff: 1    Var: 1    Page Ref: 10.2 Global:  G1 2) energy associated with the temperature of an object Diff: 1    Var: 1    Page Ref: 10.2 Global: .
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91) Identify the spectator ions in the following molecular equation. KBr(aq) + AgNO3(aq) → AgBr(s) + KNO3(aq) A) Ag+ and Br- B) K+ and NO3- C) K+ and Br- D) Ag+ and NO3- E) There are no spectator ions in this reaction. 92) Identify the polyprotic acid. A) H2SO4 B) HCl C) LiI D) NaOH E) Ba(OH)2 93) How many H+ ions can.
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61) Determine the name for aqueous HBr. A) bromic acid B) bromous acid C) hydrobromous acid D) hydrogen bromate E) hydrobromic acid 62) Determine the name for HFO3. A) hydrofluoric acid B) hydrofluorus acid C) fluorate acid D) fluoric acid E) perfluoric acid 63) Which one of the following compounds behaves as an acid when dissolved in water? A) CaO B) C2H6 C) HF D).
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  10.1  Multiple Choice Questions 1) 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) energy associated with the position or composition of an object 2) Define.
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  9.1   Multiple Choice Questions 1) Determine the molarity of a solution formed by dissolving 97.7 g LiBr in enough water to yield 750.0 mL of solution.  A) 1.50 M B) 1.18 M C) 0.130 M D) 0.768 M E) 2.30 M 2) Determine the molarity of a solution formed by dissolving 468 mg of MgI2 in.
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31) Which of the following processes is endothermic? A) the freezing of water B) the combustion of butane C) a hot cup of coffee (system) cools on a countertop D) the chemical reaction in a "hot pack" often used to treat sore muscles E) the vaporization of rubbing alcohol 32) Which of the following processes is.
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  11.1  Multiple Choice Questions 1) An instrument used to measure atmospheric pressure is called a A) barometer. B) manometer. C) sphygmomanometer. D) spectrophotometer. E) spectrometer. 2) An instrument used to measure the pressure of a gas in a laboratory is called a A) barometer. B) manometer. C) sphygmomanometer. D) spectrophotometer. E) spectrometer. 3) An instrument used to measure blood pressure is called a A).
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10.4  Short Answer Questions 1) Describe the energy changes that occur when a book is held 6 ft off the floor and then dropped. 2) Define chemical energy. 3) Where does the energy absorbed during an endothermic reaction go?  4) Explain the difference between ΔH and DE. 5) Give the temperature and pressure for.
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51) Use the bond energies provided to estimate ΔH°rxn for the reaction below. 2 Br2(l) + C2H2(g) → C2H2Br4(l)ΔH°rxn = ? BondBond Energy (kJ/mol) Br-Br193 C≡C837 C-C347 C-Br276 C-H414 A) +407 kJ B) -324 kJ C) -228 kJ D) +573 kJ E) -648 kJ 52) Use the bond energies provided to estimate ΔH°rxn for the reaction below. CH3OH(l) + 2 O2(g) → CO2(g) +.
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51) Balance the chemical equation given below, and determine the number of milliliters of 0.00300 M phosphoric acid required to neutralize 40.00 mL of 0.00150 M calcium hydroxide. ________ Ca(OH)2(aq) + ________ H3PO4(aq) → ________ Ca3(PO4)2(aq) + ________ H2O(l) A) 2.70 mL B) 13.3 mL C) 20.0 mL D) 30.0 mL 52) According to the.
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8.3   Short Answer Questions 1) Describe the greenhouse effect. 2) Balance the following equation. ________ C10H12 + ________ O2 → ________ H2O + ________ CO2 3) Balance the following equation. ________ C9H20 + ________ O2 → ________ H2O + ________ CO2 4) If 588 grams of FeS2 is allowed to react with 352 grams of O2.
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