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Study Resources (Chemistry)

Short Answer Questions 1) What does the term amphoteric mean? 2) What is the difference between a strong and weak acid? 3) What is the autoionization of water? 4) Do both protons ionize instantaneously from a diprotic acid such as H2CO3? Explain your answer. 5) Describe the relationship between molecular structure and acid strength. 6).
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Algorithmic Questions 1) A solution is prepared by dissolving 0.23 mol of hydrazoic acid and 0.27 mol of sodium azide in water sufficient to yield 1.00 L of solution.The addition of 0.05 mol of NaOH to this buffer solution causes the pH to increase slightly. The pH does not increase drastically.
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Matching Questions Match the following. A) equivalence point of a weak base-strong acid titration B) equivalence point of a weak acid-strong base titration C) three-quarters of the way to second equivalence point of a diprotic acid-strong base titration D) halfway to equivalence point of a weak acid-strong base titration E) equivalence point of a strong acid-strong.
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41) Identify the indicator that can be used at the lowest pH. A) alizarin B) thymol blue C) crystal violet D) phenolphthalein E) alizarin yellow R 42) Identify the indicator that has two endpoints. A) phenol red B) thymol blue C) crystal violet D) phenolphthalein E) alizarin yellow R 43) Identify the indicator that can be used at the highest pH. A) alizarin B).
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Algorithmic Questions 1) What is the reduction half-reaction for the following overall galvanic cell reaction? Co2+(aq) + 2Ag(s) → Co(s) + 2 Ag+(aq) A) Ag(s) + e- → Ag+(aq) B) Ag+(aq) + e- → Ag(s) C) Co2+(aq) + 2 e- → Co(s) D) Co2+(aq) + e- → Co(s) 2) What is the shorthand notation that represents the.
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  Multiple Choice Questions 1) Identify a good buffer. A) a solution containing small amounts of both a weak acid and its conjugate base B) a solution containing significant amounts of both a strong acid and a strong base C) a solution containing small amounts of both a strong acid and a strong base D) a.
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Matching Questions Match the following. A) E°cell < 0 B) Ecell < 0 C) E°cell > 0 D) Ecell > 0 E) Ecell = 0 F) Ecell = E°cell 1) Q = 1 Diff: 1     Type: MA     Var: 1     Page Ref: 18.6 2) Q > K Diff: 1     Type: MA     Var: 1     Page Ref: 18.6 3) Q < K Diff: 1     Type: MA    .
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Algorithmic Questions 1) When dissolved in water, which compound is generally considered to be an Arrhenius acid? A) CH3CO2H B) NaOH C) Na2CO3 D) CH3CH2OH 2) Which Bronsted-Lowry acid is not considered to be a strong acid in water? A) HBr B) HI C) H IO4 D) HNO3 3) Calculate the hydronium ion concentration in an aqueous solution.
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Matching Questions Match the following. A) proton donor B) electron pair acceptor C) proton acceptor D) electron pair donor E) produces protons in aqueous solution F) produces hydroxide ions in aqueous solution 1) Arrhenius acid Diff: 1     Type: MA     Var: 1     Page Ref: 15.3 2) Arrhenius base Diff: 1     Type: MA     Var: 1     Page Ref: 15.3 3) Bronsted-Lowry acid Diff: 1     Type: MA    .
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51) Given the following equation, N2O(g) + NO2(g) → 3NO(g)ΔrG° = -23.0 kJ mol-1 3N2O(g) + 3NO2(g) → 9NO(g) A) -23.0 kJ mol-1 B) 69.0 kJ mol-1 C) -69.0 kJ mol-1 D) -7.67 kJ mol-1 E) 23.0 kJ mol-1 52) Given the following equation, N2O(g) + NO2(g) → 3 NO(g)ΔrG° = -23.0 kJ mol-1 9NO(g) → 3N2O(g) + 3NO2(g) A).
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41) Calculate ΔrS° for the following reaction. The S? for each species is shown below the reaction. C2H2(g) + 2H2(g) → C2H6(g) S°(J K-1 mol-1)200.9130.7229.2 A) +303.3 J K-1 mol-1 B) +560.8 J K-1 mol-1 C) -102.4 J K-1 mol-1 D) -233.1 J K-1 mol-1 E) 229.2 J K-1 mol-1 42) Calculate ΔrS° for the following reaction. The.
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11) Consider the following reaction at constant pressure. Use the information here to determine the value of ΔSsurr at 355 K. Predict whether or not this reaction will be spontaneous at this temperature. 2NO(g) + O2(g) → 2NO2(g)ΔrH = -114 kJ A) ΔSsurr = +114 kJ K-1 mol-1, reaction is spontaneous B) ΔSsurr.
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  Multiple Choice Questions 1) Which of the following statements is TRUE? A) A spontaneous reaction is a reaction that takes place without any outside intervention. B) Thermodynamics is a study of reaction rates. C) A nonspontaneous reaction is a reaction that does not take place under any conditions. D) Chemical kinetics is a discipline that.
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61) Calculate ΔrG° at 298 K using the following information: 4HNO3(g) + 5N2H4(l) → 7N2(g) + 12H2O(l)ΔrG° = ? ΔfG° (kJ mol-1)-73.5149.3-237.1 A) -3.2977 × 103 kJ mol-1 B) -312.9 kJ mol-1 C) +2.845 × 103 kJ mol-1 D) +110.7 kJ mol-1 E) -954.7 kJ mol-1 62) Calculate ΔrG° at 298 K using the following information: 2HNO3(aq) +.
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41) Which of the following is the strongest oxidizing agent? A) H2O2(aq) B) Fe3+(aq) C) ClO2(g) D) I2(s) E) Fe(s) 42) Which of the following is the weakest oxidizing agent? A) H2O2(aq) B) Fe3+(aq) C) ClO2(g) D) I2(s) E) Fe(s) 43) Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in.
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31) What is undergoing reduction in the redox reaction represented by the following cell notation? Pb(s) ? Pb2+(aq) H+(aq) ? H2(g) ? Pt(s) A) H2(g) B) H+(aq) C) Pb2+(aq) D) Pb(s) E) Pt(s) 32) Which of the following is TRUE about standard electrode potentials? A) E°cell is negative for spontaneous reactions. B) Electrons will flow from a more.
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Matching Questions Match the following. A) K = 0 B) ΔrG > 0 C) ?rG < 0 D) ΔrG < ΔrG° E) equilibrium F) ΔrG > ΔrG° G) standard state 1) Q = K Diff: 1     Type: MA     Var: 1     Page Ref: 17.9 2) Q < K Diff: 1     Type: MA     Var: 1     Page Ref: 17.9 3) Q > K Diff: 1     Type: MA    .
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61) Use the provided reduction potentials to calculate ΔrG° for the following balanced redox reaction: Pb2+(aq) + Cu(s) → Pb(s) + Cu2+(aq) E°(Pb2+/Pb) = -0.13 V and E°(Cu2+/Cu) = +0.34 V A) -41 kJ mol-1 B) -0.47 kJ mol-1 C) +46 kJ mol-1 D) +91 kJ mol-1 E) -21 kJ mol-1 62) Use the provided reduction potentials.
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  Multiple Choice Questions 1) Which of the following statements is TRUE? A) A reduction process corresponds to an increase in oxidation state as a result of loss of electrons. B) An oxidation process involves the loss of electrons resulting in an increase in oxidation state. C) An oxidation process corresponds to a decrease in.
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51) Which of the following metals will dissolve in nitric acid but not hydrochloric acid? A) Fe; Eo(Fe2+/Fe) = -0.45V B) Pb; Eo(Pb2+/Pb)= -0.13V C) Cu; Eo(Cu2+/Cu) = +0.34V D) Sn; Eo(Sn2+/Sn) = -0.14V E) Ni; Eo(Ni2+/Ni) = -0.23V 52) Which of the following metals will dissolve in nitric acid but not hydrochloric acid? A) Cd;.
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11) Based on the following information, Cl2(g) + 2 e- → 2Cl-(aq)E° = +1.36 V Mg2+(aq) + 2 e- → 2Mg(s)E° = -2.37 V which of the following chemical species is the strongest reducing agent? A) Cl2(g) B) Mg2+(aq) C) Cl-(aq) D) Mg(s) 12) Using the following standard reduction potentials, Fe3+(aq) + e- →Fe2+(aq)E° = +0.77 V Ni2+(aq) +.
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Algorithmic Questions 1) Which one of the following would be expected to have the lowest standard molar entropy, S°, at 25 °C? A) C10H22(s) B) C10H22(l) C) C14H30(s) D) C14 H30OH(l) 2) The value of ΔfG° at 141.0 °C for the formation of phosphorus trichloride from its constituent elements, P2(g) + 3Cl2(g)  →  2PCl3(g) is __________ kJ.
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6) Define the second law of thermodynamics. 7) What is "free" energy? Give a fictitious example. 8) Give the standard states for a gas, liquid, solid, and solution. 9) Define the third law of thermodynamics. 10) Define allotrope. 11) How is a nonspontaneous process made spontaneous? 12) Why is the quantity of energy required to recharge.
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Short Answer Questions 1) Why is heating your home with gas more efficient than heating it with electricity? 2) Why can't we say that a spontaneous reaction is a fast reaction? 3) Why can endothermic reactions be spontaneous? 4) Define entropy. 5) How many microstates are possible in a collection of four particles that are.
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