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1) One significant difference between gases and liquids is that . A) a gas is made up of molecules B) a gas expands to fill its container C) a gas may consist of both elements and compounds D) gases are always mixtures E) All of the above answers are correct. 2) Molality is defined as the . A) moles solute/kg solvent B) moles solute/moles solvent C) moles solute/liters solution D) moles solute/kg solution E) none (dimensionless) 3) A supersaturated solution . A) is one with more than one solute B) is one that has been heated C) is one with a higher concentration than the solubility D) must be in contact with undissolved solid ) exists only in theory and cannot actually be prepared Of the following, will lower the activation energy for a reaction. raising the temperature of the reaction adding a catalyst for the reaction increasing the concentrations of reactants removing products as the recation proceeds pereasing the pressure is . Which one of the following is a valid statement of Avogadro's law? A PTM constant B) constant * P C) F- constant - n D) 17 - constant E) PF - constant 6) A reaction was found to be second order in carbon monoxide concentration The rate of the reaction if the (CO) is doubled, with everything else kept the same. A) is reduced by a factor of 2 B) remains unchanged C) increases by a factor of 4 D) doubles E) triples 7) Which statement is true about liquids but not true about solids? A) They flow and are not compressible. B) They are highly ordered and not compressible. C) They assume both the volume and the shape of their containers. D) They flow and are highly ordered E) They flow and are compressible. 8) What is the conjugate acid of NH3? A) NH3 B) NH2* C) NH3+ D) NH4+ E) NH4OH 9) In which one of the following solutions is silver chloride the most soluble? A) 0.181 M HCI B) 0.0176 M NH3 C) 0.744 M LiNO3 D) pure water E) 0.181 M NaCl 10) A BrØnsted-Lowry acid is defined as a substance that . A) increases Ka when placed in H2O B) decreases [H+] when placed in H2O C) increases [OH"] when placed in H2O D) acts as a proton acceptor E) acts as a proton donor between dinitrogen tetroxide and nitrogen dioxide? 11) Which of the following expressions is the correct équilibrium-constant expression for the equilibrium N2O4(g) 2NO2 (g) (NO2] A) [N2O4] (NO2R B) (N2O41 [NO2] C) [N2O4)² D) (NO2][N2O4] E) (NO212'N2041 12) Of the acids in the table below, is the strongest acid. Acid Ka HOAc 1.8 x 10-5 HCHO2 1.8 x 10-4 HCIO 3.0 x 10-8 HF 6.8 x 10-4 A) HOAc B) HCHO2 C) HCIO D) HF E) HOAc and HCHO2 13) A sample of a gas originally at 25 °C and 1.00 atm pressure in a 2.5 L container is subject to a pressure e 0.85 atm and a temperature of 15 °C. The final volume of the gas is L. A) 3.0 B) 2.8 C)2.6 D)2.1 E) 0.38 14) Of the following, is a valid statement of Charles' law. A) f T P = constant B) T V = constant C) PV = constant D) V = constant n E) V = constant P the is 1.05 g/mL. The concentration of Cl (chloride ions) in this solution is 15) A solution is prepared by dissolving 23.7 g of CaCh in 375 g of water. The density of the resulting solution A) 0.214 M. B) 6.64 x 10° C) 0.562 D) 1.12 E) 1.20 16) Which one of the following substances is more likely to dissolve in benzene (C6H6)? A) CH3CH2OH B) NH3 C) NaCI D) CCI4 E) HBr 17) In the gas phase reaction below, NH3 is acting as a(n) base but not as a(n) base. H lo H H H N H H* H H A) Arrhenius, BrØnsted-Lowry B) BrØnsted-Lowry, Lewis C) Lewis, Arrhenius D) Lewis, BrØnsted-Lowry E) Arrhenius, Lewis 18) The addition of hydrofluoric acid and to water produces a buffer solution. A) NaCl B) NaOH C) NaBr D) HCl E) NaNO3 19) An ideal gas differs from a real gas in that the molecules of an ideal gas . A) have no attraction for one another B) have a molecular weight of zero C) have appreciable molecular volumes D) have an average molecular mass E) have no kinetic energy 20). An alloy is a A) heterogeneous mixture of two metals. B) mineral containing two or more metals. C) nonmetal with some properties of a metal. D) pure metal. E) metallic material that is composed of two or more elements. the the DE 21) total In intermolecular which of the following forces? molecules is hydrogen bonding likely to be the most significant component of the A) CH4 B) CO2 C) CH;OH D) CsHnoH E) C6H13NH2 22) The rate law of the overall reaction A + B C is rate = K(A)2. Which of the following will not increase the rate of the reaction? A) increasing the concentration of reactant A B) increasing the concentration of reactant B C) increasing the temperature of the reaction D) adding a catalyst for the reaction E) All of these will increase the rate. 23) Acetic acid is a weak acid that dissociates into the acetate ion and a proton in aqueous solution: CH3COOH (aq) CH3COO (aq)+H* (aq) At equilibrium at 25 °C a 0.100 M solution of acetic acid has the following concentrations: M. [CH3COOH] = 0.0990 M, [CH3COO]] = 1.33 x 10-3 M, and [H*] = 1.33 x 10-3 The equilibrium constant, Keq, for the ionization of acetic acid at 25°C is . A) 1.75 x 10-7 B) 5.71 x 106 C) 5.71 x 104 D) 0.100 E) 1.79 X 10-5 Calculate the pH of a solution that is 0.322 M in nitrous acid is 4.50 (HNO2) x 10-4. and 0.178 M in potassium nitrite 24) (KNO2). The acid dissociation constant of nitrous acid A) 14.26 B) 3.093 C) 10.91 D) 4.589 E) 3.607 25) The Henderson-Hasselbalch equation is . [base] A) [H+] = Ka + [acid] B) pH=pKa-log = - [base] [acid] [base] C) pH = pKa + log [acid] [acid] D) pH = pKa + log [base] [acid] E) pH = log [base] product BaF2 is 1.7 x 10-6, g6) The concentration constant of of fluoride ions in a saturated solution of barium fluoride is A) 3.8 x 10-4 M. The solubility B) 3.0 x 10-3 C) 1.5 * 10-2 D) 7.5 x 10-3 E) 1.4 x 10-4 27) The data are as the reaction proceeds: reaction obtained A (aq) B (aq) is first order in [A]. A solution is prepared with [A] = 1.22 M. The following Time (s) 0.0 6.0 12.0 18.0 (A) (M) 1.22 0.61 0.31 0.15 The rate constant for this reaction is s-1. A) 0.23 B) 1.0 C) 0.17 D) 0.12 E) -0.12 28) Of the following equilibria, only will shift to the left, based on Le Châtelier's principle in response to a decrease in volume. A) H2 (g) + C12 (g) 2 HCI (g) B) 2 SO3 (g) 2 SO2 (g) + O2 (g) C) N2 (g) + 3H2 (g) 2 NH3 (g) D) 4 Fe (s) + 3 02 (g) 2 Fe2O3 (s) E) 2HI (g) H2 (g) + I2 (g) 29) Calculate the molarity of hydroxide ion in an aqueous solution that has a pOH of 3.00. A) 3.0 x 10-14 B) 1.1 x 10-13 C) 1.0 x 10-3 D) 1.0 x 10-11 E) 11.00 30) A result of the common-ion effect is in solubility ed Na+ (aq), frequently appear in solutions but do not participate that some ions, such as B) A) that common ions, such as Na+ (aq), don't affect equilibrium is constants promoted selective precipitation of a metal ion, such as Ag+, by the addition of an approp counterion C) that the (X-) that produces a compound (AgX) with that a very their low values solubility in so equilibrium constant expres D) that ions such as K+ and Na+ are common ions, always 1.00 E) that common ions precipitate all counter-ions 12.0 pH of 10.0 solution 80 in flask 6,0 Equivalence 4.0 Point 2.0 5 10 15 20 25 30 35 40 45 mL of 0 115 M NaOH added to flask A) titration 31) a A 25.0 curve mL sample above was of a obtained. solution of The an unknown unknown compound compound is is titrated with a 0.1151 M NaOH solution. The strong acid B) a strong base C) a weak acid D) a weak base E) neither an acid nor a base 32) Consider the following reaction at equilibrium. 2CO2 (g) 2CO (g) + O2(g) AH° = -514 k] Le Châtelier's principle predicts that the equilibrium partial pressure of CO (g) can be maximized by carrying out the reaction . A) at high temperature and high pressure B) at high temperature and low pressure C) at low temperature and low pressure D) at low temperature and high pressure E) in the presence of solid carbon 33) A solution containing which one of the following pairs of substances will be a buffer solution? A) Nal, HI B) KBr, HBr C) CsF, HF D) RbCl, HCI E) none of the above 34) The solubility of lead (II) chloride (PbCl2) is 1.6 x 10-2 M. What is the Ksp of PbC12? A) 5.0 x 10-4 B) 4.1 x 10-6 C) 3.1 x 10-7 D) 1.6 x 10-5 E) 1.6 x 10-2

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