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89 Cards in this Set
- Front
- Back
the internal energy of a system increased by___. |
volume compression |
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When a system ___, delta E is always negative. |
absorbs heat and does work |
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___solids consist of atoms or molecules held together by dipole-dipole forces, London dispersion forces, and/or covalent network |
ionic |
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a real gas will behave most like an ideal gas under condition of_____. |
low temperature and high pressure |
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of the following, ___ is a valid statement of Charles' law: |
V= constantX P |
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the strongest inter particle attractions exist between particles of ___ and the weakest inter article attractions exist between particles of a ___. |
solid, gas |
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A gas is___ and assumes___ of its container whereas a liquid is ___ and assumes ___ of its container. |
condensed, the volume and shape, condensed, the volume and shape |
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the property responsible for the "beading up" of water is ____ |
hydrogen bonding |
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in which of the following molecules is hydrogen bonding most likely to e the most significant component of the total intermolecular forces? A) CH4 B) C6H13NH2 c) CO2 D) C5H11OH E) CH3OH |
C5H11OH |
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in general, the vapor pressure of a substance increases as _____ increases |
hydrogen bonding |
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crystalline solids differ from amorphous solids in that crystalline solids have_____ |
a long range repeating pattern of atoms, molecules, or ions. |
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Of the following substances only __ has London dispersion forces as its ONLY intermolecular force. A) NH3 B) CH3OH C) HCL D) CH4 E) H2S |
HCL |
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as a solid element melts, the atom become ___ and they have ____ attraction for one another. |
more separated, less |
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A solid has a very high melting point, great hardness, and poor electrical conduction. This is a(n) ___ solid. |
metallic and covalent network |
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Elemental iodine is a solid at room temperature. what is the major attractive force that exists among different iodine molecules in the solid? |
London dispersion forces |
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which one of the following exhibits dipole dipole attraction between molecules? A) AsH3 B) Cl2 C) CO2 D) BCl3 E) XeF4 |
XeF4 |
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metallic solids do not exhibit: |
excellent thermal conductivity |
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which statements about viscosity are true? (i) Viscosity increases as temperature decreases. (ii) Viscosity increases as molecular weight increases (iii) Viscosity increases as intermolecular forces increase. |
(ii) and (iii) |
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of the following which is the weakest acid? |
HIO2 |
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in the gas phase reaction, NH3 is acting as a(n) _____ base but not as a(n)____ base. |
Arrhenius, Lewis |
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of the following acids, ___ is not a strong acid: A) H2SO4 B) HCL C) HNO2 D) HCLO4 E) HNO3 |
HNO3 |
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which of the following is a bronsted-lowry acid: A) HF B) CH3COOH C) (CH3)3NH+ D) HNO2 E) all of the above |
HF |
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A Bronsted-lowry base is defined as a substance that ______ |
acts as a proton acceptor |
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which on of the following is the weakest acid: A) HNO2 (Ka= 4.5X10^-4) B) HClO (Ka=3.0X10^-8) C) HCN (Ka= 4.9X10^-10) D) HF (Ka= 6.8X10^-4) E) Acetic Acid (Ka= 1.8X10^-5) |
HNO2 (Ka= 4.5X10^-4) |
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Le Chateliers principle predicts that ___ will result in an increase in the number of moles of SO3(g) in the reaction container. |
decreasing the pressure |
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at equilibrium, ______. |
the value of the equilibrium constant is 1 |
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how is the reaction quotient used to determine whether a system is at equilibrium? |
at equilibrium, the reaction quotient is undefined. |
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which of the following aqueous solution has the highest [OH-] |
a solution with oH of 3.0 |
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le chateliers principle predicts that an increase in temperature will result in _____? |
no changes in equilibrium partial pressure. |
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In the arrhenius equation: K=Ae^-Ea/RT ______ is the frequency factor. |
K |
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of the following, all are valid units for a reaction rate except_____. A) mol/L-hr B) mol/hr C) M/s D)mol/L E) g/s |
A) mol/L-hr |
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_____ are used in automotive catalytic conveyers. |
homogeneous catalysts |
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A 25.0 mL sample of an unknown solution compound is titrated with a 0.115M NaOH solution. The titration curve above was obtained. The unknown compound is _____ |
strong acid |
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what change will be caused by addition of small amount of HCL to a solution containing fluoride ions and hydrogen fluoride ? |
the concentration of fluoride ions will increase as will the concentration of hydronium ions. |
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a catalyst can increase the rate of reaction _____. |
by increasing the overall activation energy (Ea) of the reaction |
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of the following, which is the strongest acid? A) HIO B) HIO4 C) HIO2 D) HIO3 E) the acid strength of all of the above is the same. |
HIO |
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a solution containing which one of the following pairs of substances will be a buffer solution? A) NaI, HI B) RbCl, HCL C) KBr, HBr D) CsF, HF E) None of the above |
E) none of the above |
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the mechanism for formation of the product X: A+B---> C+D (slow) B+D---> X (Fast) the intermediate reactant in the reaction is _____ |
D |
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as the temperature of a reaction is increased, the rate of the reaction increases because the ____. |
reactant molecules collide more frequently and with greater energy per collision. |
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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 reaction? |
increasing the temperature of the reaction |
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which of the following is true? |
since intermediate compounds can be formed, the chemical equations for the elementary reactions in a multistep mechanism do not always have to add to give the chemical equation of the overall process |
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in the energy profile of a reaction, the species that exists at the maximum on the curve is called the _____. |
enthalpy of reaction |
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which one of the following conditions would always result in an increase in the internal energy of a system? |
the system gains heat that has work done on it by the surroundings |
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of the following which is a state function? A) w B) H C) q D) heat E) none of the above |
B) H |
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A _____ delta H corresponds to an ___ process |
negative, exothermic |
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a chemical reaction that absorbs heat from the surroundings is said to be___ and has a ___ Delta H at constant pressure |
endothermic, positive |
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the units of heat capacity are ____ |
J/K or J/g-degree C |
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which of the following is a statement of Hess's Law |
if a reaction is carried out in a series of steps, the delta H for the reaction will equal the sum of the enthalpy changes for the individual steps |
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with references to enthalpy changes, the term standard conditions means____. A) P=1 atm B) some common temperatures, usually 298K C) V=1L A) a only B) b only C) c only D) a&c E) a&b |
E) a&b |
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which of the following statements about gases is false? |
all gases are colorless and odorless at room temperature |
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one significant difference between gases and liquids is that______ |
a gas assumes the volume of its container |
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which of the following equations shows an incorrect relationship between pressures given in terms or different units? A) 0.760 atm = 578 mmHg B) 1.0 torr = 2.00 mmHg C)1.00 atm= 760 torr D) 1.20 atm = 122 kPa E) 152 mmHg = 2.03X10^4 Pa |
1.0torr=2.00mmHg |
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of the following, only ____ is impossible for an ideal gas. A) V1/V2= T1/T2=0 B) V1/T1=V2/T2 C) V1/V2=T1/T2 D) V2=(T2/T1)V1 E) V1T1=V2T2 |
E) V1T1=V2T2
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the average kinetic energy of the particles of a gas is directly Proportional to ______. |
the square of the rms speed |
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the kinetic molecular theory predicts that pressure rises as the temperature of gas increases because______. |
both the gas molecules collide more frequently with the wall and the gas molecules collide more energetically with the wall |
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Arrange the following gases in order of increasing average molecular speed at 25 C He, O2, CO2, N2 |
CO2 |
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a real gas will behave most like an ideal gas under conditions of ______. |
high temperature and low pressure. |
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hydration is a specific example of the phenomenon known generally as ____ |
solcation |
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the dissolution of gases in water is virtually always exothermic because_____ |
ine of the two endothermic steps ( separation of solute particles) in the solution- formation process in unnecessary |
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the phrase " like dissolves like" refers o the fact that _____ |
polar solvents dissolve polar solutes and non-polar solvents dissolve non-polar solutes |
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a saturated solution ______. |
contains dissolved solute n equilibrium with undissolved solute. |
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in a saturated solution of a salt in water, ______. |
the rate of crystallization = the rate of dissolution |
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the principle reason for the extremely low solubility of NaCl in benzene is the ____ |
weak salvation of Na+ and Cl- by C6H6 |
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which one of the following substances would be the most soluble in CCl4? A) H2O B) Ch3Ch2OH C) NaCl D) C10H22 E) NH3 |
C10H22 |
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which of the following substances is more likely to dissolve in water? |
HOCH2CH2OH |
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which on of the following substances is more likely to dissolve in benzene (C6H6) A) CH3CH2OH B) CCl4 C) NH3 D) HBr E) NaCl |
B) CCl |
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which on of the following is most soluble in hexane (C6H14) A) CH3CH2OH B) CH3CH2CH2CH2OH C) CH3CH2CH2CH2CH2OH D) CH3OH E) CH3CH2CH2OH |
C) CH3CH2CH2CH2CH2OH
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which of the following statements is false? |
the weaker the attraction between molecules the solute and solvent molecules, the greater the solubility. |
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calculate the molarity of a 17.5%(by mass) aqueous solution of nitric acid. |
the density of the solution is needed to solve the problem |
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a solution contains 15 ppm of benzene. the density of the solution is 1.00g/ml. this means that ______. |
there are 15mg of benzene in a 1.0L of this solution |
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A 0.1oom solution of which one of the following solutes will have the lowest vapor pressure. |
Al(ClO4)3 |
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a 1.35m aq solution of compound X had a boiling point of 101.4 C. which on elf the following could be compound X? the boiling point elevation constant for water is 0.52C/m. |
KCL |
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the ideal value of i (cant hoff factor) for (NH4)3PO4. |
4 |
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which of the following cannot be a colloid |
homogenous mixture |
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WHICH ONE OF THE FOLLOWING SUBSTANCES WOULD BE THE MOST SOLUBLE IN CCl4 |
C10H22 |
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a reaction that is spontaneous as written_____. |
will proceed without outside intervention |
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which one of the following is always positive when a spontaneous process occurs? |
delta S universe |
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Formation of solutions where the process is endothermic can be spontaneous provided that ______> |
they are accompanied by an increase in disorder |
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Consider pure crystalline solid that is heated from absolute zero to a temperature above the boiling point of the liquid. which of the allowing processes produces the greatest increase in the entropy of the substance?
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vaporizing the liquid |
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a0.100m solution of which of the following solutes will have the highest vapor pressure? |
sucrose |
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which of the following choices has the compounds correctly arranged in order of increasing solubility in water? (least to most soluble ) |
CCl4< CHCl3<NaNO3 |
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of the following in a 0.1M aq solution of ____ will have the lowest freezing point. |
AL(NO3)3 |
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which of the following statements is true? |
spontaneity can depend on the temperatures |
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which of the following usbtances is more likely to dissolve in benzene (C6H6) A) CH3Ch2OH B) NH3 C) NaCl D) HBr E) CCl4 |
E) CCl4 |
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delta S is positive for the reaction _____. A) BaF2(s)---> Ba2+(aq) +2F-(aq) B) 2NO2(g)--->N2O3(g) C) 2H2(g)+ O2(g)--> 2H20(g) |
A) BaF2(s)---> Ba2+(aq) +2F-(aq)
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the largest value of henrys constant for the liquid solvent H2O will be obtained with ____ gas as the solute and a temperature of _____ degree C. |
HCL, 49 |
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Calculate the molarity of a 25.4 %(by mass) aq solution of phosphoric acid (H3PO4). |
the density of this solution is needed to solve the problem. |
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the principle reason for the extremely low solubility of NaCL in benzene (C6H6) is the ____. |
weak salvation of NA+ and CL- by C6H6 |
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in a saturated solution of a salt in water, _____. |
the rate of crystallization = the rate of dissolution. |