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54 Cards in this Set
- Front
- Back
In a solution, when the conentrations of a weak acid and its conjugate base are equal,
A.) the -log of the [H+] and the -log of the Ka are equal B.) the buffering capacity is significantly decreased C.) the system is not at equilibrium D.) all of the above are true |
A.) the -log of the [H+] and the -log of the Ka are equal
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The addition of hydrofluoric acid and __________ to water producers a buffer solution.
A.) HCl B.) NaBr C.) NaNO3 D.) NaF E.) NaCl |
D.) NaF
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In which of the following aqueous solutions would you expect AgBr to have the highest solubility?
A.) 0.10M AgNO3 B.) 0.20M NaBr C.) pure water D.) 0.15M KBr E.) 0.10M LiBr |
C.) pure water
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A reaction that is spontaneous as written _______
A.) will proceed without outside intervention B.) is very slow C.) has an equilibrium position that lies far to the left D.) is also spontaneous in the reverse direction E.) is very rapid |
A.) will proceed without outside intervention
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The Henderson-Hasselbalch equation is _________:
A.) pH=pKa - log [base]/[acid] B.) pH = pKa + log [acid]/[base] C.) pH = log [acid]/[base] D.) pH = pKa + log [base]/[acid] E.) [H+] = Ka + [base]/[acid] |
D.) pH = pKa + log [base]/[acid]
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The first law of thermodynamics can be given as __________.
A.) deltaE = q+w B.) the entropy of a pure crystalline substance at absolute zero is zero C.) forany spontaneous process, the entropy of the universe increases D.) deltaHrxn = ndeltaHf(products)-mdeltaHf(reactants) E.) deltaS = qrev/T at constant temperature |
A.) deltaE = q+w
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_______ is the oxidizing agen in the reaction below.
Cr2O7(2-) + 6S2O3(2-) +14H(+) --> 2Cr(3+) + 3S4O6(2-) + 7H2O A.) S2O3 (2-) B.) Cr(3+) C.) Cr2O7(2-) D.) S4O6(2-) |
C.) Cr2O7(2-)
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when a system is at equilibrium, ___________
A.) the reverse process is spontaneous but the forward process is not B.) the forward process is spontaneous but the reverse process is not C.) both forward and reverse processes have stopped D.) the forward and reverse processes are both spontaneous E.) the process is not spontaneous in either direction |
E.) the process is not spontaneous in either direction
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The thermodynamic quantity that expresses the degree of disorder in a system is _________.
A.) entropy B.) enthalpy C.) heat flow D.) internal energy E.) bond energy |
A.) entropy
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The gain of electrons by an element is called ________.
A.) fractionation B.) reduction C.) sublimation D.) oxidation E.) disproportionation |
B.) reduction
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The entropy of the universe is ________.
A.) zero B.) the same as the energy, E C.) continually decreasing D.) constant E.) continually increasing |
E.) continually increasing
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The second law of thermodynamics states that ________.
A.) deltaE = q+w B.) deltaS = qrev/T at constant temperature C.) the entropy of a pure crystalline substance at absolute zero is zero D.) deltaHrxn = ndeltaHf(products)-mdeltaHf(reactants) E.) for any spontaneous process, the entropy of the universe increases |
E.) for any spontaneous process, the entropy of the universe increases
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What is the oxidation number of bromine in the BrO3 (-) ion?
A.) +1 B.) +7 C.) +5 D.) +3 E.) -1 |
C.) +5
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In a voltaic cell, electrons flow from the _____ to the _______.
A.) salt bridge, anode B.) anode, cathode C.) cathode, anode D.) salt bridge, cathode E.) anode, salt bridge |
B.) anode, cathode
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1V = _______.
A.) 1 J/s B.) 96485 C C.) 1 J/C D.) 1 amp*s E.) 1 C/J |
C.) 1 J/C
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The relationship between the change in Gibbs free energy and the emf of an electrochemical cell is given by ______.
A.) delta G = -E/nF B.) delta G = -nF/E C.) delta G = -nFE D.) delta G = -nF/ERT E.) delta G = -nRTF |
C.) delta G = -nFE
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Delta S is positive for the reaction _______.
A.) CO2 (g) --> CO2 (s) B.) BaF2 (s) --> Ba (2+) (aq) + 2F(-) (aq) C.) 2Hg (l) + O2 (g) --> 2HgO (s) D.) 2NO2 (g) --> N2O4 (g) E.) 2H2 (g) + O2 (g) --> 2H2O (g) |
B.) BaF2 (s) --> Ba (2+) (aq) + 2F(-) (aq)
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One of the differences between a voltaic cell and an electrolytic cell is that an electrolytic cell ____.
A.) a nonspontaneous reaction is forced to occur B.) oxidation occurs at the cathode C.) electrons flow toward the anode D.) an electric current is produced by a chemical reaction E.) O2 gas is produced at the cathode |
A.) a nonspontaneous reaction is forced to occur
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Which one of the following processes produces a decrease in the entropy of the system?
A.) boiling water to form steam B.) melting ice to form water C.) freezing water to form ice D.) dissolution of solid KCl in water E.) mixing of two gases into one container |
C.) freezing water to form ice
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Which one of the following correctly indicates the relationsihip between the entropy of a system and the number of different arrangements, W, in the system?
A.) S = kW B.) S = k/W C.) S = k lnW D.) S = Wk E.) S = W/k |
C.) S = k lnW
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The purpose of the salt bridge in an electrochemical cell is to ______.
A.) maintain electrical neutrality in the half-cells via migration of ions. B.) provide a means for electrons to travel from the cathode to the anode C.) provide a means for electrons to travel from the anode to the cathode D.) provide a source of ions to react at the anode and cathode E.) provide oxygen to facilitate oxidation at the anode |
A.) maintain electrical neutrality in the half-cells via migration of ions
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In the formula delta G = -nFE, F is the ______.
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Faraday constant
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In general, the solubility of a slightly soluble salt is ________ by the presence of a second solute that furnishes a common ion.
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decreased
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Processes that are spontaneous in one direction are nonspontaneous in the _______ direction.
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reverse
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Entropy _____ as the number of microstates in the system increases.
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increases
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The most difficult a species is to reduce and the poorer an ________ agent is it.
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oxidizing
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The phrase "like dissolves like" refers to the fact that ____.
A.) solvents can only dissolve solutes of similar molar mass B.) polar solvents dissolve polar solutes and nonpolar solvents dissolve nonpolar solutes C.) condensed phases can only dissolve other condensed phases D.) polar solvents dissolved nonpolar solutes and vice versa E.) gases can only dissolve other gases |
B.) polar solvents dissolve polar solutes and nonpolar solvents dissolve nonpolar solutes
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A solution with a concentration higher than the solubility is ______.
A.) is unsaturated B.) is not possible C.) is supercritical D.) is saturated E.) is supersaturated |
E.) is supersaturated
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Molality is defined as the _____.
A.) moles solute/Liters solution B.) moles solute/ moles solvent C.) moles solute/ kg solvent D.) moles solute/ kg solution E.) none (dimensionless) |
C.) moles solute/kg solvent
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The process of solute particles being surrounded by solvent particles is known as ______.
A.) salutation B.) solvation C.) agglomeration D.) dehydration E.) agglutination |
B.) solvation
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Formation of solutions where the process is endothermic can be spontaneous provided that ______.
A.) they are accompanied by another process that is exothermic B.) the solvent is a gas and the solute is a solid C.) they are accompanied by an increase in order D.) the solvent is water and the solute is a gas E.) they are accompanied by an increase in disorder |
E.) they are accompanied by an increase in disorder
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The rate law for a reaction is:
rate = k[A][B]2 Which one of the following statements is false? A.) the reaction is second order overall B.) k is the reaction rate constant C.) if [B] is doubled, the reaction rate will increase by a factor of 4 D.) the reaction is first order in A E.) the reaction is second order in B |
A.) the reaction is second order overall
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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 the reaction? A.) increasing the concentration of reactant A B.) increasing the temperature of the reaction C.) adding a catalyst for the reaction D.) increasing the concentration of reactant B E.) all of these will increase the rate |
D.) increasing the concentration of reactant B
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The mechanism for formation of the product X is:
A+B --> C + D (slow) B + D --> X (fast) The intermediate reactant in the reaction is _______. A.) A B.) B C.) C D.) D E.) X |
D.) D
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At equilibrium, ___________.
A.) the rates of the forward and reverse reactions are equal B.) the rate constants of the forward and reverse reactions are equal C.) all chemical reactions have ceased D.) the value of the equilibrium constant is 1 E.) the limiting reagent has been consumed |
A.) the rates of the forward and reverse reactions are equal
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Which of the following expressions is the corect equilibrium-constant expression for the equilibrium between dinitrogen tetroxide and nitrogen dioxide?
N2O4 (g) --> 2NO2 (g) A.) [NO2]2/[N2O4] B.) [NO2]/[N2O4] C.) [NO2]2[N2O4] D.) [NO2]/[N2O4] E.) [NO2]/[N2O4] |
A.) [NO2]2/[N2O4]
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The equilibrium constant for the gas phase reaction
N2 (g) + 3H2 (g) <--> 2NH3 (g) is Keq = 4.34*10^-3 at 300 degrees Celsius. At equilibrium, _____. A.) only products are present B.) products predominate C.) reactants predominate D.) roughly equal amounts of products and reactants are present E.) only reactants are present |
C.) reactants predominate
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The equlibrium constant for the gas phase reaction
2NH3 (g) <--> N2 (g) + 3H2 (g) is Keq = 230 at 300 degrees Celsius. At equilibrium, _____. A.) only products are present B.) reactants predominate C.) products predominate D.) roughly equal amounts of products and reactants are present E.) only reactants are present |
C.) products predominate
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The reaction below is exothermic:
2SO2 (g) + O2 (g) <--> 2SO3 (g) Le Chatelier's Principle predicts that _____ will result in an increase in the number of moles of SO3 (g) in the reaction container. A.) increasing the volume of the container B.) increasing the pressure C.) removing some oxygen D.) decreasing the pressure E.) increasing the temperature |
B.) increasing the pressure
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The conjugate acid of HSO4 (-) is _____.
A.) HSO4 (+) B.) SO4 (2-) C.) H (+) D.) HSO3 (+) E.) H2SO4 |
E.) H2SO4
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According to the Arrhenius concept, an acid is a substance that _____.
A.) tastes bitter B.) reacts with the solvent to form the cation formed by autoionization of that solvent C.) causes an increase in the concentration of H+ in aqueous solutions D.) fan accept a pair of electrons to form a coordinate covalent bond E.) is capable of donating one or more H+ |
C.) causes an increase in the concentration of H+ in aqueous solutions
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A Bronsted-Lowry base is defined as a substance that _____.
A.) acts as a proton acceptor B.) increases [H+] when placed in H2O C.) decreases [H+] when placed in H2O D.) increases [OH-] when placed in H2O E.) acts as a proton donor |
A.) acts as a proton acceptor
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A Bronsted-Lowry acid is defined as a substance that ____.
A.) acts as a proton donor B.) decreases [H+] when placed in H2O C.) increases Ka when placed in H2O D.) acts as a proton acceptor E.) increases [OH-] when placed in H2O |
A.) acts as a proton donor
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A substance that is capable of acting as both an acid and as a base is _____.
A.) conjugated B.) miscible C.) amphoteric D.) saturated E.) autosomal |
C.) amphoteric
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Which solution below has the highest concentration of hydroxide ions?
A.) pH = 3.21 B.) pH = 12.6 C.) pH = 7.00 D.) pH = 7.93 E.) pH = 9.82 |
B.) pH = 12.6
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An aqueous soltuion contains 0.10M NaOH. The solution is _____.
A.) basic B.) very dilute C.) acidic D.) neutral E.) highly colored |
A.) basic
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Nitric acid is a strong acid. This means that _____.
A.) aqueous solutions of HNO3 contain equal concentrations of H+ (aq) and OH- (aq) B.) HNO3 cannot be neutralized by a weak base C.) HNO3 dissociates completely to H+ (aq) and NO3- (aq) when it dissolves in water D.) HNO3 produces a gaseous product when it is neutralized E.) HNO3 does not dissociate at all when it is dissolved in water |
C.) HNO3 dissociates completely to H+ (aq) and NO3- (aq) when it dissolves in water
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Of the following, ___ is a weak acid.
A.) HF B.) HClO4 C.) HCl D.) HBr E.) HNO3 |
A.) HF
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The pH is defined as ________.
A.) -log[OH-] B.) -log[Ka] C.) -log[Kb] D.) -log[H+] |
D.) -log[H+]
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Physical properties of a solution that depend on the quantity of the solute particles present, but not the kind or identity of the particles, are termed ____ properties.
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colligative
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If a rate law is second order (reactant), doubling the reactant _____ the reaction rate.
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quadrupling
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The minimum energy to initiate a chemical reaction is the _______.
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activation energy
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Pure _____ and pure _____ are excluded from equilibrium-constant expressions.
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solids
liquids |
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If the value for the equilibrium constant is much greater than 1, then the equilibrium mixture contains mostly _____.
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products
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