Chemistry 1202 Final
accepts electrons
A lewis acid _________
the equilibrium shifts away from heat
According to Le Chatelier's principle __________
ethyl alcohol (alcoholic drinks)
Animals will lick up ethylene glycol (antifreeze) due to its sweet taste. The antidote for ethylene glycol poisoning is the administration of ________________.
sublimes
At atmospheric pressure, dry ice
enzymes
Biological catalysts that increase the rates of biochemical reactions are known as
Q=Ksp
Give the equation for a saturated solution in comparing Q with Ksp
[Ba2+][F-]2
Give the expression for the solubility product constant for BaF2
[Pb2+][Cl-]2
Give the expression for the solubility product constant for PbCl2
reversible
Give the name of the reaction that achieves the theoretical limits with respect to free energy in thermodynamics.
irreversible
Give the name of the reaction that does not achieve the theoretical limits with respect to free energy in thermodynamics.
molality
Give the term for the amount of solute in moles per kilogram of solvent.
molarity
Give the term for the amount of solute in moles per liter of solution.
CH3COOH (acetic acid)
Identify the acid that is in vinegar
lead-acid storage battery
Identify the battery that is in most automobiles.
dry-cell battery
Identify the battery that is used as a common flashlight battery.
indefinite shape and volume
Identify the characteristics of a gas.
indefinite shape, but definite volume
Identify the characteristics of a liquid.
All of them are correct
Identify the colligative property. A) vapor pressure lowering B) freezing point depression C) boiling point elevation D) osmotic pressure E) all of the above
hydrogen-oxygen
Identify the components of a fuel cell.
(CH3)3N
Identify the compound that does not have hydrogen bonding.
First
The __________ Law of thermodynamics states the energy is conserved in chemical processes.
dipole-dipole forces
The forces between polar molecules is known as
critical point
The set of conditions at which point a phase boundary no longer exists is know as the
the weaker the conjugate base
The stronger the acid, then which of the following is true?
zinc
To prevent rusting, nails are coated with ________
ln[reactant] vs. time
What data should be plotted to show that experimental concentration data fits a first-order reaction?
1/[reactant] vs. time
What data should be plotted to show that experimental concentration data fits a second-order reaction?
ΔG°rxn is zero and the reaction is at equilibrium.
What is TRUE if ln K is 1?
BCl3
Which of the following is a Lewis acid?
H2O
Which of the following is a Lewis base?
HI
Which of the following is a strong acid?
HCN (weak acid)
Which of the following is a weak acid?
H2SO4
Which of the following is an Arrhenius acid?
KOH
Which of the following is an Arrhenius base?
a buffer resists PH change by neutralizing added acids and bases.
Which of the following is true regarding a buffer?
hydrocyanic acid, Ka = 4.0 x 10^-10
Which of the following weak acids has the strongest conjugate base? (high Ka=weak)
AlF6^-
Which of the following would be considered a complex ion?
H2SO3
Which of these is an example of a polypro tic oxyacid?
Bronsted-lowry
based on reactions in water (aq) Common definition of acids as proton donors and bases as proton acceptors.
the phase transition from solid to gas
define sublimation
10^6
parts per million requires a multiplication factor of
A voltaic cell is an electrochemical cell that uses a chemical reaction to produce electrical energy.
what is a voltaic cell?
NH(CH3)2
which of the following is a weak base?
M-1 s-1
A graph of 1/[A] vs. t gives a straight line. What are the units of k for this system?
donates electrons
A lewis base __________
Lewis base
A ligand is a molecule or ion that acts as a _______
∆Suniverse
According to the Second Law of Thermodynamics, in order for a reaction to be spontaneous which value must increase?
Cl-
All of the following anions are considered basic except _________
a reaction speeding up upon the addition of a catalyst
All of the following are examples of a spontaneous process except ___________
dry cell batteries
All of the following are examples of rechargeable batteries EXCEPT
Na+
All of the following cations are considered acidic except ________
NH3 (aq)+ H20 (l) ----> NH4+ (aq) + OH - (aq)
An aqueous solution of ammonia is found to be basic. This observation can be explained by the net ionic equation ________________
carbonic acid and bicarbonate ion
An important buffer in the blood is a mixture of ______________
opposing reactions attaining equal rates
Chemical equilibrium is the result of
ΔGrxn = 0 at equilibrium.
Choose the statement below that is true regarding deltaGrxn.
This reaction will be spontaneous at all temperatures.
Consider a reaction that has a negative ΔH and a positive ΔS. Which of the following statements is TRUE?
This reaction will be nonspontaneous only at low temperatures.
Consider a reaction that has a positive ΔH and a positive ΔS. Which of the following statements is TRUE?
This reaction will be spontaneous only at high temperatures.
Consider a reaction that has a positive ΔH and a positive ΔS. Which of the following statements is TRUE?
A pathway by which counter ions can flow between the half-cells without the solutions in the half-cell totally mixing.
Define a salt bridge.
a liquid becomes a gas
Define boiling.
Buffer capacity is the amount of acid or base that can be added to a buffer without destroying its effectiveness.
Define buffer capacity.
a gas becomes a solid
Define deposition.
the phase transition from solid to liquid
Define fusion.
The entropy of a perfect crystal at absolute zero (0 K) is zero.
Define the third law of thermodynamics.
9.22 x 10^-9 M
Determine the molar solubility of AgI in pure water. Ksp (AgI) = 8.51 x 10^-17
2.223
Determine the pH of a 0.00598 M HClO4 solution.
rate of dissolution > rate of deposition.
Dissolving can be defined as
dynamic
Equilibrium in which rate of the forward reaction equals the rate of the reverse reaction is
a positive ΔH and a positive ΔS
For the following example, identify the following. H2O(l) → H2O(g)
a negative ΔH and a negative ΔS
For the following example, identify the following. H2O(l) → H2O(s)
the rate of the reaction is directly proportional to the concentration of the reactant.
Give the characteristic of a first order reaction having only one reactant.
The rate of the reaction is proportional to the square of the concentration of the reactant.
Give the characteristic of a second order reaction having only one reactant.
The rate of the reaction is not proportional to the concentration of the reactant.
Give the characteristic of a zero order reaction having only one reactant.
ionizes completely in an aqueous solution, has equilibrium far to the right, has a polar bond, has a weaker bond to hydrogen. (all of the above)
Give the characteristics of a strong acid.
the reverse reaction is favored
Give the direction of the reaction, if K << 1.
The forward reaction is favored.
Give the direction of the reaction, if K >> 1.
critical temperature
Give the term for the temperature at which the gas and liquid phases form a supercritical fluid.
Al(OH)3 precipitates
Give what happens at neutral pH for aluminum hydroxide
4 2 He
ID an alpha particle
increase in oxidation number, loss of electrons (both A and B)
ID oxidation.
H2SO4 (2 H)
ID the diprotic acid
7.4
ID the pH of normal blood.
H3PO4 (3 H)
ID the triprotic acid
Phenolphthalein
Id the most common indicator
salt, moisture, and acid (all of the above)
Identify a component in the formation of rust.
H2(g)
Identify the compound with the standard free energy of formation equal to zero.
the anode
Identify the location of oxidation in an electrochemical cell.
the cathode
Identify the location of reduction in an electrochemical cell.
rusting of iron
Identify the process that is spontaneous.
Free atoms have greater entropy than molecules
Identify the statement that is FALSE. A) The entropy of a gas is greater than the entropy of a liquid. B) Entropy generally increases with increasing molecular complexity. C) Free atoms have greater entropy than molecules. D) Entropy increases with dissolution. E) For noble gasses, entropy increases with size.
H2Te
Identify the strongest acid. (increases down a column)
capillary action
Identify the term used to describe the ability of a liquid to flow against gravity up a narrow tube.
H2SO3 and H2CO3
Identify the weak Diprotic acid (2 questions)
HF
Identify the weakest acid. (weakest at the top of a column)
9.10 x 10^-4
If a chemist wishes to prepare a buffer that will be effective at a pH of 3.00 at 25 degrees C, the best choice would be an acid component with a Ka equal to __________
[HCHO2] > [NaCHO2]
If the pKa of HCHO2 is 3.74 and the PH of an HCHO2/NACHO2 solution is 3.11 which of the following is true?
HCHO2=NaCHO2
If the pKa of HCHO2 is 3.74 and the pH of an HCHO2/NaCHO2 solution is 3.74 which of the following is true?
HCHO2<NaCHO2
If the pKa of HCHO2 is 3.74 and the pH of an HCHO2/NaCHO2 solution is 3.89 which of the following is true?
∞
In a reaction mixture containing only products, what is the value of Q?
0
In a reaction mixture containing only reactants, what is the value of Q?
1
In a reaction mixture containing reactants and products, each at a concentration of 1M, what is the value of Q?
Ka1
In a triprotic acid, which Ka has the highest value?
reactant
In endothermic reactions heat is a __________
product
In exothermic reactions heat is a ________
10^9
Parts per billion requires a multiplication factor of
CH4 < CH3CH3 < CH3CH2CH3
Place the following compounds in order of increasing strength of intermolecular forces. CH4 CH3CH2CH3 CH3CH3
N2H4 > HCl > He
Place the following in order of decreasing molar entropy at 298 K. HCl N2H4 He
HBrO<HBrO2<HBrO3<HBrO4
Place the following in order of increasing acid strength. HBrO2 HBrO3 HBrO HBrO4
H2O(s) < H2O(l) < H2O(g)
Place the following in order of increasing standard molar entropy. H2O(l) H2O(g) H2O(s)
second
The ________ Law of Thermodynamics states that for any spontaneous reaction, the entropy of the universe increases.
third
The ________ Law of Thermodynamics states the entropy of a perfect crystal at absolute zero is zero.
[reactant] vs. time
What data should be plotted to show that experimental concentration data fits a zeroth-order reaction?
Cr Oxidized, Cl reduced
What element is being oxidized and reduced in the following redox reaction? Cr(OH)4−(aq) + ClO−(aq) → CrO42-(aq) + Cl−(aq)
An electrolytic cell is an electrochemical cell that drives a non-spontaneous redox reaction through the application of electrical energy.
What is an electrolytic cell?
1.21 x 10^-7 M
What is the concentration of hydroxide ions in pure water at 30 degrees C is Kw at this temp is 1.47 x 10^-14? (H3O+ x OH- = Kw)
H2CO3
What is the conjugate acid of HCO3^-?
HPO4^2-
What is the conjugate base of H2PO4^-?
positive
What is the sign of ΔSuniv for a biological system?
dipole-dipole
What is the strongest type of intermolecular force present in CH2F2?
hydrogen bonding
What is the strongest type of intermolecular force present in NH2CH3?
pH will be less than 7 at the equivalence point
When titrating a monoprotic strong acid with a weak base at 25 degrees C, the _____________
pH will be equal to 7 at the equivalence point
When titrating a strong monoprotic acid with KOH at 25 degrees C, the ____________
pH will be greater than 7 at the equivalence point
When titrating a weak monoprotic acid with NaOH at 25 degrees C, the ______________
HClO2, 1.1 x 10^-2
Which of the following acids is the strongest? it is followed by its Ka, (Ka low is strong)
HIO, 2.3 x 10^-11
Which of the following acids is weakest?
HCN
Which of the following acids will have the STRONGEST conjugate BASE? (so is must be a weak acid)
entropy, enthalpy, and gibbs free energy (all of the above)
Which of the following are extensive properties?
(CH3CH2)2NH, 8.6 x 10^-4
Which of the following bases is the strongest? (low 10^ value of Kb= strongest)
C5H5N, 1.7 x 10^-9
Which of the following bases is the weakest? (high value Kb = weakest)
H3O+/OH-
Which of the following is NOT a conjugate acid-base pair?
A buffer is most resistant to pH change with [acid] = [conjugate base]
Which of the following is TRUE regarding buffers?
The equivalence point is where the amount of acid equals the amount of base during any acid-base titration
Which of the following is true regarding equivalence point?
an acidic solution has H3O+> OH-
Which of the following is true regarding solutions?
Condensation of water vapor into rain drops
Which of the following processes have a ΔS < 0?
C) CH4(g) + H2O(g) → CO(g) + 3 H2(g)
Which of the following processes have a ΔS > 0? A) CH3OH(l) → CH3OH(s) B) N2(g) + 3 H2(g) → 2 NH3(g) C) CH4(g) + H2O(g) → CO(g) + 3 H2(g) D) Na2CO3(s) + H2O(g) + CO2(g) → 2 NaHCO3(s) E) All of the above processes have a DS > 0.
.10 M HCN and .10 M LiCN .10 M HC2H3O2 and .10 M LiC2H3O2
Which of the following solutions is a good buffer system? (2 questions)
HCN, 4.9 x 10^-10
Which of the following solutions would have the highest pH? the acid is followed by its Ka value.
HClO2, 1.1 x 10^-2
Which of the following solutions would have the lowest pH? (low Ka 10^)
HPO4^-
Which of the following species is amphoteric?
Vapor pressure increases with temperature.
Which of the following statements is TRUE?
none of the above
Which of the following statements is TRUE? A) If N/Z ratio is too high, there are too many protons and the nuclide will undergo positron emission or electron capture. B) If N/Z ratio lies somewhere below 1, the nuclide is stable. C) If N/Z ratio is too low, there are too many neutrons and the nuclide will undergo beta decay. D) The valley of stability is the geographic location where many of the known nuclides were first discovered.
all of the above
Which of the following statements is TRUE? A) Positrons are similar in ionizing power and penetrating power to beta particles. B) A positron is the antiparticle of the electron. C) Beta decay occurs when a neutron changes into a proton while emitting an electron. D) An alpha particle is a helium 2+ ion.
There is a "heat tax" for every energy transaction.
Which of the following statements is TRUE? (regarding energy)
Entropy is an extensive property.
Which of the following statements is TRUE? regarding entropy
Gamma rays have the lowest ionizing power of any radioactivity.
Which of the following statements is TRUE? regarding radiation
The solubility of a solid is highly dependent on temperature.
Which of the following statements is generally true regarding solubility?
The conjugate base of a very weak acid is stronger than the conjugate base of a strong acid.
Which of the following statements is true regarding the conjugate base?
I2(g)
Which one of the following has the highest standard molar entropy, S°, at 25°C?
BaO and NaF
Which one of the following salts when dissolved in water produces the solution with the highest pH? (2 questions)
AlI3
Which one of the following salts when dissolved in water produces the solution with the lowest pH?
NH4Cl
Which one of the following will form an acidic solution in water?
e) all of the above
Why is water an extraordinary substance? A) Water has a low molar mass, yet it is a liquid at room temperature. B) Water is the main solvent within living organisms. C) Water has an exceptionally high specific heat capacity. D) Water has strong hydrogen bonding. E) All of the above
entropy
________ is a thermodynamic function that increases with the number of energetically equivalent ways to arrange components of a system to achieve a particular state.
CH3COOH
_________ is the active component in vinegar
H2CO3
___________ is found in carbonated beverages due to the reaction of carbon dioxide with water
Lewis definition
acids accept or need electron pairs, bases donate and electron pair to another substance
Arrhenius
acids are substances when dissolved in water produce H30+ bases are substances that when dissolved in water produce OH-
neither direction is favored
give the direction of the reaction, if K ≈ 1.
significant amounts of both a weak acid and its conjugate base
identify a good buffer
10
the highest pH for an effective buffer occurs when the base is how many times as concentrated as the acid?