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WorksheetsAP Chem Review Quiz 1
Total questions: 25
Worksheet time: 49mins
Which of the following liquids experiences dipole-dipole intermolecular forces?
O2(l)
CCl4(l)
SO3(l)
CF2Cl2
Which of the following best explains why temperature increases cause reaction rates to increase?
As temperature increases, activation energy increases
As temperature increases, activation energy decreases
As temperature increases, collisions between reactant particles increases
As temperature increases, more collisions between particles have a required amount of energy.
A sample of a solid substance conducts electricity in both the solid and liquid phase. Which of the following types of interactions is most likely found between particles in the substance?
ionic bonds
metallic bonds
covalent bonds
hydrogen bonds
N2(g) + 3 H2(g) ---> 2 NH3(g) ΔH<0
Gaseous ammonia was synthesized in the presence of a catalyst and allowed to reach equilibrium. Which of the following changes would cause more ammonia to be present in the mixture when equilibrium is reestablished?
increase the temperature
increase the container’s volume
add a chemical that reacts with hydrogen gas
add hydrogen gas to the container
Which of the following shows the molecules F2, Cl2, and Br2 in order of their bond enthalpies from least to greatest?
F2 < Cl2 < Br2
Cl2 < Br2 < F2
Br2 < Cl2 < F2
Br2 < F2 < Cl2
Based on Coulomb’s Law and the data in the table above, which of the following would have the weakest interactions with an adjacent water molecule in an aqueous solution?
Hg2+
Ba2+
Al3+
Mg2+
On the basis of the data in the table above, which of the following arranges the bonds in molecules from least to most polar?
NF3 < NO2 < CF4 < OF2
CF4 < NO2 < OF2 < NF3
NO2 < OF2 < NF3 < CF4
NF3 < NO2 < OF2 < CF4
For element X, which of the following most likely explains the large difference between the 3rd and 4th ionization energies?
The effective nuclear charge decreases with each successive ionization energy
The distance between the nucleus and the electron being removed increases with each successive ionization energy
The electron removed for the 4th ionization energy has much less energy than the electron removed for the 3rd ionization energy
The ionic radius increases with each successive ionization energy
A student performs an acid base titration. The data are plotted above. Which of the following best describes the type of titration done?
a strong acid was titrated with a strong base
a weak acid was titrated with a strong base
a strong acid was titrated with a weak base
a weak acid was titrated with a weak base
A student performs an acid base titration. The data are plotted above. Which of the following best describes the type of titration done?
a strong base was titrated with a strong acid
a weak base was titrated with a strong acid
a strong base was titrated with a weak acid
a weak base was titrated with a weak acid
A sample of a compound contains 24.0 g C, 5.0 g H, and 8.0 g O. Which of the following is the empirical formula of the compound?
C2H5O
C4H10O
C6H15O2
C8H20O2
The Ksp values of several salts are shown in the table above. A saturated solution of which of the following compounds has the highest Br- concentration?
PbBr2
CuBr
AgBr
HgBr2
The Ksp values of several salts are shown in the table above. A saturated solution of which of the following compounds has the lowest Br- concentration?
PbBr2
CuBr
AgBr
HgBr2
Based on the following information
3 Pb + 2 Au3+ ---> 3 Pb2+ + 2 Au Eo = 1.63 V
Pb2+ + 2e- ---> Pb Eo = ?
Au3+ + 3 e- ---> 2 Au Eo = 1.50 V
What is the standard reduction potential for the lead (II) half reaction?
-3.13 V
-0.13 V
+0.13 V
+3.13 V
Based on the following information
3 Pb + 2 Au3+ ---> 3 Pb2+ + 2 Au Eo = 1.63 V
Pb2+ + 2e- ---> Pb Eo = ?
Au3+ + 3 e- ---> 2 Au Eo = 1.50 V
Which of the following is true for the reaction overall balanced reaction listed above under standard conditions?
K>1, ΔGo<0
K>1, ΔGo>0
K<1, ΔGo>0
K<1, ΔGo<0
C2H2(g) + H2(g) ---> C2H4(g)
For the reaction above, which of the following will most likely increase the rate of reaction?
decrease the temperature of the reaction container
decrease the volume of the reaction container
pressurize the system with an inert gas, keeping temperature constant
remove acetylene (C2H2) from the reaction container
Which of the following molecules is least soluble in water?
CH2F2
CH3OH
CH2O
CH3CH3
At room temperature, bromine, Br2, is a liquid. Which of the following provides a characteristic of bromine with a correct explanation?
bromine has a higher boiling point than chlorine (which is a gas at room temperature) because bromine has more electrons than chlorine
bromine has a lower first ionization energy than krypton (an atomic element that is a gas at room temperature) because bromine is a liquid at room temperature.
bromine is a not a good conductor of electricity because it has lone pairs of electrons.
bromine is soluble in water because bromine is polar.
Based on the information in the table above, which liquid has a higher vapor pressure at 25oC and why?
CBr4(l), because it has weaker intermolecular forces
CBr4(l), because it has stronger intermolecular forces
CCl4(l), because it has weaker intermolecular forces
CCl4(l), because it has stronger intermolecular forces
HX(aq) + Y-(aq) <===> HY(aq) + X-(aq) K = 1.5 x 10-5
Based on the information above, which is the strongest acid?
HX(aq)
Y-(aq)
HY(aq)
X-(aq)
Pb(NO3)2(aq) + Na2CO3(aq) --> PbCO3(s) + Na2CO3(aq)
A student wanted to determine the molarity of lead(II) nitrate in a solution. She added a large excess of sodium carbonate solution to a sample of the Pb(NO3)2 solution. The lead(II)carbonate precipitate was collected via filtration and dried. After analyzing the data, the student results suggested the lead(II) nitrate concentration was 3% higher than expected. Which of the following could account for this error?
The precipitate was dried at too high a temperature, causing some of the solid to decompose into CO2 and PbO.
The filter paper allowed some of the precipitate to escape into the liquid portion
Not all the liquid and precipitate was transferred to the filter paper
the precipitate was not rinsed with distilled water after collection
A student titrated a 30.0 mL sample of hydrochloric acid with 1.00 M NaOH. She plotted the experimental data and obtained the graph above.
At point B in the plot, which ions have a concentration greater than 0.10 M?
only Na+, Cl-
only Na+, Cl-, OH-
only Na+, Cl-, H+
only Na+, Cl-, H+, OH-
A student titrated a 30.0 mL sample of hydrochloric acid with 1.00 M NaOH. She plotted the experimental data and obtained the graph above.
How would the titration curve above differ if the student used 0.100 M NaOH rather than 1.00 M NaOH for the titrant?
The initial pH would be 1, rather than 0
The pH at equivalence would be higher than in the original titration
The pH well past the equivalence point would be lower than in the original titration
The pH well past the equivalence point would be higher than in the original titration
A student conducted an experiment to determine for the reaction between HCl(aq) and NaOH(aq) indicated in the table above, and determined the amount of heat released. Which of the following best explains the relationship between X and Y?
Y = 2X, because the volume of HCl(aq) used in trial 2 is twice the volume used in trial 1.
Y = X, because the number of moles of acid and base reacting with each other is the same in both trials.
Y = 2X/3, because the heat is distributed over more particles in trial 2 than in trial 1.
The relationship between X and Y cannot be predicted.
A student mixes a 10.0mL sample of 1.0M NaOH(aq) with a 10.0mL sample of 1.0M HCl(aq) in a polystyrene container. The temperature of the solutions before mixing was 20.0◦C. If the final temperature of the mixture is 26.0◦C, what is the experimental value of ΔH0? (Assume that the solution mixture has a specific heat of 4.2J/(g•K) and a density of 1.0g/mL.)
-50.0kJ/molrxn
-25 kJ/molrxn
-5.0x104 kJ/molrxn
-5.0x102 kJ/molrxn
