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1) In which of the following aqueous solutions would you expect CuBr to have the
highest solubility?
A) 0.0100 M KBr
B) 0.040 M CuNO3
C) 0.030 M NaBr
D) 0.020 M LiBr
E) CuBr will have the same solubility in all solutions.
2) Oxides of most nonmetals combine with base to form ________.
A) hydrogen gas
B) an acid
C) a base
D) water
E) water and a salt
3) A 25.0 mL sample of 0.723 M HClO4 is titrated with a 0.273 M KOH solution. The
H3O+ concentration after the addition of 0.00 mL of KOH is ________ M.
A) 0.0181
B) 0.430
C) 0.723
D) 0.273
E) none of the above
4) Calculate the work (kJ) done during a reaction in which the internal volume expands
from 14 L to 50 L against a vacuum (an outside pressure of 0 atm).
A) 0; kJ No work is done.
B) 3.6 kJ
C) -3.6 kJ
D) 6.5 kJ
E) -6.5 kJ
5) The value of ΔH° for the reaction below is -126 kJ. ________ kj are released when
2.00 mol of NaOH is formed in the reaction?
2Na2O2 (s) + 2H2O (l) → 4NaOH (s) + O2 (g)
A) 252
B) 63
C) 3.9
D) 7.8
E) -126
6) In which of the following aqueous solutions does the weak acid e xhibit the highest
percentage ionization?
A) 0.01 M H2SO3 (Ka = 1.4 x 10-2)
B) 0.01 M HCN (Ka = 6.2 x 10-10)
C) 0.01 M H2CO3 (Ka = 4.5 x 10-7)
D) 0.01 M HC3H5O2 (Ka = 1.3 x 10-5)
E) 0.01 M HOCl (Ka = 3.5 x 10-8)
7) Ammonia is a ________.
A) weak acid
B) strong base
C) weak base
D) strong acid
E) salt
8) The half-life of 131I is 0.220 years. How much of a 500.0 mg sample remains after 24
hours?
A) 496 mg
B) 560 mg
C) 219 mg
D) 405 mg
E) 337 mg
9) CO (5.00 g) and CO2 (5.00 g) were placed in a 750.0 mL container at 50.0 °C. The
partial pressure of CO2 in the container was ________ atm.
A) 4.02
B) 10.3
C) 1.60
D) 0.292
E) 6.31
10) Which electron configuration denotes an atom in its ground state?
A)
B)
C)
D)
E)
11) The value of ΔH° for the reaction below is -1107 kJ:
2Ba (s) + O2 (g) → 2BaO (s)
How many kJ of heat are released when 5.75 g of Ba (s) reacts completely with oxygen
to form BaO (s)?
A) 96.3 kJ
B) 26.3 kJ
C) 46.4 kJ
D) 23.2 kJ
E) 193 kJ
12) Given the data in the table below, ΔH°rxn for the reaction
SO3 (g) + H2O (l) → H2SO4 (l)
is ________ kJ.
A) -132
B) 1496
C) 704
D) -704
E) -2.16 x 103
13) Thermodynamic Quantities for Selected Substances at 298.15 K (25 oC)
The value of G o at 25 oC for the decomposition of phosphorous trichloride into its
constituent elements,
2PCl3 (g) --> P2 (g) + 3Cl2 (g)
is ________ kJ/mol.
A) -539.2
B) +539.2
C) -642.9
D) +642.9
E) -373.3
14) The subatomic particles located in the nucleus with no overall charges are
________.
A) electrons
B) protons
C) neutrons
D) protons and neutrons
E) protons, neutrons, and electrons
15) Which of the following is a statement of the first law of thermodynamics?
A)
B) A negative H corresponds to an exothermic process.
C) ΔE = Efinal - Einitial
D) Energy lost by the system must be gained by the surroundings.
E) 1 cal = 4.184 J (exactly)
16) Which one of the following compounds produces a basic solution when dissolved in
water?
A) Rb2O
B) SO2
C) OBr2
D) ZnCl2
E) N2
17) The energy of a photon that has a wavelength of 12.3 nm is ________ J.
A) 1.51 X 10-17
B) 4.42 X 10-23
C) 1.99 X 10-25
D) 2.72 X 10-50
E) 1.62 X 10-17
18) The kinetic energy of a 23.2-g object moving at a speed of 81.9 km/hr is ________
J.
A) 1900
B) 77.8
C) 145
D) 1.43 x 10-3
E) 6.00
19) Elements in Group 7A are known as the ________.
A) chalcogens
B) alkali metals
C) alkaline earth metals
D) halogens
E) noble gases
20) The correct name for HNO2 is ________.
A) nitrous acid
B) nitric acid
C) hydrogen nitrate
D) hyponitrous acid
E) pernitric acid
