As defined by Ludwig Boltzmann, the third law of thermodynamics states that
A.there is no disorder in a perfect crystal at 0 K.
B.in a spontaneous process, the entropy of the universe increases.
C.the total entropy of the universe is always increasing.
D.the total mass of the universe is constant.
E.mass and energy are conserved in all chemical reactions.
According to collision theory, which condition(s) must be met in order for molecules to
react?
1/ The reacting molecules must collide with sufficient energy to initiate the process of
breaking and forming bonds.
2/ A catalyst must be in contact with the reacting molecules for a reaction to occur.
3/ The reacting molecules must collide with an orientation that can lead to
rearrangement of the atoms.
A.1 only
B.2 only
C.3 only
D.1 and 2
E.1 and 3
Write the expression for Kp for the reaction below.
2 NOBr(g) 2 NO(g) + Br2( )
A.
B.
C.
D.
E.
What is the charge on a beta particle?
A.+2
B.+1
C.0
D.-1
E.-2
The principal product of the reaction of potassium and oxygen is not K2O. The product
is named ____ and has the formula ____.
A.dipotassium trioxide, K2O3
B.potassium monoxide, KO
C.potassium superoxide, KO2
D.potassium peroxide, K2O2
E.potassium trioxide, KO3
How many orbitals have the following set of quantum numbers: n = 5, = 3, = +2?
A.0
B.1
C.3
D.6
E.7
Copper has an average atomic mass of 63.55 u. If 69.17% of Cu exists as Cu-63
(62.93960 u), what is the identity and the atomic mass of the other isotope?
A.Cu-64; 63.82 u
B.Cu-64; 64.16 u
C.Cu-65; 64.16 u
D.Cu-65; 64.92 u
E.Cu-66; 65.91 u
If 5.15 g Fe(NO3)3 is dissolved in enough water to make exactly 150.0 mL of solution,
what is the molar concentration of nitrate ion?
A.0.00319 M
B.0.0343 M
C.0.142 M
D.0.313 M
E.0.426 M
A plot of the number of neutrons versus the number of protons in nuclei shows a narrow
band of stable isotopes. Isotopes with a low proton-neutron ratio (i.e., ones that fall
below the band of stability) decay by
A.positron emission or electron capture.
B.positron emission or alpha emission.
C.beta emission or electron capture.
D.gamma ray emission or beta emission.
E.neutron capture or alpha emission.
Which of the statement concerning the phase diagram is/are CORRECT?
1/ Only the solid phase exists at point A.
2/ At point C, the solid and liquid phases are in equilibrium.
3/ At point D, the critical point, the substance exists as a supercritical fluid.
A.1 only
B.2 only
C.3 only
D.1 and 3
E.1, 2, and 3
An electronic balance is used to determine that a sample has a mass of 4.94691 g. If the
balance’s precision is 0.02 mg, what is the correct number of significant figures for this
measurement?
A.2
B.3
C.4
D.5
E.6
If 495 J is required to change the temperature of 12.7 g of sodium chloride from 275.0
K to 335.0 K, what is the specific heat capacity of sodium chloride?
A.0.866 J/gK
B.2.60 J/gK
C.0.650 J/gK
D.1.15 J/gK
E.2.83 105 J/gK
The pH of a vinegar solution is 4.15. What is the H3O+ concentration of the solution?
A.7.1 10“5 M
B.1.6 10“2 M
C.0.62 M
D.1.4 M
E.1.4 104 M
Which one of the following molecules is polar?
A.CS2
B.SO2
C.XeF2
D.XeF4
E.SO3
Assuming the following reaction proceeds in the forward direction,
3 Sn4+(aq) + 2 Cr(s) 3 Sn2+(aq) + 2 Cr3+(aq)
A.Sn4+(aq) is the reducing agent and Cr(s) is the oxidizing agent.
B.Cr(s) is the reducing agent and Sn2+(aq) is the oxidizing agent.
C.Sn4+(aq) is the reducing agent and Sn2+(aq) is the oxidizing agent.
D.Cr(s) is the reducing agent and Cr3+(aq) is the oxidizing agent.
E.Cr(s) is the reducing agent and Sn4+(aq) is the oxidizing agent.
Which of the following chemical equations corresponds to Ka3 of phosphoric acid?
A.HPO4
2″(aq) + H2O( ) PO4
3″(aq) + H3O+(aq)
B.PO4
3″(aq) + H2O( ) HPO4
2″(aq) + OH“(aq)
C.H3PO4(aq) + H2O( ) H2PO4
“(aq) + H3O+(aq)
D.H3PO4(aq) + 2 H2O( ) HPO4
2″(aq) + 2 H3O+(aq)
E.H2PO4
“(aq) + H2O( ) HPO4
2″(aq) + H3O+(aq)
Which of the following mathematical expressions is the Henderson-Hasselbalch
equation?
A.
B.
C.
D.
E.
What 2+ ion has the following ground state electron configuration?
A.Mn2+
B.Co2+
C.Ni2+
D.Cu2+
E.Ge2+
The number of disintegrations per minute (dsm) of a sample of iodine-133 is measured
at 5.5 102 dsm. When the sample is measured 295 minutes later, the number of
disintegrations has decreased to 4.7 102 dsm. What is the half-life of iodine-133?
A.5.7 10“4 m.
B.2.6 m.
C.1.3 103 m.
D.3.9 102 m.
E.9.7 104 m.
Which of the following combinations would be best to buffer an aqueous solution at a
pH of 7.0?
A.H3PO4 and H2PO4
“, Ka1 = 7.5 10“3
B.HNO2 and NO2
“, Ka = 4.5 10“4
C.CH3CO2H and CH3COO“, Ka = 1.8 10“5
D.H2PO4
“ and HPO4
2″, Ka2 = 6.2 10“8
E.NH4
+ and NH3, Ka = 5.7 10“10
A 2.5 L flask is filled with 0.25 mol SO3, 0.20 mol SO2, and 0.40 mol O2, and allowed
to reach equilibrium. Assume the temperature of the mixture is chosen so that Kc =
0.12. Predict the effect on the concentration of SO3 as equilibrium is achieved by using
Q, the reaction quotient.
2 SO3(g) 2 SO2(g) + O2(g)
A.[SO3] will decrease because Q > K.
B.[SO3] will decrease because Q < K.
C.[SO3] will increase because Q < K.
D.[SO3] will increase because Q > K.
E.[SO3] will remain the same because Q = K.
The becquerel is an SI unit for the measurement of radiation. One Bq represents
A.1 J energy absorbed per kg of tissue.
B.3.7 1010 disintegrations per second.
C.1 disintegration per second.
D.0.01 J energy absorbed per kg of tissue.
E.1 calorie energy absorbed per kg of tissue.
Lead-200 has a half-life of 21.5 hours. Starting with 3.77 mg of this isotope, how much
would remain after 72 hours?
A.0.0 mg
B.0.098 mg
C.0.37 mg
D.0.47 mg
E.1.1 mg
An unknown gaseous hydrocarbon contains 85.63% C. Its density is 1.524 g/L at 0.665
atm and 373 K. What is the molecular formula of the gas? (R = 0.08206 Latm/molK)
A.C2H4
B.C3H6
C.C4H8
D.C5H10
E.C6H12
CaO(s) reacts with water to form Ca(OH)2(aq). If 6.50 g CaO is combined with 99.70 g
H2O in a coffee cup calorimeter, the temperature of the resulting solution increases
from 21.7 C to 43.1 C. Calculate the enthalpy change for the reaction per mole of CaO.
Assume that the specific heat capacity of the solution is 4.18 J/gK.
A.”1.45 kJ/mol
B.”82.0 kJ/mol
C.”9.42 kJ/mol
D.”165 kJ/mol
E.”532 kJ/mol
Phosphorus was first isolated in 1669 by Hennig Brandt, a German alchemist. Brandt
was able to isolate approximately 30 grams of phosphorus from 60 gallons of
________.
A.sea water
B.Chilean saltpeter
C.urea
D.honey
E.urine
If a pure substance begins at point C on the phase diagram below and the pressure on
the substance is increased until point B is reached, what process occurs?
A.fusion
B.vaporization
C.condensation
D.sublimation
E.none of these
What is the name of the following compound?
A.pentanol
B.cyclopentane
C.cyclohexane
D.cyclopentene
E.1,5-pentane
The conjugate base of OH“ is ____.
A.H3O+
B.OH+
C.O2″
D.H+
E.OH“
Write a balanced chemical equation for the electrolysis of brine (i.e., salt water).
A.2 NaCl(aq) + 2 H2O( ) 2 Na(s) + 2 HCl(aq) + O2(g)
B.2 NaCl( ) 2 Na( ) + Cl2(g)
C.2 NaCl(aq) + O2(g) Na2O2(s) + Cl2(g)
D.4 NaCl(aq) + O2(g) 4 Na(s) + 2 OCl2(g)
E.2 NaCl(aq) + 2 H2O( ) Cl2(g) + 2 NaOH(aq) + H2(g)
Which element is most likely to form a 2″ ion?
A.K
B.Mg
C.P
D.Br
E.S