Exam 1
Exam 2
Exam 3
Exam 4
RANDOM!?!?!
100
Liquid and vapor phases of a substance become indistinguishable at the . . .
Critical Point
100
Which is not usually a factor in determining the rate of a reaction according to collision theory? a) Orientation of the colliding molecules b) Enthalpy of reaction c) Temperature of the reaction mixture d) collision frequency of the molecules
b) Enthalpy of reaction
100
What is the pH of a 0.035 M HBr solution?
1.46
100
Describe the pH curve of a titration of a weak base with a strong acid?
has a plateau before achieving equilibrium at a shifted acidic pH . . . . look at his curves.
100
Which of the following is the best definition of a Lewis Acid? a) Substance that increases the concentration of H3O+ in water b) an electron pair acceptor c) a proton donor d) a proton acceptor
B) an electron pair acceptor
200
Assume the krypton crystallizes into a FCC unit cell. If the atomic radius of Kr is 183 pm, what is the length of the edge of the cell?
518 pm
200
A 1st order reaction has a half-life of 15.0 seconds. What is the rate constant?
0.046 seconds
200
Which is TRUE for this reaction? HCOOH + H20 ---> HCOO- + H3O+ a) in this reaction, HCOOH and H2O are a conjugate acid/base pair b) in this reaction, the equilibrium lies to the left c) in this reaction, HCOOH is a stronger acid than H3O+ d) in this reaction, H2O is a spectator
B) in this reaction, the equilibrium lies to the left
200
Which of the following statements is TRUE about spontaneous processes? a) A spontaneous process must be endothermic b) A spontaneous process must be exothermic c) A spontaneous process must increase the randomness of the universe d) A spontaneous process must increase the entropy of the system
C) A spontaneous process must increase the randomness of the universe
200
In a solution made up of CaS and hexane (C6H14) what is the main IMF between solute and solvent?
Ion/Induced Dipole Forces
300
Suppose the phase diagram for methanol (CH3OH) has a solid-liquid curve with a negative slop. Which statement is true based on this statement? a) Solid Ch3OH has the same density as liquid Ch3OH b) Solid Ch3OH has a lower density than liquid Ch3OH c) Ch3OH vapor has the same density as liquid Ch3OH d) Solid Ch3OH has a higher density than liquid Ch3OH
B) Solid Ch3OH has a lower density than liquid Ch3OH
300
What is the equilibrium constant expression for the following? 2 CaBr2 (s) + O2 (g) --> 2 CaO (s) + 2 Br2 (g)
Keq = [Br]^2 / [O2]
300
Suppose a 0.50 M solution of weak hypo-iodous acid has a pH of 4.09 what is the Ka of this acid?
1.3 E -8
300
What is the delta G in kJ at 298 K for a reaction for which K = 1.25 E 3
-17.7
300
Assume that for the following reaction Kc = 2.00 2 SO2 + O2 <--> 2 SO3 If initial concentrations o 2.00 mol/L for each species are placed in the reaction vessel, which way must the reaction shift to reach equilibrium? and Why?
Right, because Q < K
400
A Chemist dissolves 1.75g of an unknown compound in 3.00 g of water. The solution freezes at -2.14 degrees Celsius. If the normal freezing point of water is 0 degrees Celsius and the kf for water is 1.86 deg/molal, what is the molar mass of the compound?
507 g/mol
400
The method of initial rates was used to collect the data below for the following reaction: X + Y --> Products Experiment 1 // X = 3.00 Y = 0.880 Rate = 1.00 E-3 Experiment 2 // X = 1.50 Y = 0.880 Rate = 0.500 E-3 Experiment 3 // X = 1.50 Y = 0.440 Rate = 0.250 E-3 What is the correct rate law?
k[X][Y] overall 2nd order rxn
400
What is the molar solubility of HgBr2 (Ksp = 7.4 E-11) in the presence of 0.30 M KBr?
8.2 E-10
400
Find the pH during the titration of 50.00 mL of 0.1000 M formic acid, HCOOH (Ka = 1.8E-4), after the addition of 50.00 mL of 0.1000 M NaOH titrant.
8.22 pH
400
Put the following species in order of acidity, from most basic on the left to most acidic on the right HOCl, H2O, NH4+, H30+
NH4+, H2O, HOCl, H30+
500
Assume that acetone has a vapor pressure of 0.525 atm at 305 K, and 1.050 atm at 335 K. What is the value of delta H vaporization for acetone? in kj/mol
19.6 kj/mol
500
Consider the second order decomposition of "R" under the following conditions: The initial concentrate of R is 0.200 M and the rate constant is equal to 0.100 1/ M s R --> Products What is the concentration of R after 10.0 s?
0.167 M
500
What is [OH-] for a 0.050 M solution of the weak base methyl amine? CH3NH2's Kb = 9.8E-4 . . . . . . oooohhhhhhhh this is a difficult problem . . . . .
0.0065 M
500
Balance this chemical reaction? And tell me how many moles of H+ there are? MnO2 + Sn --> Mn 2+ + Sn 4+
8 moles of H+
500
Which of the following statements about spontaneous voltaic cells is true? a) Electric current in the salt bridge is carried by free electrons b) the electrons in the external wire flow from anode to cathode c) the cathode is labeled as negative (-) d) Oxidation occurs at the anode and cathode
B) the electrons in the external wire flow from anode to cathode
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