Intermolecular Forces
Solubility
Acids and Bases
Equilibrium
Free Energy
100
Which of the following would you expect to have the highest boiling point? a. H2 b. CH4 c. F2 d. HBr
HBr
100
The solubilty of gas in H2O (liquid) will increase with increasing a. temperature b. vapor pressure of gas c. volume of gas d. molar mass of gas
vapor pressure of gas
100
Which is the weakest acid of the following a. Formic acid Ka = 1.8 x 10^-4 b. Phenol Ka = a.3 x 10 X 10^-10 c. Acetic acid Ka = 1.8 x 10^-5 d. Hydrocyanic acid Ka = 2.9 x 10^-8
Phenol Ka = a.3 x 10 X 10^-10
100
Select the correct statement for the reaction and information provided N2 (g) + 3 H2 (g) --><-- 2 NH3 (g) Kc = 3.5 x 10^-8 a. The reaction rate must be very slow b. At equilibrium, the concentration of NH3 is very high compared to N2 and H2. c. At equilibrium, the concentration of NH3 will be equal to the sum of the concentration of N2 and H2. d. The reaction is an endothermic process.
At equilibrium, the concentration of NH3 is very high compared to N2 and H2.
100
Which of the following process would lead to a decrease in entrophy? a. Hg (s) --> Hg (l) b. 2 SO3 (g) --> 2 SO2 (g) + O2 (g) c. 4 Fe (s) + 3 O2 (g) --> 2 FeO3 (s) d. C2H4 (g) --> C2H2 (g) + H2 (g)
4 Fe (s) + 3 O2 (g) --> 2 FeO3 (s)
200
Which of the following would have the highest vapor pressure? a. H2O b. HCl c.CH3CH3 d. CH3OH
CH3CH3
200
Which of the following would be most soluble in hexane (C6H6) a. NH3 b. CCl4 c. H2O d. NaNO3
CCl4
200
Which acid/base pair should be used to prepare a buffer pH of 10.0? a. Carbonic acid (ka = 4.7 x 10^-11) b. Benzoic acid (ka = 6.4 x 10^-5) c. Acetic acid (ka = 1.8 x 10^-5) d. hydrofluoric acid (ka = 6.3 x 10^-4)
Carbonic acid (ka = 4.7 x 10^-11)
200
The equilibirum constant is 0.50 at 600oC. The initial concentrations of HCHO is 1.5 M, H2 is 0.5 M and CO is 1.0 M. Which of the following is true for the reaction HCHO--><-- H2 + CO a. The reaction mixture is at equilibrium b. No reaction will occur c. More HCHO will be formed d. More H2 and CO will be formed
More H2 and CO will be formed
200
Which statement is true for the following spontaneous (product- favored) reactions at 298K? CaO (s) + CO2 (g)--> CaCO3 (s) a. Delta S is positive for the reaction b. Delta H is negative for the reacion c. Delta is "0" for the reaction d. The reaction will be spontaneous (reactant- favored) at high temperatures
Delta H is negative for the reacion
300
Which species has the strongest London Dispersion Forces? a. Xe b. Ne c. Ar d. Rn
Rn
300
A solution is formed at room temperature by vigorously dissolving enough of solid solute so that some solid remains at the bottom of the solution. Which statement is true? a. Solution is considered unsaturated b. Solution is considered supersaturated c. Solution is considered saturated d. Solution would be considered unsaturated if it were cooled a bit to increase solubility of the solid
Solution is considered saturated
300
For propionic acid with a Ka = 1.3 x 10^-5. How many grams of sodium propionic (molar mass = 96.08 g/mol) would need to dissolve in 0.100 M propionic acid in order to make 200.0mL of solution with pH of 5.0?
2.56
300
For the following exothermic reaction: 2 NO (g) + H2 (g) -->N2O (g) + H2O (g). In which direction, left or right, will the equilibrium shift if the following changes are made? a. NO is added b. H2 is removed c. N2O is added d. decrease in temperature e. pressure is increased
a. right b. left c. left d. right e. right
300
If the reaction is reactant favored (nonspontaneous) at all temperatures, it is true that a. Delta H is negative and delta S is positive b. Delta H is positive and delta S is positive c. Delta H is negative and delta S is negative d. Delta H is positive and delta S is negative
Delta H is positive and delta S is negative
400
Which of the following would display hydrogen bonding? a. H2 b. NH3 c. PH3 d. Cl2
NH3
400
Two liquids, methanol and propanol, are miscible in each other. Which of the following statements is true? a. Methanol is a polar molecule and propanol is a nonpolar molecule. b. Primary attractive forces between the two molecules would be London Dispersion. c. After mixing the two liquids, they will form two distinct layers in the container. d. Solute- solvent interactions are at least equal to or more favorable than solute-solute and solvent-solvent interactions
Solute- solvent interactions are at least equal to or more favorable than solute-solute and solvent-solvent interactions
400
The conjugate base of HPO4^-2 is a. H3PO4 b. HPO4^-2 c. PO4^-3 d. H3O^+1
PO4^-3
400
Consider the reaction: NH4HS (s) --> NH3 (g) + H2S (g) An equilibrium mixture of this reaction at a certain temperature has NH3 = 0.278 M and H2S = 0.355 M. What is the value of the equilibrium constant (kc) at this temperature?
Kc= 0.0987
400
Determine Delta G for a reaction where delta H is -226.8 kJ and delta S is 58.84 J/k? Is it spontaneous or nonspontaneous?
-244.3 kJ and spontaneous
500
Rank the following compounds from weakest intermolecular forces to strongest. H2S, I2, N2, H2O
N2<I2<N2<H2O
500
When concentrated HCl is dissolved in water the solution becomes very hot. It is therefore true that a. Hydration process is exothermic in nature b. Hydration process requires input of energy to occur c. Covalent bonds within water are broken in hydration process d. Hydration process is endothermic in nature
Hydration process is exothermic in nature
500
A 0.150 M solution of a weak base has a pH of 10.5. What is the Kb for the weak acid?
Kb= 6.67 x 10^-7
500
Consider the reaction: 2 H2S (g) <----> 2 H2 (g) + S2 (g) A 0.120 mol sample of H2S was initially placed in a 24.0 L flask and heated. The Kc= 1.35 x 10^-9. Determine the equilibrium concentrations of all species in the mixture.
H2S = 4.95 x 10^-3 M H2 = 4.072 x 10^-5 M S2 = 2.036 x 10^-5 M
500
If delta G is 52.38 kJ for a reaction with a temperature of 350oC, find the equilibrium constant for the reaction.
4.05 x 10^-5
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