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Chemistry
Q:
A solution is 2.25% by mass NaHCO3. How many grams of NaHCO3 are in 150.0 g of solution?
A) 1.50 g
B) 3.38 g
C) 66.7 g
D) 225 g
Q:
What molality of pentane is obtained by dissolving 15 g pentane, C5H12, in 245.0 g hexane, C6H14?
A) 0.058 m
B) 0.068 m
C) 0.85 m
D) 61 m
Q:
To make a 2.00 m solution, one could take 2.00 moles of solute and add
A) 1.00 L of solvent.
B) 1.00 kg of solvent.
C) enough solvent to make 1.00 L of solution.
D) enough solvent to make 1.00 kg of solution.
Q:
To make a 0.500 M solution, one could take 0.500 moles of solute and add
A) 1.00 L of solvent.
B) 1.00 kg of solvent.
C) enough solvent to make 1.00 L of solution.
D) enough solvent to make 1.00 kg of solution.
Q:
How much water must be added to 40.0 g of CaCl2 to produce a solution that is 35.0 mass % CaCl2?
A) 54.0 g
B) 74.2 g
C) 87.5 g
D) 114 g
Q:
What volume of 3.00 M CH3OH solution is needed to provide 0.220 mol of CH3OH?
A) 1.52 mL
B) 13.6 mL
C) 73.3 mL
D) 660 mL
Q:
What volume of a 0.716 M KBr solution is needed to provide 30.5 g of KBr?
A) 21.8 mL
B) 42.7 mL
C) 184 mL
D) 357 mL
Q:
What is the weight percent of a caffeine solution made by dissolving 8.35 g of caffeine, C8H10N4O2, in 75 g of benzene, C6H6?
A) 0.010%
B) 0.011%
C) 10%
D) 11%
Q:
What is the mass percent of vitamin C in a solution made by dissolving 6.50 g of vitamin C, C6H8O6, in 55.0 g of water?
A) 0.547%
B) 1.21%
C) 10.6%
D) 11.8%
Q:
What is the mole fraction of oxygen in a gas mixture that is 37% oxygen and 63% nitrogen by volume?
A) 0.34
B) 0.37
C) 0.25
D) 0.52
Q:
What is the mole fraction of I2 in a solution made by dissolving 55.6 g of I2 in 245 g of hexane, C6H14?
A) 0.0715
B) 0.0770
C) 0.133
D) 0.154
Q:
What is the mole fraction of ethanol in a solution made by dissolving 29.2 g of ethanol, C2H5OH, in 53.6 g of water?
A) 0.176
B) 0.213
C) 0.352
D) 0.545
Q:
Which cation in each set is expected to have the larger (more negative) hydration energy?
I Be2+ or Ca2+
II Rb+ or Zn2+
A) Be2+ in set I and Rb+ in set II
B) Be2+ in set I and Zn2+ in set II
C) Ca2+ in set I and Rb+ in set II
D) Ca2+ in set I and Zn2+ in set II
Q:
At 80C, pure liquid A has a vapor pressure of 700 mm Hg and pure liquid B has a vapor pressure of 940 mm Hg. What is XA for a solution of A and B with a normal boiling point of A) 0.25B) 0.50C) 0.75D) A solution of A and B cannot boil at 80C.
Q:
What is the approximate boiling temperature of the liquid formed from the condensation of the vapor above a boiling solution that is 0.70 XA and 0.30 XB?
A) 50C
B) 55C
C) 90C
D) 100C
Q:
What is the approximate vapor composition above a boiling solution that is 0.70 XA and 0.30 XB ?
A) 0.70 XA, 0.30 XB
B) 0.50 XA, 0.50 XB
C) 0.30 XA, 0.70 XB
D) 0 XA, 1.00 XB
Q:
What is the approximate boiling temperature of a mixture that is 0.70 XA and 0.30 XB?A) 50CB) 75CC) 95CD) 100C
Q:
Assume that the vapor at point c is condensed and reboiled. What is the boiling point?A) temperature at point bB) temperature at point cC) temperature at point dD) temperature at point f
Q:
Assume that the vapor at point c is condensed and reboiled. What is the vapor composition during reboiling?
A) 100% decane
B) composition at point b
C) composition at point c
D) composition at point e
Q:
Assume that the vapor at point c is condensed and reboiled. What is the liquid composition of the condensed vapor prior to reboiling?
A) 100% decane
B) composition at point b
C) composition at point d
D) composition at point e
Q:
Assume that you start with a mixture containing 0.80 mol of decane and 0.20 mol of octane, what is the vapor composition at the boiling point?
A) 100% decane
B) composition at point b
C) composition at point c
D) composition at point e
Q:
Assume that you start with a mixture containing 0.80 mol of decane and 0.20 mol of octane, what is the liquid composition at the boiling point?
A) 100% decane
B) composition at point b
C) composition at point c
D) composition at point e
Q:
A phase diagram of temperature versus composition for a mixture of the two volatile liquids octane (bp = and decane (bp = 126C) is shown.Assume that you start with a mixture containing 0.80 mol of decane and 0.20 mol of octane, at what approximate temperature will the mixture begin to boil?A) temperature at point aB) temperature at point bC) temperature at point dD) temperature at point f
Q:
Assume that you start with a mixture containing 0.80 mol of decane and 0.20 mol of octane, what region of the diagram corresponds to vapor?A) region aB) region bC) region cD) regions a and c
Q:
A phase diagram of temperature versus composition for a mixture of the two volatile liquids octane (bp = and decane (bp = 126C) is shown.Assume that you start with a mixture containing 0.80 mol of decane and 0.20 mol of octane, what region of the diagram corresponds to liquid?A) region aB) region bC) region cD) regions a and c
Q:
Two beakers, one with pure water (light gray) and the other with an aqueous solution of KBr (dark gray), are placed in a closed container represented by drawing (a). Which of the drawings (a)-(d) represents what the beakers will look like after a substantial amount of time has passed?A) drawing (a)B) drawing (b)C) drawing (c)D) drawing (d)
Q:
Drawing (1) shows a nonequilibrium system comprised of pure water separated from an aqueous solution by a semipermeable membrane. Shaded spheres represent solute particles and unshaded spheres represent water molecules. Which drawing (2)-(5) represents this system after equilibrium is reached? A) drawing (2)
B) drawing (3)
C) drawing (4)
D) drawing (5)
Q:
The following diagram shows a close-up view of the vapor pressure curves for two pure liquids and two different solutions composed of these two liquids. Which curves represent pure liquids and which curves represent the solutions? A) Curves (a) and (b) are the pure liquids and curves (c) and (d) are the solutions.
B) Curves (a) and (c) are the pure liquids and curves (b) and (d) are the solutions.
C) Curves (a) and (d) are the pure liquids and curves (b) and (c) are the solutions.
D) Curves (c) and (d) are the pure liquids and curves (a) and (b) are the solutions.
Q:
Which curve is the solvent and what happens to the boiling point when the solute is dissolved in the solvent?
A) Curve (a) is the solvent and the boiling point decreases.
B) Curve (a) is the solvent and the boiling point increases.
C) Curve (b) is the solvent and the boiling point decreases.
D) Curve (b) is the solvent and the boiling point increases.
Q:
The following diagram shows a close-up view of the vapor pressure curves for a pure solvent and a solution containing a nonvolatile solute dissolved in this solvent.Which curve is the solvent and what happens to the vapor pressure when the solute is dissolved in the solvent?A) Curve (a) is the solvent and the vapor pressure decreases.B) Curve (a) is the solvent and the vapor pressure increases.C) Curve (b) is the solvent and the vapor pressure decreases.D) Curve (b) is the solvent and the vapor pressure increases.
Q:
Drawings (1) and (2) show the equilibrium vapor pressures of two pure liquids. Which drawing (3)-(6) represents the equilibrium vapor pressure of a solution made by mixing equal moles of each liquid?A) drawing (3)B) drawing (4)C) drawing (5)D) drawing (6)
Q:
Drawing (1) shows the equilibrium vapor pressure of a pure liquid. Which drawing (2)-(5) represents the equilibrium vapor pressure when a nonvolatile solute is dissolved in the liquid? A) drawing (2)
B) drawing (3)
C) drawing (4)
D) drawing (5)
Q:
Drawing (1) shows a system in which an equilibrium exists between dissolved and undissolved gas particles at P = 1 atm. According to Henry's law, if the pressure is decreased to 0.5 atm and equilibrium is restored, which drawing (2)-(5) best represents the equilibrium at 0.5 atm? A) drawing (2)
B) drawing (3)
C) drawing (4)
D) drawing (5)
Q:
Drawing (1) shows a system in which an equilibrium exists between dissolved and undissolved gas particles at P = 1 atm. According to Henry's law, if the pressure is increased to 2 atm and equilibrium is restored, which drawing (2)-(5) best represents the equilibrium at 2 atm? A) drawing (2)
B) drawing (3)
C) drawing (4)
D) drawing (5)
Q:
Which ion-dipole interaction results in the larger (more negative) hydration energy? A) diagram (a)
B) diagram (b)
C) diagram (c)
D) diagram (d)
Q:
Which ion-dipole interaction results in the larger (more negative) hydration energy? A) diagram (a)
B) diagram (b)
C) diagram (c)
D) diagram (d)
Q:
Arrows in the energy diagram below represent enthalpy changes occurring in the endothermic formation of a solution:Hsoln = enthalpy of solutionHsolute-solute = enthalpy change involving solute-solute interactionsHsolute-solvent = enthalpy change involving solute-solvent interactionsHsolvent-solvent = enthalpy change involving solvent-solvent interactionsWhich arrow represents Hsoln?A) arrow (a)B) arrow (b)C) arrow (c)D) arrow (d)
Q:
Which arrows represent Hsolute-solute and Hsolvent-solvent?A) arrow (a) and arrow (b)B) arrow (a) and arrow (c)C) arrow (a) and arrow (d)D) arrow (c) and arrow (d)
Q:
Which arrow represents Hsolute-solvent?A) arrow (a)B) arrow (b)C) arrow (c)D) arrow (d)
Q:
Arrows in the energy diagram below represent enthalpy changes occurring in the exothermic formation of a solution:Hsoln = enthalpy of solutionHsolute-solute = enthalpy change involving solute-solute interactionsHsolute-solvent = enthalpy change involving solute-solvent interactionsHsolvent-solvent = enthalpy change involving solvent-solvent interactionsWhich arrow represents Hsoln?A) arrow (a)B) arrow (b)C) arrow (c)D) arrow (d)
Q:
Which drawing above represents the system with the second highest entropy?A) drawing (a)B) drawing (b)C) drawing (c)D) drawing (d)
Q:
Which drawing above represents the system with the second lowest entropy?
A) drawing (a)
B) drawing (b)
C) drawing (c)
D) drawing (d)
Q:
Which drawing above represents the system with the lowest entropy?
A) drawing (a)
B) drawing (b)
C) drawing (c)
D) drawing (d)
Q:
Which drawing above represents the system with the highest entropy?A) drawing (a)B) drawing (b)C) drawing (c)D) drawing (d)
Q:
A solution of 62.4 g of insulin in enough water to make 1.000 L of solution has an osmotic pressure of 0.305 atm at 25C. Based on these data, what is the molar mass of insulin?A) 621 g/molB) 5000 g/molC) 7570 g/molD) 71,900 g/mol
Q:
Which of the intermolecular forces is the most important contributor to the high surface tension shown by water?
A) dipole-dipole forces
B) dispersion forces
C) hydrogen bonding
D) ion-dipole forces
Q:
When a narrow diameter glass tube is inserted into a body of water, water rises in the tube and its surface inside is concave upwards. Which statement, concerning the strength of the intermolecular forces between glass and water molecules compared to those between water molecules, is accurate?
A) The forces of attraction between the glass and water are weaker than those in water.
B) The forces of attraction between the glass and water are stronger than those in water.
C) The forces of attraction between the glass and water are the same as those in water.
D) Intermolecular forces are irrelevant to this situation.
Q:
In liquid methanol,
CH3OH
which intermolecular forces are present?
A) Dispersion, hydrogen bonding and dipole-dipole forces are present.
B) Only dipole-dipole and ion-dipole forces are present.
C) Only dispersion and dipole-dipole forces are present.
D) Only hydrogen bonding forces are present.
Q:
Which of the following compounds exhibits only dipole-dipole intermolecular interactions?
A) N2
B) HBr
C) CO2
D) H2O
Q:
Which substance in each of the following pairs is expected to have the larger dispersion forces? A) Br2 in set I and n-butane in set II
B) Br2 in set I and isobutane in set II
C) I2 in set I and n-butane in set II
D) I2 in set I and isobutane in set II
Q:
Which is expected to have the largest dispersion forces?
A) C2H6
B) C8H18
C) N2
D) CO2
Q:
Which of the following exhibits ion-dipole forces?
A) NaCl(s)
B) NaCl(aq)
C) Na(s)
D) Cl2(g)
Q:
Which of the following exhibits hydrogen bonding?
A) OH
B) O
C) D) HCN
Q:
Which of the following compounds exhibits hydrogen bonding?
A) CH3Cl
B) HI
C) H3C-O-CH3
D) NH3
Q:
Which of the following does not exhibit hydrogen bonding?
A) B) C) HF
D) HOCOH
Q:
Which has the smallest dipole-dipole forces?
A) CH3F
B) HCl
C) N2
D) CO
Q:
AgCl is found to have 78.1% ionic character, and its gas phase dipole moment is 11.5 D. What is the distance between the Ag and Cl atoms in gaseous AgCl?
A) 9.19 x 10-10 pm
B) 14.7 pm
C) 307 pm
D) 903 pm
Q:
The dipole moment of BrF is 1.29 D, and its bond length is 178 pm. What is the percent ionic character of the Br-F bond?
A) 3.9%
B) 8.5%
C) 15%
D) 33%
Q:
The dipole moment of ClF is 0.88 D, and its bond length is 163 pm. What is the percent ionic character of the Cl-F bond?
A) 0.54%
B) 7.8%
C) 11%
D) 25%
Q:
Which of the following should have the largest dipole moment?
A) H2(g)
B) CO2(g)
C) KCl(g)
D) CH3F(g)
Q:
Which of the following molecules does not have a dipole moment?
A) CH2=CH2
B) NH3
C) CH3NH2
D) HCl
Q:
Which has a dipole moment?A) CO2B) CO32-C) SO2D) SO42-
Q:
The bonds in the polyatomic ion CO32- are classified asA) ionic.B) metallic.C) nonpolar covalent.D) polar covalent.
Q:
Ni has a face-centered unit cell. The number of Ni atoms in the unit cell is ________.
Q:
The solids formed by K, K2O2, SiO2, and O2 are classified as ________, ________, ________, and ________, respectively.
Q:
Of C2H5OH and C3H5(OH)3 the one expected to have the higher vapor pressure is ________, and the one expected to have the higher boiling point is ________.
Q:
The phase change H2(g) -> H2(s) is called ________, and the enthalpy change, H, for this phase change has a ________ sign.
Q:
Of C2H5OH and C3H5(OH)3 the one expected to have the higher viscosity is ________, and the one expected to have the higher surface tension is ________.
Q:
Helium can be liquefied when He atoms are attracted to one another by intermolecular ________ forces.
Q:
The intermolecular forces responsible for CH3CH2OH being at liquid at 20C are ________ bonds.
Q:
The intermolecular forces formed when NaCl is dissolved in water are ________ forces.
Q:
In the molecule BF3 there is a + charge on the ________ atom and a - charge on the ________ atom.
Q:
The bonds in the polyatomic ion NO3- are classified as
Q:
How many H- ions are around each Na+ ion in NaH, which has a cubic unit cell with H- ions on each corner and each face?A) 1B) 4C) 6D) 8
Q:
NaCl crystallizes in a cubic unit cell with Cl- ions on each corner and each face. How many Na+ and Cl- ions are in each unit cell of NaCl?
A) 1 Na+ ion and 1 Cl- ion
B) 2 Na+ ions and 2 Cl- ions
C) 4 Na+ ions and 4 Cl- ions
D) 8 Na+ ions and 8 Cl- ions
Q:
Lithium crystallizes in a body-centered cubic structure. What is the coordination number of each atom?
A) 4
B) 6
C) 8
D) 12
Q:
Cesium has a radius of 272 pm and crystallizes in a body-centered cubic structure. What is the edge length of the unit cell?
A) 314 pm
B) 385 pm
C) 544 pm
D) 628 pm
Q:
A certain metal crystallizes in a face-centered cubic structure. What is the edge length of the unit cell if the atomic radius of the metal is 144 pm?
A) 204 pm
B) 288 pm
C) 333 pm
D) 407 pm
Q:
Nickel has a face-centered cubic structure and has a density of 8.90 g/cm3. What is its atomic radius?
A) 125 pm
B) 249 pm
C) 353 pm
D) 997 pm
Q:
What is the edge length of a face-centered cubic unit cell made up of atoms having a radius of 128 pm?
A) 181 pm
B) 362 pm
C) 512 pm
D) 1020 pm