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WorksheetsSummative Test
Total questions: 30
Worksheet time: 4hrs 10mins
Which of the following schematic drawings best describes a solution of Li2SO4 in water?
Butanol has higher boiling point but lower vapor pressure compared to ethanol. What causes this?
Butanol is polar and therefore has higher IMFA compared to the nonpolar ethanol.
Butanol and ethanol are both nonpolar but the former has lower IMFA compared to the latter.
Ethanol is polar making it asymmetrical and has high VP but low in BP compared to the other alcohol – butanol.
Ethanol and butanol are both nonpolar but the latter has higher molar mass making it higher in IMFA in comparison to the former alcohol.
What is the existing IMFA in the first diagram (i)?
London force
Dipole-dipole
H-bond
Dispersion
Which has the higher IMFA, molecule (i) or the compound (iv) and why?
Molecule (iv) has the higher IMFA since it has dipole-dipole interaction.
The latter molecule has the higher IMFA since it has H-bond.
The compound (i) is polar therefore it has higher intermolecular force compared to the latter molecule.
The molecule (i) has H-bond and is stronger compared to the IMFA of the latter molecule.
The molecules - propanol and ethyl methyl ether have the same molecular formula of C3H8O but different in terms of boiling point. Why do you think so?
Propanol is a polar molecule while ethyl methyl ether is nonpolar which makes the latter high in terms of boiling point.
Propanol has larger dispersion interaction compared to the ether compound.
Ethyl methyl ether has dipole-dipole force while propanol has the London force which makes the latter higher in boiling point.
Ethyl methyl alcohol has dipole-dipole force while propanol has the H-bond making the former compound lower in boiling point due to the lower IMFA.
The point 1 in diagram the shows what?
Sublimation point
Critical point
Triple point
Supercritical point
At STP, in what state do you think the substance would exist?
Supercritical
Gas
Liquid
Solid
Holding the prevailing pressure at constant, what do you think would happen to the substance as it is heated?
Melt then evaporate
Sublime
Condense then crystallize
Solidify
Arrange the following compounds in increasing vapor pressure:
MgCl2, CH3F, CH3OH and H2O
CH3OH, MgCl2, H2O, CH3F
CH3F, CH3OH, H2O, MgCl2
MgCl2, H2O, CH3OH, CH3F
CH3OH, H2O, CH3F, MgCl2
The DNA double helix at the atomic level looks like a twisted ladder, where the “rungs” of the ladder consist of molecules that are hydrogen-bonded together. Shown on the right are the structures of the adenine-thymine (AT) “base pair” and the guanine-cytosine (GC) base pair. Which base pair is more stable to heating? Why?
The AT pair is more stable to heating since it has higher IMFA.
The GC pair is less stable to heating since it has weak IMFA.
The AT pair is less stable because it has one H-bond pair that could easily be broken.
The GC pair is more stable to heating because of the presence of three H-bonds that won’t be easily broken.
Which of the following does not belong to the group?
steel
baking soda
groundwater
air
Dirty ice cream was made possible because of the application of what colligative property?
Osmotic pressure
Vapor pressure lowering
Boiling point elevation
Freezing point depression
How would you compare the boiling point elevation of 1 mol NaCl to 1 mol of sucrose (C12H22O11) in aqeous solution?
The boiling point elevation of 1 mol NaCl is the same with the boiling point resultant of 1 mol sucrose.
One mol of sugar has higher boiling point elevation since it is molecular solid compared to the NaCl which is ionic solid.
The boiling point elevation of 1 mol NaCl is higher compared to one mol of sucrose since the former has higher concentration due to the dissociation of the compound to 2 mol of solute particles.
The boiling point elevation of 1 mol sucrose is higher compared to the former compound since one molecule of sucrose could dissociates into 12 C ions, 22 H ions and 11 O ions when it is dissolved in water.
What type of crystalline solid is B2H6 based on the data given?
Metallic
Ionic
Molecular
Network
What type of crystalline solid is CsI based on the data given?
Network
Molecular
Metallic
Ionic
A solution was prepared by dissolving 28.8 g of ferric chloride and 100. g water at 20 0C The density of the pure water and solution at this temperature is 0.998 g/mL and 1.28 g/mL respectively.
Calculate the % mass of solution.
22.3%
22.4%
21.3%
21.4%
A solution was prepared by dissolving 28.8 g of ferric chloride and 100. g water at 20 0C The density of the pure water and solution at this temperature is 0.998 g/mL and 1.28 g/mL respectively.
What is the concentration of the solution in molality?
1.78 m
1.79 m
1.78 M
1.79 M
A solution was prepared by dissolving 28.8 g of ferric chloride and 100. g water at 20 0C The density of the pure water and solution at this temperature is 0.998 g/mL and 1.28 g/mL respectively.
What is the mole fraction of the solvent?
0.968
0.967
0.969
0.966
Calculate the mass of solid AgCl that is produced when 600. mL of 0.500 M FeCl3 is used with excess Ag2SO4 solution.
Ag2SO4 + FeCl3 → Fe2(SO4)3 + AgCl
128.7 g AgCl
129 g AgCl
128 g AgCl
129.0 g AgCl
What volume of 0.25 M FeCl3 is needed to react completely with 450 mL of 0.75 M Ag2SO4?
Ag2SO4 + FeCl3 → Fe2(SO4)3 + AgCl
0.92 L FeCl3
0.90 L FeCl3
0.91 L FeCl3
0.93 L FeCl3
List the following aqueous solutions in order of increasing boiling point: 0.120 m glucose, 0.050 m LiBr, 0.050 m Zn(NO3)2 and 0.015 m of CaCl2
0.015 m of CaCl2, 0.050 m LiBr, 0.120 m glucose, 0.050 m Zn(NO3)2
0.120 m glucose, 0.050 m LiBr, 0.015 m of CaCl2 , 0.050 m Zn(NO3)2
0.050 m LiBr, 0.120 m glucose, 0.050 m Zn(NO3)2 , 0.015 m of CaCl2
0.050 m Zn(NO3)2, 0.120 m glucose, 0.050 m LiBr, 0.015 m of CaCl2
Calculate the vapor pressure of water above a solution prepared by adding 22.5 g of lactose (C12H22O11) to 200.0 g of water at 338 K. (P0 at 338 K is 187.5 torr)
186.3 torr
186.4 torr
185.3 torr
185.4 torr
Camphor (C10H16O) melts at 1790C and it has a particularly freezing point depression constant, Kf = 40.00C/m. When 0.186 g of an organic compound substance of unknown molar mass is dissolved in 22.01 g of liquid camphor the freezing point of the mixture is to be found -176.70C. What is the molar mass of the solute?
0.0973 g/mol
1.90 g/mol
0.972 g/mol
1.91 g/mol
If I leave 950. mL of 0.75 M calcium chloride solution uncovered on a windowsill and 250. ml of the solvent evaporates, what will be the new concentration of the calcium chloride?
2.0 M
1.01 M
1.02 M
1.0 M
What is the osmotic pressure formed by dissolving 44.2 mg of aspirin (C9H8O4) in 0.358 L of water at 250C?
0.168 atm
0.0167 atm
0.169 atm
0.0168 atm
BONUS QUESTION
Module one of General Chemistry 2 is all about what?
Kinetic Molecular Model of Solids and Liquids
Phase Diagram and Phase Changes
Intermolecular Forces of Attraction
Colligative Properties
Which of the following does not belong to the group?
Snowflakes
Dry ice
Diamond
Crystalline glass
What do you call to the properties that are dependent on the amount of the solute particles and not affected by the substances' nature and chemical identity?
Collative properties
IMFA properties
Colligative properties
Chemical nature
Which of the following has the highest kinetic energy in its individualized particles?
Chair
Oobleck
air
oil
What particular model is used to describe the properties of solid, liquid and gas?
Elementary Molecular Model
Quantum mechanics model
Kinetic Molecular Model
Electron cloud model
