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Work sheet (1) Chapter (12+13)
Subject
Name
Date
Grade
11
Cluster
Chemistry
HST/ES
Q1-Choose the best answer:
1.
a.
b.
c.
d.
The SI unit of pressure is :
Newton
Kelvin
Liter
Pascal
2. Measure of the kinetic energy of all particles in a gaseous sample is :
a. Temperature
b. Pressure
c. Volume
d. Mass
3. Which of the following is an intramolecular force ?
a. Hydrogen bond
b. Dipole-dipole bond
c. Ionic bond
d. London dispersion force
4. Which gas/es will diffuse faster than Carbon dioxide gas ( CO2 ) ?
a. Oxygen gas
b. Chlorine gas ( Cl2 )
c. Hydrogen gas
d. a and c will diffuse faster than CO2
5. Which of the following has same kind of intermolecular force as in water ( H2O ) ?
a. Hydrofluoric acid ( HF )
b. Nitrogen dioxide gas ( NO2 )
2
c. Carbon dioxide ( CO2 )
d. Argon ( Ar )
6. At STP , the temperature is ____________ and the pressure is _______
A. 0.00oC , 1 KPa
B. 0K , 1 atm
C. 0.00oC , 1atm
D. -273oC, 1 atm
7. Which of the following shows the relation between temperature and pressure at constant
volume ?
a. Boyle’s law
b. Charle’s law
c. Gay-Lussac’s law
d. Henry’s law .
8. The value of the ideal gas law constant R in ( PV=nRT) is __________________
a. 22.4 atm.L/mol.K
b. 1 mol .K/atm.L
c. 0.082 atm.L/mol.K
d. 273 K/L
9. Use the manometer below to find the pressure in mmHg .
a. 1000mmHg
b. 650 mmHg
c. 760 mmHg
d. 320mmHg
10. A solution was prepared by dissolving carbon dioxide gas in water . Which of the following
conditions gives the highest concentration ?
a. 20 Kpa and 20 oC
b. 13 Kpa and 20 oC
c. 8 Kpa and 20 oC
d. 11 Kpa and 20 oC
11. Which of the following solutions has the highest boiling point ?
a. 2 m
NaCl solution
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b. 2.5 m KCl solution
c. 4 m
LiCl solution
d. 3 m NaCl solution
12. Which of the following describe/s a colloid?
a- Particles scatter the light .
b- Particles are smaller in size than suspensions’ particles.
c- Particles move in Brownian motion to prevent them from settling down .
d- All of the above
13. The measure of how much solute is dissolved in a specific amount of the solvent is __________
a. Boiling point elevation .
b. Concentration
c. Dilution
d. Mass.
14. What is the percent by volume of a solution made by adding 20.0ml of methanol in 160.0 ml of
water ?
a. 11.11%
b. 12.5%
c. 0.11%
d. 0.125%
15. What mass of solvent is needed to dissolve 120.0g of CaCO3 to prepare a solution of 13% by
mass ?
a. 100 g
b. 308.7 g
c. 803.08g
d. 13g
16. The density of carbon dioxide gas at STP is ________ .
a. 1.97 g/L
b. 0.508 g/L
c. 0.082 g/L
d. 1.97 g/ml
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Use the graph below to answer the questions (17-19)
17.Which law describes the graph ?
a.
b.
c.
d.
Boyle’s law
Gay-Lusacc’s law
Charle’s law
No enough data
18. What is the volume when the temperature is 400K ?
a. 300 ml
b. 400 L
c. 400 ml
d. 100 ml
19. Which of the following is true at the volume of zero?
a. Temperature is the absolute zero and pressure is 1atm
b. Temperature is the absolute zero and the pressure is zero .
c. Temperature is the highest and pressure is the lowest .
d. Temperature is the absolute zero and pressure is the highest .
20. A sample of oxygen gas ( O2),hydrogen gas ( H2 ).What is the ratio of diffusion of oxygen gas to
hydrogen gas?
a. 0.25
b. 4
c. 32
d. 1
21.What is the mol fraction of HCl in an aqueous solution that has 21.7g HCl and 78.3g of water ?
a.
b.
c.
d.
12
0.0012
8.333
0.120
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22.According to Avogadro’s principle, equal volumes of gases at the same temperature and
pressure contain_________ numbers of particles.
a.
b.
c.
d.
Different
Small
Equal
Large
23.Which of the following increase/s the solvation ?
a.
b.
c.
d.
Agitation
Increase the temperature
Increase the surface area of the solute .
All the above factors affect the salvation .
24. Which of the following describe/s a supersaturated solution ?
a. It contains more dissolved solute particles that the saturated solution .
b. It can be made by adding more solute particles at high temperature then cooling the
saturated solution .
c. It contains more solvent particles than the saturated solution .
d. a and b
25. Suspensions are :
a.
b.
c.
d.
Heterogenous mixtures containing particles settle out if left undisturbed.
Homogenous mixtures containing particles settle out if left undisturbed.
Heterogenous mixtures containing particles that don’t settle down under any condition.
Heterogenous mixtures that have smaller particles than colloids.
26. When two liquids mix together but separate shortly after, then these liquids are _______:
a.
b.
c.
d.
miscible
immiscible
soluble
insoluble
27. All of the following describe the ideal gas particles except :
a.
b.
c.
d.
Particles colloid the container and each other elastically .
Particles move in constant and random motion .
Particles don’t take up space .
Particles experience attraction or repulsion forces between the particles.
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28.The molar volume of any gas at STP is :
a.
b.
c.
d.
24.2
22.4
22.4
2.24
L
mL
L
L
29. Which of the following states that equal volumes of gases at the same temperature and pressure
contain the same number of particles?
a.
b.
c.
d.
Charle’s law
Gay lussac’s law
Boyle’s law
Avogadro’s principal
30.Which intermolecular force depends on the formation of temporary dipoles?
a.
b.
c.
d.
London dispersion force
Hydrogen bond
Dipole-dipole bond
Ionic bond .
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31.How does the density of the gas change by moving from
A
a.
b.
c.
d.
B to A ( compression )?
B
C
Density increases
Density decreases
Density does not change by compressing
No enough data .
32. The pressure of a sample of helium in a 1.0-L container is 0.857 atm. What is the new pressure if the
sample is placed in a 0.5-L container? (Assume the temperature is constant.)
a. 0.143 atm
b. 0.429 atm
c. 1.38 atm
d. 1.71 atm
33. The theory that describes the behavior of gases in terms of the motion of gas particles is _____
a. the theory of intermolecular forces
b. Graham's law of effusion
c. Dalton's law of partial pressure
d. the kinetic-molecular theory
34. A device that is used to measure atmospheric pressure is a___________:
a. Barometer
b. Thermometer
c. Spring balance
d. Balance
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Question Two :
Solve the following
35. If 60 g of a gas dissolves in 1.0 L of water at 27KPa what will be the solubility of this gas
at 100KPa?
36. A mixture of nitrogen gas , carbon monoxide gas and hydrogen gas at atmospheric
pressure . If the partial pressure of nitrogen is 100 atm and 350 atm for hydrogen gas .
What is the partial pressure of carbon monoxide gas in this mixture?
37. An aqueous solution of sodium hydroxide ( NaOH ) was prepared by dissolving 11g of
the solute (NaOH) in 900 ml water .
a. What is the molarity of this solution ?
b. What will be the new concentration ( molar ) if this solution was diluted to a
volume of 1.3L ?
38. What are the boiling point and the freezing points of 0.35 m of sucrose in ethanol ?
(Kf=1.99 C/m , Kb=1.22C/m , boiling point = 78.5oC , Freezing point = -114.1oC) .
39. The pressure in a tire is 1.5 atm at 30oC , what will be the temperature in Celsius if the
pressure increases to 4.7 atm?
40. What is the ratio of diffusion between gas A and B . If the molar mass of gas A is 3 times
the molar mass of B ?
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41. A gas at 115 kPa and 310K fills a fixable container with an initial volume of 2.5 L. If
the temperature is raised to 358 K and the pressure increases to 410KPa, what is
the new volume?
42. If the pressure exerted by a gas at 30oC in a volume of 0.13L is 0.12KPa .How many
moles of the gas are present?
43. In the reaction ( N2(g) +H2(g)
NH3(g) ) if 4.8L of nitrogen gas react
completely with Hydrogen gas at a pressure of 3.8atm and temperature of 301K .a.
a. Find the volume of ammonia produced?
b. What is the mass of ammonia NH3 produced?
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Question three:
Answer the following questions .
44. List four colligative properties of a solution .
__________________________________________________________________
__________________________________________________________________
45. Explain why a solution has a higher boiling point than that of the pure solvent.
_________________________________________________________________________________________
46. Explain the effect of temperature and pressure on the solubility of gases.
_____________________________________________________________________________________
______________________________________________________________________________________
47.List the three basic assumptions of the kinetic-molecular theory.
_______________________________________________________
_______________________________________________________
48.Explain what determines a substance’s state at a given temperature.
____________________________________________________________________