IDEAL GAS LAW WORKSHEET 3RD QUARTER 2013-2014

Ideal Gas Law Problems

1)         If I have 4 moles of a gas at a pressure of 5.6 atm and a volume of 12 liters, what is the temperature?

204.6 K

2)         If I have an unknown quantity of gas at a pressure of 1.2 atm, a volume of 31 liters, and a temperature of 87 ⁰C, how many moles of gas do I have?

1.25 mol

3)         If I contain 3 moles of gas in a container with a volume of 60 liters and at a temperature of 400 K, what is the pressure inside the container?

1.642 atm

4)         If I have 7.7 moles of gas at a pressure of 0.09 atm and at a temperature of 56 ⁰C, what is the volume of the container that the gas is in?

2310 L

5)         If I have 17 moles of gas at a temperature of 67 ⁰C, and a volume of 88.89 liters, what is the pressure of the gas?

5.3 atm

 

6)         If I have an unknown quantity of gas at a pressure of 0.5 atm, a volume of 25 liters, and a temperature of 300 K, how many moles of gas do I have?

0.5 mol 

 

7)         If I have 21 moles of gas held at a pressure of 78 atm and a temperature of 900 K, what is the volume of the gas?

19.89 L

8)         If I have 1.9 moles of gas held at a pressure of 5 atm and in a container with a volume of 50 liters, what is the temperature of the gas?

1602 K

9)         If I have 2.4 moles of gas held at a temperature of 97 ⁰C and in a container with a volume of 45 liters, what is the pressure of the gas?

1.62 atm

10)       If I have an unknown quantity of gas held at a temperature of 1195 K in a container with a volume of 25 liters and a pressure of 560 atm, how many moles of gas do I have?

142 mol

11)       If I have 0.275 moles of gas at a temperature of 75 K and a pressure of 1.75 atmospheres, what is the volume of the gas?

.96 L

12)       If I have 72 liters of gas held at a pressure of 3.4 atm and a temperature of 225 K, how many moles of gas do I have?

13.25L

COMBINED GAS LAW WORKSHEET 3RD QUARTER 2013-2014

Combined Gas Law Problems

1)         If I initially have a gas at a pressure of 12 atm, a volume of 23 liters, and a temperature of 200 K, and then I raise the pressure to 14 atm and increase the temperature to 300 K, what is the new volume of the gas?

29.57 L

2)         A gas takes up a volume of 17 liters, has a pressure of 2.3 atm, and a temperature of 299 K.  If I raise the temperature to 350 K and lower the pressure to 1.5 atm, what is the new volume of the gas?

30.5 L

3)         A gas that has a volume of 28 liters, a temperature of 45 ⁰C, and an unknown pressure has its volume increased to 34 liters and its temperature decreased to 35 ⁰C.  If I measure the pressure after the change to be 2.0 atm, what was the original pressure of the gas?

2.5 atm

4)         A gas has a temperature of 14 ⁰C, and a volume of 4.5 liters.  If the temperature is raised to 29 ⁰C and the pressure is not changed, what is the new volume of the gas?

4.7 L

5)         If I have 17 liters of gas at a temperature of 67 ⁰C and a pressure of 88.89 atm, what will be the pressure of the gas if I raise the temperature to 94 ⁰C and decrease the volume to 12 liters?

135.9 atm

6)         I have an unknown volume of gas at a pressure of 0.5 atm and a temperature of 325 K.  If I raise the pressure to 1.2 atm, decrease the temperature to 320 K, and measure the final volume to be 48 liters, what was the initial volume of the gas?

117 L

7)         If I have 21 liters of gas held at a pressure of 78 atm and a temperature of 900 K, what will be the volume of the gas if I decrease the pressure to 45 atm and decrease the temperature to 750 K?

30.33 L

 

8)         If I have 2.9 L of gas at a pressure of 5 atm and a temperature of 50 ⁰C, what will be the temperature of the gas if I decrease the volume of the gas to 2.4 L and decrease the pressure to 3 atm?

160 K

9)         I have an unknown volume of gas held at a temperature of 115 K in a container with a pressure of 60 atm.  If by increasing the temperature to 225 K and decreasing the pressure to 30 atm causes the volume of the gas to be 29 liters, how many liters of gas did I start with?

7.41 L

GAY-LUSAC'S LAW WORKSHEET 3RD QUARTER 2013-2014

Gay-Lussac's Law

1.  Determine the pressure change when a constant volume of gas at 1.00 atm is heated from 20.0 °C to 30.0 °C.

1.03 atm

2.  A gas has a pressure of 0.370 atm at 50.0 °C. What is the pressure at standard temperature?

0.313 atm

3.  A gas has a pressure of 699.0 mm Hg at 40.0 °C. What is the temperature at standard pressure?

340.3 K

4.  If a gas is cooled from 323.0 K to 273.15 K and the volume is kept constant what final pressure would result if the original pressure was 750.0 mm Hg?

634 mm Hg

5.  If a gas in a closed container is pressurized from 15.0 atmospheres to 16.0 atmospheres and its original temperature was 25.0 °C, what would the final temperature of the gas be?

317.9 K

6. A 30.0 L sample of nitrogen inside a rigid, metal container at 20.0 °C is placed inside an oven whose temperature is 50.0 °C. The pressure inside the container at 20.0 °C was at 3.00 atm. What is the pressure of the nitrogen after its temperature is increased?

3.3 atm

7. A sample of gas at 3.00 x 10³ mm Hg inside a steel tank is cooled from 500.0 °C to 0.00°C. What is the final pressure of the gas in the steel tank?

105.9 mm Hg

8.  The temperature of a sample of gas in a steel container at 30.0 kPa (kilopascal) is increased from -100.0 °C to 1.00 x 10³ °C. What is the final pressure inside the tank?

220.8 kPa

9. Calculate the final pressure inside a scuba tank after it cools from 1.00 x 10³ °C to 25.0°C. The initial pressure in the tank is 130.0 atm.

30 atm

CHARLES LAW WORKSHEET 3RD QUARTER S.Y. 2013-2014

Charles’s Law Problems

1) A container holds 50.0 mL of nitrogen at 25° C and a pressure of 736 mm Hg.
What will be its volume if the temperature increases by 35° C?

2) A sample of oxygen occupies a volume of 160 dm3 at 91° C. What will be
volume of oxygen when the temperature drops to 0.00° C?

3) A sample of hydrogen has an initial temperature of 50.° C. When the
temperature is lowered to -5.0° C, the volume of hydrogen becomes
212 cm3. What was the initial volume of the hydrogen in mL?

4) 568 cm3 of chlorine at 25° C will occupy what volume at -25° C while the
pressure remains constant?

5) A sample of helium has a volume of 521 dm3 at a pressure of 75 cm Hg and
a temperature of 18° C. When the temperature is increased to 23° C, what is
the volume of the helium?.

Answers:

55.9 mL N2

120 dm3 O2

2.56 cm3 H2

473 cm3 Cl2

530. dm3 He

BOYLE'S LAW WORKSHEETS 3RD QUARTER S.Y. 2013-2014

1. To compress nitrogen at 1 atm from 750 mL to 500 mL, what must the new pressure be  if the temperature is kept constant?
2.  If oxygen at 128 kPa is allowed to expand at constant temperature until its pressure is 101.3 kPa, how much larger will the volume become?
3. A sample of nitrogen at 101.3 kPa with a volume of 100 mL is carefully compressed at constant temperature in successive changes in pressure, equalling 5 kPa at a time, until the final pressure is 133.3 kPa. Calculate the new volume.
4. A sample of nitrogen at a constant temperature of 20^oC was compressed from 300 mL to 0.360 mL and its new pressure was found to be 400.0 Pa. What was the original pressure in  kPa?
5. The pressure on 6.0 L of a gas is 200 kPa. What will be the volume if the pressure is doubled, keeping the temperature constant? 

ANSWERS: 1.5 atm, 1.26 times larger, 75.99 mL, 0.48 Pa, 3.0 L

S.Y. 2013-2014: Chemical Bonding

1) There are __________ paired and __________ unpaired electrons in the Lewis symbol for a phosphorus atom.

A) 4, 2

B) 2, 4

C) 2, 3

D) 4, 3

E) 0, 3 

 

2) In the Lewis symbol for a fluorine atom, there are __________ paired and __________ unpaired electrons.

A) 4, 2

B) 4,1

C) 2, 5

D) 6, 1

E) 0, 5 

 

3) The halogens, alkali metals, and alkaline earth metals have __________ valence electrons, respectively.

A) 7, 4, and 6

B) 1, 5, and 7

C) 8, 2, and 3

D) 7, 1, and 2

E) 2, 7, and 4 

4) The only noble gas without eight valence electrons is __________.

A) Ar

B) Ne

C) He

D) Kr

E) All noble gases have eight valence electrons.

5) Which of the following would have to lose two electrons in order to achieve a noble gas electron configuration?

             O        Sr        Na        Se        Br

A) O, Se

B) Sr

C) Na

D) Br

E) Sr, O, Se

6) Elements from opposite sides of the periodic table tend to form __________.

A) covalent compounds

B) ionic compounds

C) compounds that are gaseous at room temperature

D) homonuclear diatomic compounds

E) covalent compounds that are gaseous at room temperature

7) How many single covalent bonds must a silicon atom form to have a complete octet in its valence shell?

A) 3

B) 4

C) 1

D) 2

E) 0

8) What is the maximum number of double bonds that a hydrogen atom can form?

A) 0

B) 1

C) 2

D) 3

E) 4

9) The ability of an atom in a molecule to attract electrons is best quantified by the __________.

A) paramagnetism

B) diamagnetism

C) electronegativity

D) electron change-to-mass ratio

E) first ionization potential

10) Electronegativity __________ from left to right within a period and __________ from top to bottom within a group.

A) decreases, increases

B) increases, increases

C) increases, decreases

D) stays the same, increases

E) increases, stays the same

11) The type of compound that is most likely to contain a covalent bond is __________.

A) one that is composed of a metal from the far left of the periodic table and a nonmetal from the far right of the periodic table

B) a solid metal

C) one that is composed of only nonmetals

D) held together by the electrostatic forces between oppositely charged ions

E) There is no general rule to predict covalency in bonds.

12) Of the atoms below, __________ is the most electronegative.

A) Br

B) O

C) Cl

D) N

E) F

13) Of the atoms below, __________ is the least electronegative.

A) Rb

B) F

C) Si

D) Cl

E) Ca

14) Which of the following names is/are correct for the compound TiO2?

A) titanium dioxide and titanium (IV) oxide

B) titanium (IV) dioxide

C) titanium oxide

D) titanium oxide and titanium (IV) dioxide

E) titanium (II) oxide

15) The Lewis structure of N2H2 shows __________.

A) a nitrogen-nitrogen triple bond

B) a nitrogen-nitrogen single bond

C) each nitrogen has one nonbonding electron pair

D) each nitrogen has two nonbonding electron pairs

E) each hydrogen has one nonbonding electron pair

Answers: cddcb   bbacc   ceaac