Grade 11 Core Chemistry

Section; 13.1,13.2;13.3

1. A milkshake is sipped through a straw at the noted pressure. The straw contains 5.0 mL of liquid. How much liquid is consumed at 0.092 atm?

A 6.3 mL

B 3.9 mL

C 0.10 mL

D 7.8 mL

2. The volume of a sample of helium is 4.5 mL at 20.0°C and 203.0 kPa. What will its volume be in the figure?

A 6.85 mL

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B 3.78 mL

C 4.34 mL D 34.4 ml

1. If the volume of a fixed amount of gas is 10 L at 100 K, then its volume will be___________ at 200 K, assuming the pressure does not change

A 5L

B 20L

C 10L

D 15L

4. Absolute zero is the lowest possible theoretical temperature which equals

A. 0°C

B. 273°C

C.--

273°C

D. 0 F

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6. If two variables are inversely proportional, what happens to the value of one as the value of the other increases?

A. Increases

B. Decreases

C. Increases then decreases

D. Stay the same

7. A balloon is filled with 3.50 L of water at 24.0°C and 2.27 atm. The balloon in the figure is placed outside on a hot day, what is the volume of the balloon (assuming constant pressure)?

A 3.38 L

B 2.47 L

C 8.19 L

D 3.62 L

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8. Gas is confined in a metal tank in the figure. At 20.20C, the gas exerts a pressure of 8.532 atm. After heating the tank, the pressure of the gas increases to 10.406 atm. What is the temperature of the heated gas?

A 24.630C

B 84.590C

C 92.640C

D 32.600C

9. What principle is illustrated in the figure? ( weather balloon )

A Boyle’s Law

B Ideal Gas Law

C Gaylu-ssac’s lawD Charles’s Law

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10. A given mass of gas in a rigid container is heated from 100°C to 500°C. Which of the following responses best describes what will happen?

A The pressure will decrease by a factor of five.

B The pressure will increase by a factor of five

C The pressure will increase by a factor of about two

D The pressure will increase by a factor of about twenty-five

11.A given mass of gas in a rigid container is heated from 100K to 500K. Which of the following responses best describes what will happen?

A The pressure will decrease by a factor of five

B The pressure will increase by a factor of five

C The pressure will increase by a factor of about two

D The pressure will increase by a factor of about twenty-five

12. A 0.5L container of nitrogen gas at 18 degrees Celsius is heated under constant pressure to the boiling point of water. What is its new volume?

A 0.5 L

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B 0.568

C 0.641 L

D 0.728

13. One atmosphere is equal to a pressure of _____

A 76 mm Hg

B 101.3 kPa

C 706 torr.

D 670mmHg

14. The _____ in a balanced equation specify volume ratios for gaseous

reactants and products.

A constants

B coefficients

C Masses

D Variables

15. What quantity of gas, in moles, is contained in 2.21 L at STP?

A 0.0987 mol

B 2948 mol

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C 1974 mol

D 0454 mol

16. A steel tank with a volume of 9.583 L contains N2 gas under a pressure of 4.972 atm at 31.8 °C. Calculate the number of moles of N2 in the tank.

A 0.525 mol

B 0.002 mol

C 0.018 mol

D 1.90 mol

17. What is the density (in g/L) of a gas with a molar mass of 60 g/mol at 0.75 atm and 27 °C?

A 1.04

B 2.85g/l

C 1.83 g/L

D 2.03

19. What are standard temperature and pressure conditions for gases?

A 0°C and 0 torr

B 0 K and 760 torr

C -273°C and 1 atm

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D 0°C and 1 atm.

21. A 50. mL sample of a gas is at 3.00 atm. of pressure and a temperature of 298K . What volume would the gas occupy at STP?

A 0.00728 mL

B 15.3 mL

C 18.2 mL

D 137 mL

23.A gas is held under conditions of standard temperature and pressure. It is found that 44.0 grams of the gas occupies a volume of 22.4 L under these conditions. What is the gas?

A CO2

B Cl2

C F2

D N2

24. Which gas deviates LEAST from ideal behavior?

A SO2

B Ne

C H2

D N2

25. An 11.2L container will hold about 8.5g of which of the

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following gases at 0˚C and 1atm?

A C4H8

B NH3

C CO2

D SO2

26. Calculate the mass of KClO3 that would be required to produce 29.5 L of oxygen measured at 127oC and 760 torr. 2KClO3(s) 2KCl(s) + 3O2(g)

A 73.5 g

B 7.82 g

C 12.2 g

D 14.6 g

27. Non-ideal behavior for a gas is most likely to be observed under conditions of

A. standard temperature and pressure.

B. low temperature and high pressure.

C. low temperature and low pressure.

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D. high temperature and high pressure.

29. 0.200 moles of a gas are contained in a 2.00 L vessel at a temperature of 300C at a pressure of 10.00 atm. The gas is allowed to expand to a new volume of 8.00 liters, but at the same time maintaining the original temperature. What is the new pressure?

A 10 atm.

B 7.50 atm

C 2.50atm

D 5.00 atm

30.What is the chemical formula of a gas if it has a pressure of 1.40 atm. and a density of 1.82 g/L at 27°C?

A CO2

B CO

C CH4

D O2

31. Which of the following would have a density of 1.21 g/L at 70 C and 0.987 atm?

A Ar

B N2

C Ne

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D O2

32. How many moles of oxygen must be placed in a 3.00 L container in order to exert a pressure of 2.00 atm. at 25 °C?

A 0.245

B 146.8

C 4.08

D 21778

33. The density of chlorine gas at STP, in grams per liter, is approximately:

A 6.2

B 3.2

C 3.9

D 4.5

34. What is the molar mass of a gas which has a density of 1.30g/L measured at 27°C and 0.400 atm?

A 38.0 g/mol

B 48.0 g/mol

C 61.0 g/mol

D 80.0 g/mol

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35. If the volume of a confined gas is doubled while the temperature remains constant, what change (if any) would be observed in the pressure?

A It would be half as large.

B It would be 1/4 as large.

C It would be four times as large.

D It would remain the same.

36. 80 ml of carbon monoxide (CO) are reacted with 40 ml of oxygen (O2). What volume of carbon dioxide (CO2) is formed?

2CO + O2 --> 2CO2

A 120ml

B 200ml

C 40ml

D 80ml

37.If the molar volume of a gas at STP is 22.4 litres, how many moles are there in 11.2 L of hydrogen gas?

A 10 moles

B 0.5 moles

C 2 moles

D 3 moles

38.What volume will one mole of a gas occupy under standard temperature and pressure?

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A 22.4 L

B 1 L

C 273 L

D 293L

39. What variable is mentioned in the ideal gas law that is assumed to be constant in the other gas laws?

A temperature

B pressure

C number of moles

D volume

40.The ____________of a gas is the volume that a mole of a gas occupies at a pressure of one atmosphere and a temperature of 0.00°C

A. molar mass

B. Combined volume

C. molar volume

D. Compressed volume

41.________relates the amount of a gas present to its pressure, temperature, and volume.

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A. Ideal Gas Law

B. Boyle’s Law

C. Charles’s law

D. Avogadro’s law

Answer the following Questions

1.Study the graph below and answer the following question

a.Which gas law this graph represents?Boyle’s Lawb.Pressure and volume directly or indirectly proportional?

indirectly

c.What two variables must be held constant when comparing pressure and volume?Temperature & Amount of gasd. Determine the volume of a gas with a pressure of 4 atm.

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2.Study the graph below and answer the following question:

a.Which gas law this graph represents?Charles’s Law b.Temperature and volume directly or indirectly proportional?directlyc. What two variables must be held constant when comparing temperature and volume? Pressure & Amount of gasd.Determine the volume of a gas with a temperature of 600 K.

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3.Use the graph to answer the following questions.

a. What gas law does this graph illustrate? Gay-Lussac’s law

b.What is the pressure of Sample A if the temperature is 400 K? 4.0 atm

c.What is the temperature of Sample B if the pressure is 2.5 atm? 500k

d.Compare the pressures of Sample A and Sample B at 400 K.

The pressure of Sample A is twice that of Sample B.

e.If the samples contain the same amount of gas, which sample has a greater volume? Explain, using the ideal gas law.

Sample B; compare two pressures at the same temperature. With n, R, and T being constant, the ideal gas law equation shows that P is

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inversely proportional to V for each sample. The sample with the lower pressure will have the greater volume.

f. If the samples have the same volume, which sample contains a greater amount of gas? Explain, using the ideal gas law.

Sample A; compare two pressures at the same temperature. With V, R, and T being constant, the ideal gas law equation shows that P is directly proportional to n for each sample. The sample with the greater pressure will have the greater amount of gas.

5.A weather balloon is released into the atmosphere. You know the

initial volume, temperature, and air pressure. What information will you need to predict its volume when it reaches its final altitude? Which law would you use to calculate this volume?

(You would need to know the final temperature and final pressure to calculate the final volume. Use the combined gas law.

6.State Boyle’s law, Charles’s law, Gay-Lussac’s law, and the combined gas law in words and equations.

Boyle’s law: the volume of a given amount of gas held at a constant tem-perature varies inversely with pressure

P1V1=P2V2

Charles’s law: the volume of a given mass of gas is directly proportional to its kelvin temperature at constant pressure,

V1/T1= V2/T2

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Gay-Lussac’s law: the pressure of a given mass of gas varies directly with the kelvin temperature when the volume remains constant

P1/T1= P2/T2

combined gas law: states the relationship among pres-sure, volume, and temperature of a fixed amount of gas.

P1V1/T1 =P2V2/T2

7.Explain why R can have different numerical values.

The numerical value depends on the unit used to measure the pressure of a sample of gas.

8.Explain the relationship between the kinetic-molecular theory and an ideal gas.

An ideal gas follows all the assumptions of the kinetic-molecular theory: the

particles take up no space, the particles experience no intermolecular attractive forces, and the particles are perfectly elastic.

9.Why must an equation be balanced before using it to determine the volumes of gases involved in a reaction? (Outcome 1.6; PI,19)

Equation coefficients represent ratios among gas volumes in the reaction

10. Analyze; Is the volume of a gas directly or inversely proportional to the number of moles of a gas at constant temperature and pressure?

Explain (Directly proportional; as the amount of gas increases, so does volume

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12.Explain why Avogadro’s principle holds true for gases that have small particles and for gases that have large particles.

The size of any gas particle is so small compared to the volume of the gas, it is assumed that no particle has any volume of its own.

13.What information do you need to solve a volume-mass problem that involves gases?

balanced equation, at least one mass or volume value for a reactant or product, and Pand Tconditions under which gas volumes have been measured.

14.Define the term ideal gas,and explain why there are no true ideal gases in nature

An ideal gas is one whose particles take up no space and have no intermolecular attractive forces and it follows the gas laws under all conditions of tempera-ture and pressure. No gas is truly ideal because all gas particles have some volume and are subject to inter-molecular interactions.

Problem solving;

1. Some students believe that teachers are full of hot air. If I inhale 2.2 liters of gas at a temperature of 180 C and it heats to a temperature of 380 C in my lungs, what is the new volume of the gas?

Ans; 2.35 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? Ans; 30.5 L

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3.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?

Ans ;117 L

4.The highest pressure ever produced in a laboratory setting was about 2.0 x 106 atm. We have a 1.0 x 10-5 liter sample of a gas at that pressure.Then the pressure is released until the volume is equal to 72.7 L what would the new pressure of that gas ? Ans; 0.275 atm

5.Atmospheric pressure on the peak of Mt. Everest can be as low as 150 mm Hg, which is why climbers need to bring oxygen tanks for the last part of the climb. If the climbers carry 10.0 liter tanks with an internal gas pressure of 3.04 x 104 mm Hg, what will be the volume of the gas when it is released from the tanks

Ans;2.0 x 103 L

6. The temperature inside my refrigerator is about 40 Celsius. If I place a balloon in my fridge that initially has a temperature of 220 C and a volume of 0.5 liters, what will be the volume of the balloon when it is fully cooled by my refrigerator?

Ans;0.47 L

7. The pressure in a laboratory is 1.5 ×102kPa. What is this pressure in atm, &mmHgAns; 1.45 atm; 1102 mmHg;

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8. An automobile tire has a pressure of 210.0 kPa at 20.0°C. What will be the tire pressure after driving, if the tire temperature rises to 35.0°C?

Ans; 220.7 Kpa

9.When a sample of a gas was placed in a sealed container with a volume of 3.35 L and heated to 1050C, the gas vaporized and the resulting pressure inside the container was 170.0 kPa. How many moles of the gas was present? (Outcome 1.4; PI,16)

Ans;0.181 mol

10. What is the molar mass of a sample of gas that has a density of 2.85g/L at 101.3 kPa pressure and 290C? (

Ans;70.7 g/mol

11. Use the reaction shown to calculate the mass of iron that must be used to obtain 0.500 L of hydrogen at STP. 3Fe(s) + 4H2O(l) --. Fe3O4(s) + 4H2(g)

Ans;0.934 g Fe

12.What is the density of a gas at STP that has a molar mass of 50.0 g/mol?

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