Deck 6: Gases, Solutions, Colloids, and Suspensions

Question 1

When the pressure is increased above 760 torr, the boiling point of water

A) decreases to temperatures below 100 C.
B) remains the same at 100C.
C) increases to temperatures above.
D) drops to temperatures below 0C.

Answer 1

increases to temperatures above.

Question 2

The atmospheric pressure on a given day is 742 torr. What is this pressure in atmospheres?

A) 0.976 atm
B) 5.63 x 10⁵ atm
C) 50.5 atm
D) 1.09 x 10⁴ atm

Answer 2

0.976 atm

Question 3

Certain automobile tires are to be inflated to a pressure of 35.0 psi. What is this pressure in torr?

A) 0.0461 torr
B) 0.677 torr
C) 515 torr
D) 1810 torr

Answer 3

1810 torr

Question 4

A steel tank is filled with nitrogen gas at a pressure of 2.30 atm. What is this pressure in torr?

A) 2.30 torr
B) 1750 torr
C) 3.03 x 10^-3 torr
D) 760 torr

Question 5

Standard temperature and pressure corresponds to

A) temperature of 0C and pressure of 1 psi.
B) temperature of 25C and pressure of 1 atm.
C) temperature of 0C and pressure of 2 psi.
D) temperature of 0C and pressure of 1 atm.

Question 6

The equivalent of 1 atmosphere of pressure is ___.

A) 14.7 mm mercury
B) 650 mm mercury
C) 700 torr
D) 760 torr

Question 7

A hurricane might be preceded by an atmospheric pressure of 727 torr. Express 727 torr in atmospheres of pressure.

A) 0.727 atm
B) 0.957 atm
C) 1.05 atm
D) 49.5 atm

Question 8

The device used to determine a patient's blood pressure is the

A) manometer.
B) barometer.
C) sphygmomanometer.
D) hyperbarometer.

Question 9

When a person inhales air,

A) lung volume decreases and lung pressure increases.
B) lung volume increases and lung pressure decreases.
C) lung volume decreases and lung pressure decreases.
D) lung volume increases and lung pressure increases.

Question 10

In Death Valley, which is located below sea level, the atmospheric pressure exceeds 760 torr. Water boils at ___.

A) a temperature less than 100^ºC
B) 100^ºC
C) a temperature greater than 100^ºC
D) None of these choices.

Question 11

In a mountain location where the atmospheric pressure is less than 1.00 atm, water will boil at ___.

A) a temperature less than 100^ºC
B) 100^ºC
C) a temperature greater than 100^ºC
D) None of these choices.

Question 12

The cause of chronic hypertension is

A) high blood pressure.
B) blood moving too fast though the arteries that are dilated.
C) constricted movement of blood through blood vessels.
D) the inability of the body to respond to a change in posture.

Question 13

Which blood pressure variation tends to double the risk of heart disease?

A) an increase of 5 points systolic pressure
B) an increase of 10 points systolic pressure
C) an increase of 5 points diastolic pressure
D) an increase of 10 points diastolic pressure

Question 14

According to Charles' law, when the Kelvin temperature of a gas doubles (at constant pressure), its volume will ___.

A) double
B) reduced to 1/2
C) quadruple
D) remain the same

Question 15

According to Gay-Lussac's law, when the Kelvin temperature of a gas doubles (at constant volume), its pressure will ___

A) double
B) reduced to 1/2
C) quadruple
D) remain the same

Question 16

According to Boyle's law, when the pressure on a gas is doubled (at constant temperature), its volume will ___.

A) double
B) be reduced to 1/2
C) quadruple
D) remain the same

Question 17

The gas constant is used in some calculations. The value of the gas constant is

A) to make certain that all gases are ideal gases.
B) 0.0821 L atm/mol K.
C) 25°C and 1 atm.
D) 0°C and 1 atm at 1-L volume.

Question 18

What will be the mass of hydrogen gas, H₂, that is stored in a 15.0-L container at the pressure of 7.50 atm? The container is kept at 20.0°C. (Use the mass of 2.00 g/mol for the hydrogen.)

A) 225 g
B) 137 g
C) 80.0 g
D) 9.35 g

Question 19

A cylinder of gas originally at 28.0°C and 1.00 atm of pressure is heated to 112.0°C. What is the new pressure?

A) 4.00 atm
B) 0.250 atm
C) 0.782 atm
D) 1.28 atm

Question 20

A balloon containing 0.56 mole of helium has a volume of 10.0 L. What volume will the balloon occupy if helium is lost and only 0.21 mole remain?

A) 27 L
B) 3.8 L
C) 2.1 L
D) 5.6 L

Question 21

A gas sample occupies 10.28 L at 8.34 atm. Its volume at 6.98 atm (assuming constant temperature conditions) is ___.

A) 12.3 L
B) 5.66 L
C) 8.60 L
D) 15.6 L

Question 22

At what pressure would methane gas occupy 13.8 L if it occupies 5.74 L at 3.67 atm assuming constant temperature?

A) 8.82 atm
B) 21.6 atm
C) 1.53 atm
D) 11.3 atm

Question 23

A sample of nitrogen gas exerts a pressure of 9.80 atm at 32 C. What would its temperature be (in C) when its pressure is increased to 11.2 atm?

A) 76 C
B) - 6.2 C
C) 49 C
D) 3.5 x 10² C

Question 24

A gas sample occupies 5.38 L at 36.0 C. What is its temperature if the volume is changed to 4.86 L?

A) 69.1 C
B) 44.8 C
C) 11.9 C
D) 6.12 C

Question 25

A 0.45 mole of krypton gas occupies a volume of 1.6 L. What volume will 1.8 moles of krypton occupy assuming the temperature and pressure remain the same?

A) 6.4 L
B) 0.51 L
C) 0.40 L
D) 3.2 L

Question 26

The warning label on metallic aerosol cans state that one should not heat or incinerate them. At high temperature a rigid container may have its pressure increase to the point that it may fail and explode. This is best explained by ___.

A) Boyles' law
B) Charles' law
C) Gay-Lussac's law
D) Avogadro's law

Question 27

What is the volume of a mole of an ideal gas under standard conditions (STP)?

A) 0.0821 liter
B) 760 liters
C) 22.4 liters
D) 1.0 liter

Question 28

A gas occupies a volume of 8.60 L at 45C and 764 torr. What pressure would it occupy if the volume is adjusted to 13.3 L at 20C?

A) 536 torr
B) 455 torr
C) 109 torr
D) 188 torr

Question 29

A sample of neon gas fills a 6.85-L container. What is the new temperature (in Kelvin) if the gas is transferred into a 9.64-L container and pressure adjusted to 604 torr?

A) 305 K
B) 483 K
C) 244 K
D) 656 K

Question 30

An uninflated balloon full of air has a volume of 300.0 mL and contains 0.0240 mole of air. A 2.00 g piece of dry ice (solid CO₂) is placed in the vessel and sealed. What is the volume of the balloon after the dry ice has vaporized? Assume constant temperature and pressure. Also, assume no change in the initial amount of air.

A) 869 mL
B) 300 mL
C) 240 mL
D) 455 mL

Question 31

Carbon dioxide gas occupies a volume of 20.0 L at 308K and 2.30 atm. What volume would it occupy at 416 K and 5.40 atm?

A) 6.3 L
B) 11.5 L
C) 0.460 L
D) 22.4 L

Question 32

A sample of hydrogen gas (H₂) has a volume of 17.4 L at a temperature of 0.00C and a pressure of 1.60 atm. The number of moles of H₂ molecules of hydrogen in the sample is

A) 2.48 mol
B) 0.652 mol
C) 1.24 mol
D) 4.41 mol

Question 33

A cylinder of gas at a temperature of 21^oC has a pressure of 3.8 atm. If the closed cylinder were heated in a fire to a temperature of 365^oC, what would be the new pressure?

A) 8.2 atm
B) 66 atm
C) 1.8 atm
D) 0.22 atm

Question 34

A pressurized tank contains nitrogen at 1.3 atm, oxygen at 0.7 atm, and helium at 0.1 atm. The reading of the pressure gauge is expected to be ___.

A) 0.5 atm
B) 0.91 atm
C) 1.3 atm
D) 2.1 atm

Question 35

A 155-L helium balloon is heated from 24.0 C to 38.0 C. What would be its new volume assuming the pressure remains constant?

A) 148 L
B) 162 L
C) 597 L
D) 258 L

Question 36

A gas cylinder at a pressure of 4408 torr contains a mixture of N₂, O₂, and helium gases. If the partial pressure of N₂ gas is 1520 torr and the partial pressure of helium is 25 torr, what is the partial pressure of O₂?

A) 760 torr
B) 4020 torr
C) 5953 torr
D) 2863 torr

Question 37

In a homogeneous mixture

A) the substances are not evenly distributed.
B) the substances are always liquid.
C) the substances are always solids.
D) the substances are uniformly distributed.

Question 38

Which of the following mixtures is heterogeneous?

A) sea water
B) carbonated water
C) Kool Aid solution
D) concrete

Question 39

Oxygen is dissolved into water to make a solution. If the temperature of the solution is increased, the solubility of the oxygen will ___.

A) decrease
B) increase
C) be unchanged

Question 40

Which is a pure substance?

A) calcium chloride and potassium chloride crystals in a beaker
B) air
C) water
D) sodium chloride and potassium chloride dissolved in water

Question 41

The solute of a solution is the component

A) that is dissolved in the solvent.
B) in the greatest supply.
C) that must be ionic.
D) that must be a solid.

Question 42

For solute particles to be soluble in liquid solvents

A) they must be about the same size as the solvent molecules and be able to interact with the solvent molecules through noncovalent interactions.
B) the solvent must be nonpolar.
C) they must be polar.
D) they must be of smaller size than solvent molecules and be able to interact with solvent molecules through covalent interactions.

Question 43

In water, Vanillin, C₈H₈O₃, has a solubility of 0.070 moles of vanillin per liter of solution at 25C. What will be produced if 5.00 g of vanillin are added to 1 L of water at 25 C?

A) a homogeneous mixture
B) a heterogeneous mixture
C) a precipitate
D) a strong electrolyte

Question 44

Which of the following ionic substances is insoluble in water?

A) KNO₃
B) BaSO₄
C) Na₃PO₄
D) NH₄Br

Question 45

Which of the following ionic substances is soluble in water?

A) Ca(OH)₂
B) PbCO₃
C) AgCl
D) KNO₃

Question 46

Identify the compound that is soluble in water.

A) Ca(OH)₂
B) Ba(NO₃)₂
C) AgCl
D) Fe₂(CO₃)₃

Question 47

Identify the compound that is insoluble in water.

A) Ba₃(PO₄)₂
B) Ba(NO₃)₂
C) K₃PO₄
D) AgNO₃

Question 48

The net ionic equation for the reaction of sodium hydroxide, NaOH, and magnesium nitrate, Mg(NO₃)₂, contains which of the following species?

A) 2Mg²⁺ (aq)
B) Na+
C) Mg(OH)₂ (s)
D) NaNO₃ (aq)

Question 49

The "bends" is a condition in which nitrogen gas is released from solution in the blood vessels of a scuba diver. It is caused by a diver rising too quickly to the surface of the water. This condition is explained by Henry's Law. The solubility of a gas in solution ___ as the pressure ___.

A) decreases/decreases
B) increases/decreases
C) decreases/increases

Question 50

Oxygen dissolves in water to the extent of 6 mL O₂ per liter of water at 20°C and 1 atm pressure. Suppose the pressure were to be increased to 3 atm and the temperature is maintained at 20°C. How will the solubility of the oxygen be affected?

A) The solubility will increase to 18 mL/L.
B) The solubility will decrease to 2 mL/L.
C) The solubility will remain at 6 mL/L.
D) There is no predictable trend in solubility on the basis of temperature and pressure.

Question 51

Unlike acetic acid (CH₂COOH), which is completely soluble in water, 1-hexanoic acid (CH₂CH₂CH₂CH₂CH₂COOH) is only slightly soluble in water because

A) only acetic acid forms hydrogen bonds.
B) acetic acid has a higher boiling point than 1-hexanoic acid.
C) the increased length of carbon chain in 1-hexanoic acid increases its hydrophobic character.
D) acetic acid does not ionize in water.

Question 52

Which of the following is a general statement concerning the solubility of organic compounds?

A) The larger molecules dissolve best in a solvent with a low molecular weight.
B) The polar organic compounds dissolve best in polar solvents.
C) The nonpolar compounds can dissolve well in polar solvents if the molecules are close to the same size.
D) Those compounds that have only covalent bonds dissolve well in water.

Question 53

A compound is likely to be hydrophilic if

A) it contains polar groups.
B) all of the chemical bonds are covalent.
C) the compound forms strong London force interactions between molecules.
D) there are many carbon atoms in the skeleton of the molecule.

Question 54

Soaps are amphipathic compounds. Which statement best describes them?

A) Soaps cannot be attracted to either polar or nonpolar compounds.
B) Soaps dissolve best in polar solvents, which is why they can remove dirt.
C) Soaps have a hydrophobic end, which will attract nonpolar substances, such as soil on clothing.
D) The soaps that are the most effective in cleaning contain the calcium ion.

Question 55

Based on its structure, menthol is expected to be ___.

A) hydrophilic
B) hydrophobic
C) predominantly polar
D) ionic

Question 56

Ethyl alcohol (CH₃CH₂OH) is completely soluble in water. It is made of both polar and non-polar groups. Ethyl alcohol is best classified as a(n) ___ substance.

A) hydrophilic
B) hydrophobic
C) lipophilic
D) amphipathic

Question 57

A prodrug is

A) used because it is less expensive than the regular medication.
B) a more professional type of medication than is normally used.
C) the metabolic result of normal bodily processes on commonly available materials.
D) a precursor of a drug that is converted by metabolic processes to that drug.

Question 58

A patient's blood test indicates that 1.00 mL of serum contains 0.00140 g of fibrinogen (a protein that aids in coagulation of blood). What is the concentration of the fibrinogen in mg/dL?

A) 280 mg/dL
B) 14 mg/dL
C) 0.014 mg/dL
D) 140. mg/dL

Question 59

How many milliliters of 6.0 M HCl must be diluted to make 500.0 mL of a 0.10 M solution?

A) 1.2 mL
B) 8.3 mL
C) 30. mL
D) 300 mL

Question 60

What is the %(w/v) of a 1500mL solution containing 45 g of NaCl?

A) 5.0%
B) 3.0%
C) 2.0%
D) 0.030%

Question 61

How many grams of vitamin B₁₂ are present in a 100.0 mL blood serum sample with a vitamin B12 concentration of 148 ng/L?

A) 1.48 x 10^-9 g
B) 1.48 x 10^-8 g
C) 1.48 x 10^-5 g
D) 1.48 g

Question 62

Sodium fluoride is added to drinking water. A 25-L sample of city water contains 0.018 g NaF. Express this concentration in molarity.

A) 0.000017 M
B) 0.00072 M
C) 0.018 M
D) 18 M

Question 63

If 48L of city water contains 0.030 g sodium fluoride, what is the concentration in parts per thousand?

A) 16 ppt
B) 0.0025 ppt
C) 0.00063 ppt
D) 1.4 ppt

Question 64

What is the concentration in parts per billion of an 8 L solution containing 0.017 g of potassium iodide?

A) 2.1 x 10² ppb
B) 3.1 x 10² ppb
C) 1.1 x 10² ppb
D) 5.8 x 10² ppb

Question 65

What volume of 2.00 % NaCl must be diluted to make 10.00 mL of 0.90% NaCl, also known as normal saline solution?

A) 4.5 mL
B) 0.18 mL
C) 9.0 mL
D) 22.2 mL

Question 66

How many grams of AgNO₃ are required to make 500.0 mL of a 0.10 M solution?

A) 8.5 g
B) 17 g
C) 85 g
D) 0.10 g

Question 67

15.0 g of KCl is dissolved into a solution with a total volume of 250.0 mL. What is the molarity of the solution?

A) 0.200 M
B) 3.75 M
C) 0.804 M
D) 1.24 M

Question 68

The concentration of calcium ion in blood is found to be 1.21 mmol/L. What is this concentration in mEq/L?

A) 0.605 mEq/L
B) 1.21 mEq/L
C) 2.42 mEq/L
D) 4.84 mEq/L

Question 69

Blood serum has a calcium ion (Ca²⁺) concentration of 3.9 x 10^-4 M. What is the concentration in mEq/L?

A) 0.78 mEq/L
B) 0.39 mEq/L
C) 2.3 mEq/L
D) 6.8 mEq/L

Question 70

An egg yolk with the volume of 3.75 mL contains 5.00 µg vitamin D (cholecalcifoerol). What is the concentration of vitamin D in mg/dL? (1 µg = 10^-6 g and 1 dL = 10^-1 L)

A) 0.0188mg/dL
B) 0.133 mg/dL
C) 0.750 mg/dL
D) 1.30 mg/dL

Question 71

Polocaine is a local anesthetic administered by injection. A 50-mL, multidose vial is available containing 100 mg of mepivacaine hydrochloride. What is the percent concentration of the solution?

A) 0%
B) 0.2%
C) 50%
D) 5,000%

Question 72

A water sample taken from the ocean is 36 ppt salt content. What is the mass of salt present in a liter of this ocean water?

A) 0.028 g
B) 27.8 g
C) 36 g
D) 36,000 g

Question 73

Sucralfate (molecular weight: 2087g/mol) is a major component of Carafate, which is prescribed for the treatment of gastrointestinal ulcers. The recommended dose for a duodenal ulcer is 1.0g taken orally in 10.0 mL (2 teaspoons) of a solution four times a day. Calculate the molarity of the solution.

A) 0.0005 M
B) 0.048 M
C) 0.02087 M
D) 0.010 M

Question 74

A patient has been trying to achieve total blood cholesterol of 175 mg or less per 100 mL. A recent test result of a 3 mL blood sample found that 4.95 mg cholesterol were present. Has the patient reached the goal?

A) No, 4.95 mg/3 mL is more than the goal.
B) Yes, 4.95 mg/3 mL is equivalent to 165 mg/100 mL.
C) Yes, the result (4.95 x 3) is much less than the goal (175 x 100).
D) Undetermined; 100 mL blood would have to be drawn to do a valid test.

Question 75

A free thyroxine concentration in plasma of 1.1 ng/dL is in the normal range. At this concentration, how many milligrams of free thyroxine are present in 30.0 mL of plasma?

A) 3.3 x 10^-10 mg
B) 3.3 x 10³ mg
C) 110 mg
D) 3.3 x 10^-7 mg

Question 76

A bottle of 6.000 M NaOH is on the lab bench. You are instructed to use 75.00 mL of 0.5000 M NaOH. How much 6.000 M NaOH do you have to dilute to 75.00 mL to meet the requirement?

A) The solution cannot be produced from 6.000 M NaOH.
B) 37.50 mL
C) 9.000 mL
D) 6.250 mL

Question 77

If 25.0 mL of 3.0 M HCl are diluted to give a final volume of 150 mL, what is the new concentration?

A) 0.50 M
B) 75 M
C) 2.0 M
D) 4.5 M

Question 78

Whipped cream is an example of a ___.

A) solution
B) suspension
C) colloid
D) solvent

Question 79

Milk of Magnesia is a heterogeneous mixture of magnesium hydroxide, Mg(OH)₂, and water. The label on the bottle says that one should "Shake Well Before Using." Milk of Magnesia would be classified as a ___.

A) solution
B) suspension
C) colloid
D) solvent

Question 80

Arrange the terms solution, suspension, and colloid in order of increasing size of the dispersed particles.

A) solution < suspension < colloid
B) solution < colloid < suspension
C) suspension < solution < colloid
D) colloid < solution < suspension