Question 1

Coastal regions tend to have more moderate climates than land-locked areas due to the

Accepted Answer

A) high specific heat of water. 
B) heat of vaporization of water. 
C) amount of solutes in ocean water. 
D) high thermal energy in the atmosphere. 
E) latitude on which it is dependent; landmass has no effect. 
A) high specific heat of water. 
B) heat of vaporization of water. 
C) amount of solutes in ocean water. 
D) high thermal energy in the atmosphere. 
E) latitude on which it is dependent; landmass has no effect.

Question 2

In living systems molecules involved in hydrogen bonding almost always contain either oxygen or nitrogen or both.How do you explain this phenomenon?

Accepted Answer

A) Oxygen and nitrogen are elements found in both nucleic acids and proteins. 
B) Oxygen and nitrogen are elements with very high attractions for their electrons. 
C) Oxygen and nitrogen are elements found in fats and carbohydrates. 
D) Oxygen and nitrogen were both components of gases that made up the early atmosphere on Earth. 
E) Oxygen and nitrogen have valence electrons. 
A) Oxygen and nitrogen are elements found in both nucleic acids and proteins. 
B) Oxygen and nitrogen are elements with very high attractions for their electrons. 
C) Oxygen and nitrogen are elements found in fats and carbohydrates. 
D) Oxygen and nitrogen were both components of gases that made up the early atmosphere on Earth. 
E) Oxygen and nitrogen have valence electrons.

Question 3

If the pH of a solution is increased from pH 5 to pH 7,it means that the

Accepted Answer

A) concentration of H⁺ is twice (2X)what it was at pH 5. 
B) concentration of H⁺ is one-half (1/2)what it was at pH 5. 
C) concentration of OH⁻ is 100 times greater than what it was at pH 5. 
D) concentration of OH⁻ is one-hundredth (0.01X)what it was at pH 5. 
E) concentration of H⁺ is 100 times greater and the concentration of OH⁻ is one-hundredth what they were at pH 5. 
A) concentration of H⁺ is twice (2X)what it was at pH 5. 
B) concentration of H⁺ is one-half (1/2)what it was at pH 5. 
C) concentration of OH⁻ is 100 times greater than what it was at pH 5. 
D) concentration of OH⁻ is one-hundredth (0.01X)what it was at pH 5. 
E) concentration of H⁺ is 100 times greater and the concentration of OH⁻ is one-hundredth what they were at pH 5.

Question 4

Use the following figure to answer the questions below.
  
-How many grams would be equal to 1 mol of the compound shown in the figure above?
(carbon = 12,oxygen = 16,hydrogen = 1)

Accepted Answer

A) 29 
B) 30 
C) 60 
D) 150 
E) 342 
A) 29 
B) 30 
C) 60 
D) 150 
E) 342

Question 5

When snow falls on Lake Superior how are the snow's water molecules impacted?

Accepted Answer

A) They absorb thermal energy. 
B) They decrease their motion. 
C) They increase their potential energy. 
D) They release kinetic energy. 
E) They move less randomly. 
A) They absorb thermal energy. 
B) They decrease their motion. 
C) They increase their potential energy. 
D) They release kinetic energy. 
E) They move less randomly.

Question 6

Which of the following statements is true about buffer solutions?

Accepted Answer

A) They maintain a constant pH when bases are added to them but not when acids are added to them. 
B) They maintain a constant pH when acids are added to them but not when bases are added to them. 
C) They maintain a relatively constant pH of approximately 7 when either acids or bases are added to them. 
D) They maintain a relatively constant pH when either acids or bases are added to them. 
E) They are found only in living systems and biological fluids. 
A) They maintain a constant pH when bases are added to them but not when acids are added to them. 
B) They maintain a constant pH when acids are added to them but not when bases are added to them. 
C) They maintain a relatively constant pH of approximately 7 when either acids or bases are added to them. 
D) They maintain a relatively constant pH when either acids or bases are added to them. 
E) They are found only in living systems and biological fluids.

Question 7

Which of the following is a hydrophobic material?

Accepted Answer

A) paper 
B) table salt 
C) wax 
D) sugar 
E) pasta 
A) paper 
B) table salt 
C) wax 
D) sugar 
E) pasta

Question 8

Increased atmospheric CO₂ concentrations might have what effect on sea water?

Accepted Answer

A) Sea water will become more acidic, and bicarbonate concentrations will decrease. 
B) Sea water will become more alkaline, and carbonate concentrations will decrease. 
C) There will be no change in the pH of sea water, because carbonate will turn to bicarbonate. 
D) Sea water will become more acidic, and carbonate concentrations will decrease. 
E) Sea water will become more acidic, and carbonate concentrations will increase. 
A) Sea water will become more acidic, and bicarbonate concentrations will decrease. 
B) Sea water will become more alkaline, and carbonate concentrations will decrease. 
C) There will be no change in the pH of sea water, because carbonate will turn to bicarbonate. 
D) Sea water will become more acidic, and carbonate concentrations will decrease. 
E) Sea water will become more acidic, and carbonate concentrations will increase.

Question 9

The nutritional information on a cereal box shows that one serving of a dry cereal has 200 kilocalories.If one were to burn one serving of the cereal,the amount of heat given off would be sufficient to raise the temperature of 20 kg of water how many degrees Celsius?

Accepted Answer

A) 0)2°C 
B) 1)0°C 
C) 2)0°C 
D) 10.0°C 
E) 20.0°C 
A) 0)2°C 
B) 1)0°C 
C) 2)0°C 
D) 10.0°C 
E) 20.0°C

Question 10

Carbon dioxide (CO₂)is readily soluble in water,according to the equation CO₂ + H₂O ↔ H₂CO₃.Carbonic acid (H₂CO₃)is a weak acid.Respiring cells release CO₂ into the bloodstream.What will be the effect on pH of blood as that blood first comes in contact with respiring cells?

Accepted Answer

A) Blood pH will decrease slightly. 
B) Blood pH will increase slightly. 
C) Blood pH will remain unchanged. 
D) Blood pH will first increase, then decrease as CO₂ combines with hemoglobin. 
E) Blood pH will first decrease, then increase sharply as CO₂ combines with hemoglobin. 
A) Blood pH will decrease slightly. 
B) Blood pH will increase slightly. 
C) Blood pH will remain unchanged. 
D) Blood pH will first increase, then decrease as CO₂ combines with hemoglobin. 
E) Blood pH will first decrease, then increase sharply as CO₂ combines with hemoglobin.

Question 11

Which of the following has the most thermal energy?

Accepted Answer

A) a boiling cup of coffee 
B) a swimming pool at 28°C 
C) a hot tub at 37°C 
D) the Pacific ocean 
E) Lake Erie 
A) a boiling cup of coffee 
B) a swimming pool at 28°C 
C) a hot tub at 37°C 
D) the Pacific ocean 
E) Lake Erie

Question 12

Equal volumes (5 mL)of vinegar from a freshly opened bottle are added to each of the following solutions.After complete mixing,which of the mixtures will have the highest pH?

Accepted Answer

A) 100 mL of pure water 
B) 100 mL of freshly brewed coffee 
C) 100 mL of household cleanser containing 0.5 M ammonia 
D) 100 mL of freshly squeezed orange juice 
E) 100 mL of tomato juice 
A) 100 mL of pure water 
B) 100 mL of freshly brewed coffee 
C) 100 mL of household cleanser containing 0.5 M ammonia 
D) 100 mL of freshly squeezed orange juice 
E) 100 mL of tomato juice

Question 13

Which of the following solutions would require the greatest amount of base to be added to bring the solution to neutral pH?

Accepted Answer

A) gastric juice at pH 2 
B) vinegar at pH 3 
C) tomato juice at pH 4 
D) black coffee at pH 5 
E) household bleach at pH 12 
A) gastric juice at pH 2 
B) vinegar at pH 3 
C) tomato juice at pH 4 
D) black coffee at pH 5 
E) household bleach at pH 12

Question 14

In a single molecule of water,two hydrogen atoms are bonded to a single oxygen atom by

Accepted Answer

A) hydrogen bonds. 
B) nonpolar covalent bonds. 
C) polar covalent bonds. 
D) ionic bonds. 
E) van der Waals interactions. 
A) hydrogen bonds. 
B) nonpolar covalent bonds. 
C) polar covalent bonds. 
D) ionic bonds. 
E) van der Waals interactions.

Question 15

A slice of pizza has 2092 kJ.If we could burn the pizza and use all the heat to warm a 50-L container of cold water,what would be the approximate increase in the temperature of the water? (Note: A litre of cold water weighs about 1 kg.)

Accepted Answer

A) 50°C 
B) 5°C 
C) 1°C 
D) 100°C 
E) 10°C 
A) 50°C 
B) 5°C 
C) 1°C 
D) 100°C 
E) 10°C

Question 16

We can be sure that a mole of table sugar and a mole of vitamin C are equal in their

Accepted Answer

A) mass in daltons. 
B) mass in grams. 
C) volume. 
D) number of atoms. 
E) number of molecules. 
A) mass in daltons. 
B) mass in grams. 
C) volume. 
D) number of atoms. 
E) number of molecules.

Question 17

The molar mass of glucose is 180 g/mol.Which of the following procedures should you carry out to make a 1 M solution of glucose?

Accepted Answer

A) Dissolve 1 g of glucose in 1 L of water. 
B) Dissolve 180 g of glucose in 1 L of water. 
C) Dissolve 180 g of glucose in 180 g of water. 
D) Dissolve 180 milligrams (mg)of glucose in 1 L of water. 
E) Dissolve 180 g of glucose in 0.8 L of water, and then add more water until the total volume of the solution is 1 L. 
A) Dissolve 1 g of glucose in 1 L of water. 
B) Dissolve 180 g of glucose in 1 L of water. 
C) Dissolve 180 g of glucose in 180 g of water. 
D) Dissolve 180 milligrams (mg)of glucose in 1 L of water. 
E) Dissolve 180 g of glucose in 0.8 L of water, and then add more water until the total volume of the solution is 1 L.

Question 18

How many grams of acetic acid (C₂H₄O₂)would you use to make 10 L of a 0.1 M aqueous solution of acetic acid? (Note: The atomic masses,in daltons,are approximately 12 for carbon,1 for hydrogen,and 16 for oxygen.)

Accepted Answer

A) 10 g 
B) 0)1 g 
C) 6)0 g 
D) 60 g 
E) 0)6 g 
A) 10 g 
B) 0)1 g 
C) 6)0 g 
D) 60 g 
E) 0)6 g

Question 19

The reason water has a high specific heat is that

Accepted Answer

A) the adhesive property of water resists heat absorption. 
B) ionic bonds require a lot of energy to be broken. 
C) a lot of heat needs to be absorbed to disrupt hydrogen bonds. 
D) the covalent bonds resist splitting. 
E) water cools very quickly. 
A) the adhesive property of water resists heat absorption. 
B) ionic bonds require a lot of energy to be broken. 
C) a lot of heat needs to be absorbed to disrupt hydrogen bonds. 
D) the covalent bonds resist splitting. 
E) water cools very quickly.

Question 20

Temperature usually increases when water condenses.Which behaviour of water is most directly responsible for this phenomenon?

Accepted Answer

A) the change in density when it condenses to form a liquid or solid 
B) reactions with other atmospheric compounds 
C) the release of heat by the formation of hydrogen bonds 
D) the release of heat by the breaking of hydrogen bonds 
E) the high surface tension of water 
A) the change in density when it condenses to form a liquid or solid 
B) reactions with other atmospheric compounds 
C) the release of heat by the formation of hydrogen bonds 
D) the release of heat by the breaking of hydrogen bonds 
E) the high surface tension of water

Exam 3: Water and Life

Coastal regions tend to have more moderate climates than land-locked areas due to the

In living systems molecules involved in hydrogen bonding almost always contain either oxygen or nitrogen or both.How do you explain this phenomenon?

If the pH of a solution is increased from pH 5 to pH 7,it means that the

Use the following figure to answer the questions below. -How many grams would be equal to 1 mol of the compound shown in the figure above? (carbon = 12,oxygen = 16,hydrogen = 1)

When snow falls on Lake Superior how are the snow's water molecules impacted?

Which of the following statements is true about buffer solutions?

Which of the following is a hydrophobic material?

Increased atmospheric CO₂ concentrations might have what effect on sea water?

The nutritional information on a cereal box shows that one serving of a dry cereal has 200 kilocalories.If one were to burn one serving of the cereal,the amount of heat given off would be sufficient to raise the temperature of 20 kg of water how many degrees Celsius?

Carbon dioxide (CO₂)is readily soluble in water,according to the equation CO₂ + H₂O ↔ H₂CO₃.Carbonic acid (H₂CO₃)is a weak acid.Respiring cells release CO₂ into the bloodstream.What will be the effect on pH of blood as that blood first comes in contact with respiring cells?

Which of the following has the most thermal energy?

Equal volumes (5 mL)of vinegar from a freshly opened bottle are added to each of the following solutions.After complete mixing,which of the mixtures will have the highest pH?

Which of the following solutions would require the greatest amount of base to be added to bring the solution to neutral pH?

In a single molecule of water,two hydrogen atoms are bonded to a single oxygen atom by

A slice of pizza has 2092 kJ.If we could burn the pizza and use all the heat to warm a 50-L container of cold water,what would be the approximate increase in the temperature of the water? (Note: A litre of cold water weighs about 1 kg.)

We can be sure that a mole of table sugar and a mole of vitamin C are equal in their

The molar mass of glucose is 180 g/mol.Which of the following procedures should you carry out to make a 1 M solution of glucose?

How many grams of acetic acid (C₂H₄O₂)would you use to make 10 L of a 0.1 M aqueous solution of acetic acid? (Note: The atomic masses,in daltons,are approximately 12 for carbon,1 for hydrogen,and 16 for oxygen.)

The reason water has a high specific heat is that

Temperature usually increases when water condenses.Which behaviour of water is most directly responsible for this phenomenon?

Introduction: Evolution and Themes of Biology

The Chemical Context of Life

Carbon and the Molecular Diversity of Life

The Structure and Function of Large Biological Molecules

A Tour of the Cell

Membrane Structure and Function

An Introduction to Metabolism

Cellular Respiration and Fermentation

Photosynthesis

Cell Communication

The Cell Cycle

Meiosis and Sexual Life Cycles

Mendel and the Gene Idea

The Chromosomal Basis of Inheritance

The Molecular Basis of Inheritance

From Gene to Protein

Regulation of Gene Expression

Viruses

DNA Tools and Biotechnology

Genomes and Their Evolution

Descent with Modification: A Darwinian View of Life

The Evolution of Populations

The Origin of Species

The History of Life on Earth

Phylogeny and the Tree of Life

Bacteria and Archaea

Protists

Plant Diversity I: How Plants Colonized Land

Plant Diversity II: The Evolution of Seed Plants

Fungi

An Overview of Animal Diversity

An Introduction to Invertebrates

The Origin and Evolution of Vertebrates

Plant Structure,Growth,and Development

Resource Acquisition and Transport in Vascular Plants

Soil and Plant Nutrition

Angiosperm Reproduction and Biotechnology

Plant Responses to Internal and External Signals

Basic Principles of Animal Form and Function

Animal Nutrition

Circulation and Gas Exchange

The Immune System

Osmoregulation and Excretion

Hormones and the Endocrine System

Animal Reproduction

Animal Development

Neurons,Synapses,and Signalling

Nervous Systems

Sensory and Motor Mechanisms

Animal Behaviour

An Introduction to Ecology and the Biosphere

Population Ecology

Community Ecology

Ecosystems and Restoration Ecology

Conservation Biology and Global Change

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