?What is matter composed of?

Define matter and list some examples.

What is matter composed of?

What are the three states of matter?

What are the properties of a solid?

What is the difference between a crystalline solid and an amorphous solid?

What are the properties of a liquid?

What are the properties of a gas?

Why are gases compressible?

What is a mixture?

What is the difference between a homogeneous mixture and a heterogeneous mixture?

What is a pure substance?

What is an element? A compound?

What is the difference between a mixture and a compound?

What is the definition of a physical property? What is the definition of a chemical property?

What is the difference between a physical change and a chemical change?

What is the law of conservation of mass?

What is the definition of energy?

What is the law of conservation of energy?

Explain the difference between kinetic energy and potential energy.

What is chemical energy? List some examples of common substances that contain chemical energy.

List three common units for energy.

What is an exothermic reaction? Which has greater energy in an exothermic reaction, the reactants or the products?

What is an endothermic reaction? Which has greater energy in an endothermic reaction, the reactants or the products?

List three common units for measuring temperature.

Explain the difference between heat and temperature.

How do the three temperature scales differ?

What is heat capacity?

Why are coastal geographic regions normally cooler in the summer than inland geographic regions?

The following equation can be used to convert Fahrenheit temperature to Celsius temperature. \({ }^{\circ} \mathrm{C}=\frac{\left({ }^{\circ} \mathrm{F}-32\right)}{1.8}\) Use algebra to change the equation to convert Celsius temperature to Fahrenheit temperature. Text Transcription: ^circ C=\^circ F-32 1.8

The following equation can be used to convert Celsius temperature to Kelvin temperature. \(\mathrm{K}={ }^{\circ} \mathrm{C}+273.15\) Use algebra to change the equation to convert Kelvin temperature to Celsius temperature. Text Transcription: K=^circ C+273.15

Classify each pure substance as an element or a compound. (a) aluminum (b) sulfur (c) methane (d) acetone

Classify each pure substance as an element or a compound. (a) carbon (b) baking soda (sodium bicarbonate) (c) nickel (d) gold

Classify each mixture as homogeneous or heterogeneous. (a) coffee (b) chocolate sundae (c) apple juice (d) gasoline

Classify each mixture as homogeneous or heterogeneous. (a) baby oil (b) chocolate chip cookie (c) water and gasoline (d) wine

Classify each substance as a pure substance or a mixture. If it is a pure substance, classify it as an element or a compound. If it is a mixture, classify it as homogeneous or heterogeneous. (a) helium gas (b) clean air (c) rocky road ice cream (d) concrete

Classify each substance as a pure substance or a mixture. If it is a pure substance, classify it as an element or a compound. If it is a mixture, classify it as homogeneous or heterogeneous. (a) urine (b) pure water (c) SnickersTM bar (d) soil

Classify each property as physical or chemical. (a) the tendency of silver to tarnish (b) the shine of chrome (c) the color of gold (d) the flammability of propane gas

Classify each property as physical or chemical. (a) the boiling point of ethyl alcohol (b) the temperature at which dry ice sublimes (turns from a solid into a gas) (c) the flammability of ethyl alcohol (d) the smell of perfume

Which of the following properties of ethylene (a ripening agent for bananas) are physical properties, and which are chemical? • colorless • odorless • flammable • gas at room temperature • 1 L has a mass of 1.260 g under standard conditions • mixes with acetone • polymerizes to form polyethylene

Which of the following properties of ozone (a pollutant in the lower atmosphere but part of a protective shield against UV light in the upper atmosphere) are physical, and which are chemical? • bluish color • pungent odor • very reactive • decomposes on exposure to ultraviolet light • gas at room temperature

Classify each change as physical or chemical. (a) A balloon filled with hydrogen gas explodes upon contact with a spark. (b) The liquid propane in a barbecue evaporates away because someone left the valve open. (c) The liquid propane in a barbecue ignites upon contact with a spark. (d) Copper metal turns green on exposure to air and water.

Classify each change as physical or chemical. (a) Sugar dissolves in hot water. (b) Sugar burns in a pot. (c) A metal surface becomes dull because of continued abrasion. (d) A metal surface becomes dull on exposure to air.

A block of aluminum is (a) ground into aluminum powder and then (b) ignited. It then emits flames and smoke. Classify (a) and (b) as chemical or physical changes.

Several pieces of graphite from a mechanical pencil are (a) broken into tiny pieces. Then the pile of graphite is (b) ignited with a hot flame. Classify (a) and (b) as chemical or physical changes.

An automobile gasoline tank holds 42 kg of gasoline. When the gasoline burns, 168 kg of oxygen are consumed and carbon dioxide and water are produced. What total combined mass of carbon dioxide and water is produced?

In the explosion of a hydrogen-filled balloon, 0.50 g of hydrogen reacts with 4.0 g of oxygen. How many grams of water vapor are formed? (Water vapor is the only product.)

Are these data sets on chemical changes consistent with the law of conservation of mass? (a) A 7.5-g sample of hydrogen gas completely reacts with 60.0 g of oxygen gas to form 67.5 g of water. (b) A 60.5-g sample of gasoline completely reacts with 243 g of oxygen to form 206 g of carbon dioxide and 88 g of water.

Are these data sets on chemical changes consistent with the law of conservation of mass? (a) A 12.8-g sample of sodium completely reacts with 19.6 g of chlorine to form 32.4 g of sodium chloride. (b) An 8-g sample of natural gas completely reacts with 32 g of oxygen gas to form 17 g of carbon dioxide and 16 g of water.

In a butane lighter, 9.7 g of butane combine with 34.7 g of oxygen to form 29.3 g carbon dioxide and how many grams of water?

A 56-g sample of iron reacts with 24 g of oxygen to form how many grams of iron oxide?

Perform each conversion. (a) 588 cal to joules (b) 17.4 J to Calories (c) 134 kJ to Calories (d) 56.2 Cal to joules

Perform each conversion. (a) 45.6 J to calories (b) 355 cal to joules (c) 43.8 kJ to calories (d) 215 cal to kilojoules

Perform each conversion. (a) 25 kWh to joules (b) 249 cal to Calories (c) 113 cal to kilowatt-hours (d) 44 kJ to calories

Perform each conversion. (a) 345 Cal to kilowatt-hours (b) 23 J to calories (c) \(5.7 \times 10^{3}\) J to kilojoules (d) 326 kJ to joules Text Transcription: 5.7 times 10^3

Complete the table:

Complete the table:

An energy bill indicates that a customer used 1027 kWh in July. How many joules did the customer use?

A television uses 32 kWh of energy per year. How many joules does it use?

An adult eats food whose nutritional energy totals approximately \(2.2 \times 10^{3}\) Cal per day. The adult burns \(2.0 \times 10^{3}\) Cal per day. How much excess nutritional energy, in kilojoules, does the adult consume per day? If 1 lb of fat is stored by the body for each \(14.6 \times 10^{3}\) kJ of excess nutritional energy consumed, how long will it take this person to gain 1 lb? Text Transcription: 2.2 times 10^3 2.0 times 10^3 14.6 times 10^3

How many joules of nutritional energy are in a bag of chips with a label that lists 245 Cal? If 1 lb of fat is stored by the body for each \(14.6 \times 10^{3}\) kJ of excess nutritional energy consumed, how many bags of chips contain enough nutritional energy to result in 1 lb of body fat? Text Transcription: 14.6 times 10^3

A common type of handwarmer contains iron powder that reacts with oxygen to form an oxide of iron. As soon as the handwarmer is exposed to air, the reaction begins and heat is emitted. Is the reaction between the iron and oxygen exothermic or endothermic? Draw an energy diagram showing the relative energies of the reactants and products in the reaction.

In a chemical cold pack, two substances are kept separate by a divider. When the divider is broken, the substances mix and absorb heat from the surroundings. The chemical cold pack feels cold. Is the reaction exothermic or endothermic? Draw an energy diagram showing the relative energies of the reactants and products in the reaction.

Classify each process as exothermic or endothermic. (a) gasoline burning in a car (b) isopropyl alcohol evaporating from skin (c) water condensing as dew during the night

Classify each process as exothermic or endothermic. (a) dry ice subliming (changing from a solid directly to a gas) (b) the wax in a candle burning (c) a match burning

Perform each temperature conversion. (a) 212 \({ }^{\circ} \mathrm{F}\) to Celsius (temperature of boiling water) (b) 77 K to Fahrenheit (temperature of liquid nitrogen) (c) 25 \({ }^{\circ} \mathrm{C}\) to kelvins (room temperature) (d) 98.6 \({ }^{\circ} \mathrm{F}\) to kelvins (body temperature) Text Transcription: ^circ F ^circ C

Perform each temperature conversion. (a) 102 \({ }^{\circ} \mathrm{F}\) to Celsius (b) 0 K to Fahrenheit (c) -48 \({ }^{\circ} \mathrm{C}\) to Fahrenheit (d) 273 K to Celsius Text Transcription: ^circ F ^circ C

The coldest temperature ever measured in the United States was -80 \({ }^{\circ} \mathrm{F}\) on January 23, 1971, in Prospect Creek, Alaska. Convert that temperature to degrees Celsius and Kelvin. (Assume that -80 \({ }^{\circ} \mathrm{F}\) is accurate to two significant figures.) Text Transcription: ^circ F

The warmest temperature ever measured in the United States was 134 \({ }^{\circ} \mathrm{F}\) on July 10, 1913, in Death Valley, California. Convert that temperature to degrees Celsius and Kelvin. Text Transcription: ^circ F

Vodka does not freeze in the freezer because it contains a high percentage of ethanol. The freezing point of pure ethanol is -114 \({ }^{\circ} \mathrm{C}\). Convert that temperature to degrees Fahrenheit and Kelvin. Text Transcription: ^circ C

Liquid helium boils at 4.2 K. Convert this temperature to degrees Fahrenheit and Celsius.

The temperature in the South Pole during the Antarctic winter is so cold that planes cannot land or take off, effectively leaving the inhabitants of the South Pole isolated for the winter. The average daily temperature at the South Pole in July is -59.7 \({ }^{\circ} \mathrm{C}\). Convert this temperature to degrees Fahrenheit. Text Transcription: ^circ C

The coldest temperature ever recorded in Iowa was -47 \({ }^{\circ} \mathrm{F}\) on February 3, 1998. Convert this temperature to kelvins and degrees Celsius. Text Transcription: ^circ F

Complete the table.

Complete the table.

Calculate the amount of heat required to raise the temperature of a 65-g sample of water from 32 \({ }^{\circ} \mathrm{C}\) to 65 \({ }^{\circ} \mathrm{C}\). Text Transcription: ^circ C

Calculate the amount of heat required to raise the temperature of a 22-g sample of water from 7 \({ }^{\circ} \mathrm{C}\) to 18 \({ }^{\circ} \mathrm{C}\). Text Transcription: ^circ C

Calculate the amount of heat required to heat a 45-kg sample of ethanol from 11.0 \({ }^{\circ} \mathrm{C}\) to 19.0 \({ }^{\circ} \mathrm{C}\). Text Transcription: ^circ C

Calculate the amount of heat required to heat a 3.5-kg gold bar from 21 \({ }^{\circ} \mathrm{C}\) to 67 \({ }^{\circ} \mathrm{C}\). Text Transcription: ^circ C

If 89 J of heat are added to a pure gold coin with a mass of 12 g, what is its temperature change?

If 57 J of heat are added to an aluminum can with a mass of 17.1 g, what is its temperature change?

An iron nail with a mass of 12 g absorbs 15 J of heat. If the nail was initially at 28 \({ }^{\circ} \mathrm{C}\), what is its final temperature? Text Transcription: ^circ C

A 45-kg sample of water absorbs 345 kJ of heat. If the water was initially at 22.1 \({ }^{\circ} \mathrm{C}\), what is its final temperature? Text Transcription: ^circ C

Calculate the temperature change that occurs when 248 cal of heat are added to 24 g of water.

A lead fishing weight with a mass of 57 g absorbs 146 cal of heat. If its initial temperature is 47 \({ }^{\circ} \mathrm{C}\), what is its final temperature?

An unknown metal with a mass of 28 g absorbs 58 J of heat. Its temperature rises from 31.1 \({ }^{\circ} \mathrm{C}\) to 39.9 \({ }^{\circ} \mathrm{C}\). Calculate the heat capacity of the metal and identify it, referring to Table 3.4. Text Transcription: ^circ C

When 2.8 J of heat are added to 5.6 g of an unknown metal, its temperature rises by 3.9 \({ }^{\circ} \mathrm{C}\). Are these data consistent with the metal being gold? Text Transcription: ^circ C

When 56 J of heat are added to 11 g of a liquid, its temperature rises from 10.4 \({ }^{\circ} \mathrm{C}\) to 12.7 \({ }^{\circ} \mathrm{C}\). What is the heat capacity of the liquid? Text Transcription: ^circ C

When 47.5 J of heat are added to 13.2 g of a liquid, its temperature rises by 1.72 \({ }^{\circ} \mathrm{C}\). What is the heat capacity of the liquid? Text Transcription: ^circ C

Two identical coolers are packed for a picnic. Each cooler is packed with eighteen 12-oz soft drinks and 3 lb of ice. However, the drinks that went into cooler A were refrigerated for several hours before they were packed in the cooler, while the drinks that went into cooler B were at room temperature. When the two coolers are opened three hours later, most of the ice in cooler A is still ice, while nearly all of the ice in cooler B has melted. Explain.

A 100-g block of iron metal and 100 g of water are each warmed to 75 \({ }^{\circ} \mathrm{C}\) and placed into two identical insulated containers. Two hours later, the two containers are opened and the temperature of each substance is measured. The iron metal has cooled to 38 \({ }^{\circ} \mathrm{C}\) while the water has cooled only to 69 \({ }^{\circ} \mathrm{C}\). Explain. Text Transcription: ^circ C

How much energy (in J) is lost when a sample of iron with a mass of 25.7 g cools from 75.0 \({ }^{\circ} \mathrm{C}\) to 22.0 \({ }^{\circ} \mathrm{C}\)? Text Transcription: ^circ C

A sample of aluminum with mass of 53.2 g is initially at 155 \({ }^{\circ} \mathrm{C}\). What is the temperature of the aluminum after it loses \(2.87 \times 10^{3}\) J? Text Transcription: ^circ C 2.87 \times 10^{3}

245 mL of water with an initial temperature of 32 \({ }^{\circ} \mathrm{C}\) absorbs 17 kJ of heat. Find the final temperature of the water. (density of water = 1.0 g/mL) Text Transcription: ^circ C

32 mL of ethanol with an initial temperature of 11 \({ }^{\circ} \mathrm{C}\) absorbs 562 J of heat. Find the final temperature of the ethanol. (density of ethanol = 0.789 g/mL) Text Transcription: ^circ C

A pure gold ring with a volume of 1.57 \(\mathrm{cm}^{3}\) is initially at 11.4 \({ }^{\circ} \mathrm{C}\). When it is put on, it warms to final temperature of 29.5 \({ }^{\circ} \mathrm{C}\). How much heat (in J) does the ring absorb? (density of gold = 19.3 g/\(\mathrm{cm}^{3}\)) Text Transcription: ^circ C cm^3

A block of aluminum with a volume of 98.5 \(\mathrm{cm}^{3}\) absorbs 67.4 J of heat. If its initial temperature is 32.5 \({ }^{\circ} \mathrm{C}\), what is its final temperature? (density of aluminum = 2.70 g/\(\mathrm{cm}^{3}\)) Text Transcription: ^circ C cm^3

How much heat in kilojoules is required to heat 56 L of water from an initial temperature of 85 \({ }^{\circ} \mathrm{F}\) to a final temperature of 212 \({ }^{\circ} \mathrm{F}\)? (The density of water is 1.00 g/mL.) Text Transcription: ^circ F

How much heat in joules is required to heat a 43-g sample of aluminum from an initial temperature of 72 \({ }^{\circ} \mathrm{F}\) to a final temperature of 145 \({ }^{\circ} \mathrm{F}\)? (The density of water is 1.00 g/mL.) Text Transcription: ^circ F

What is the temperature change \((\Delta T)\) in Celsius when 29.5 L of water absorbs 2.3 kWh of heat? Text Transcription: Delta T

If 1.45 L of water has an initial temperature of 25.0 \({ }^{\circ} \mathrm{C}\), what is its final temperature after absorption of \(9.4 \times 10^{22}\) kWh of heat? Text Transcription: ^circ C 9.4 times 10^22

A water heater contains 55 gal of water. How many kilowatt-hours of energy are necessary to heat the water in the water heater by 25 \({ }^{\circ} \mathrm{C}\)? (Hint: \(\Delta T=25^{\circ} \mathrm{C}\)) Text Transcription: ^circ C Delta T=25^circ C

A room contains 48 kg of air. How many kilowatt-hours of energy are necessary to heat the air in the room from an initial temperature of 7 \({ }^{\circ} \mathrm{C}\) to a final temperature of 28 \({ }^{\circ} \mathrm{C}\)? The heat capacity of air is 1.03 J/g \({ }^{\circ} \mathrm{C}\). Text Transcription: ^circ C

A backpacker wants to carry enough fuel to heat 2.5 kg of water from 25 \({ }^{\circ} \mathrm{C}\) to 100.0 \({ }^{\circ} \mathrm{C}\). If the fuel she carries produces 36 kJ of heat per gram when it burns, how much fuel should she carry? (For the sake of simplicity, assume that the transfer of heat is 100% efficient.) Text Transcription: ^circ C

A cook wants to heat 1.35 kg of water from 32.0 \({ }^{\circ} \mathrm{C}\) to 100.0 \({ }^{\circ} \mathrm{C}\). If he uses the combustion of natural gas (which is exothermic) to heat the water, how much natural gas will he need to burn? Natural gas produces 49.3 kJ of heat per gram. (For the sake of simplicity, assume that the transfer of heat is 100% efficient.) Text Transcription: ^circ C

Evaporating sweat cools the body because evaporation is endothermic and absorbs 2.44 kJ per gram of water evaporated. Estimate the mass of water that must evaporate from the skin to cool a body by 0.50 \({ }^{\circ} \mathrm{C}\), if the mass of the body is 95 kg and its heat capacity is 4.0 J/g \({ }^{\circ} \mathrm{C}\). (Assume that the heat transfer is 100% efficient.) Text Transcription: ^circ C

When ice melts, it absorbs 0.33 kJ per gram. How much ice is required to cool a 12.0-oz drink from 75 \({ }^{\circ} \mathrm{F}\) to 35 \({ }^{\circ} \mathrm{F}\), if the heat capacity of the drink is 4.18 J/g \({ }^{\circ} \mathrm{C}\)? (Assume that the heat transfer is 100% efficient.) Text Transcription: ^circ F ^circ C

A 15.7-g aluminum block is warmed to 53.2 \({ }^{\circ} \mathrm{C}\) and plunged into an insulated beaker containing 32.5 g of water initially at 24.5 \({ }^{\circ} \mathrm{C}\). The aluminum and the water are allowed to come to thermal equilibrium. Assuming that no heat is lost, what is the final temperature of the water and aluminum? Text Transcription: ^circ C

A 25.0-mL sample of ethanol (density = 0.789 g/mL) initially at 7.0 \({ }^{\circ} \mathrm{C}\) is mixed with 35.0 mL of water (density = 1.0 g/mL) initially at 25.3 \({ }^{\circ} \mathrm{C}\) in an insulated beaker. Assuming that no heat is lost, what is the final temperature of the mixture? Text Transcription: ^circ C

The wattage of an appliance indicates its average power consumption in watts (W), where 1 W = 1 J/s. What is the difference in the number of kJ of energy consumed per month between a refrigeration unit that consumes 625 W and one that consumes 855 W? If electricity costs $0.15 per kWh, what is the monthly cost difference to operate the two refrigerators? (Assume 30.0 days in one month and 24.0 hours per day.)

A portable electric water heater transfers 255 watts (W) of power to 5.5 L of water, where 1 W = 1 J/s. How much time (in minutes) does it take for the water heater to heat the 5.5 L of water from 25 \({ }^{\circ} \mathrm{C}\) to 42 \({ }^{\circ} \mathrm{C}\)? (Assume that the water has a density of 1.0 g/mL.) Text Transcription: ^circ C

What temperature is the same whether it is expressed on the Celsius or Fahrenheit scale?

What temperature on the Celsius scale is equal to twice its value when expressed on the Fahrenheit scale?

Classify each as a pure substance or a mixture.

Classify each as a pure substance or a mixture. If it is a pure substance, classify it as an element or a compound. If it is a mixture, classify it as homogeneous or heterogeneous.

This molecular drawing shows images of acetone molecules before and after a change. Was the change chemical or physical?

This molecular drawing shows images of methane molecules and oxygen molecules before and after a change. Was the change chemical or physical?

Global warming refers to the rise in average global temperature due to the increased concentration of certain gases, called greenhouse gases, in our atmosphere. Earth’s oceans, because of their high heat capacity, absorb heat and therefore act to slow down global warming. How much heat would be required to warm Earth’s oceans by 1.0 \({ }^{\circ} \mathrm{C}\)? Assume that the volume of water in Earth’s oceans is \(137 \times 10^{7} \mathrm{~km}^{3}\) and that the density of seawater is \(1.03 \mathrm{~g} / \mathrm{cm}^{3}\). Also assume that the heat capacity of seawater is the same as that of water. Text Transcription: ^circ C 137 times 10^7 km^3 1.03 g cm^3

Examine the data for the maximum and minimum average temperatures of San Francisco and Sacramento in the summer and in the winter. (a) Notice the difference between the August high in San Francisco and Sacramento. Why is it much hotter in the summer in Sacramento? (b) Notice the difference between the January low in San Francisco and Sacramento. How might the heat capacity of the ocean contribute to this difference?

Using white and black circles to represent different kinds of atoms, make a drawing that accurately represents each of the following: a solid element, a liquid compound, a homogeneous mixture, and a heterogeneous mixture.

Make a drawing (clearly showing before and after) depicting your liquid compound from Question 120 undergoing a physical change. Make a drawing depicting your solid element undergoing a chemical change.

A friend asks you to invest in a new motorbike that he invented that never needs gasoline and does not use batteries. What questions should you ask before investing?

In a grammatically correct sentence or two (and in your own words), describe what heat and temperature have in common and how they are different. Make sure you are using the words correctly with their precise scientific meanings.

The graph at right shows U.S. energy consumption by source from 1980 to 2040 (based on projections). The consumption is measured in quadrillion BTUs or quads (1 quad = \(1.055 \times 10^{18}\) J). (a) What were the three largest sources of U.S. energy in 2013 in descending order? What total percent of U.S. energy do these three sources provide? (b) What percent of total U.S. energy is provided by renewables in 2013? (c) Which two sources of U.S. energy decline as a percentage of total energy use between 1989 and 2040 (based on projections)? (d) How much U.S. energy (in joules) was produced by nuclear power in 1990? Text Transcription: 1.055 times 10^18

A major event affecting global climate is the El Niño/La Niña cycle. In this cycle, equatorial Pacific Ocean waters warm by several degrees Celsius above normal (El Niño) and then cool by several degrees Celsius below normal (La Niña). This cycle affects weather not only in North and South America, but also in places as far away as Africa. Why does a seemingly small change in ocean temperature have such a large impact on weather?