3.7 Changes of State

• Changes of state include melting and freezing.

• The particles move faster when heat is added to a solid.

• Random pat processes separate the particles in the solid.

• The reverse process takes place if the temperature of a liquid is lowered.

• It takes 80 cal of heat to melt 1 g of ice.

• The amount of heat that must be removed to freeze 1 g of water at its freezing point is also known as the heat of fusion.

• The heat of fusion can be used as a conversion factor.
• The mass of ice in grams is used to determine the heat needed to melt it.
• Sample Problem 3.8 shows that there is no temperature change given in the calculation if the ice is melting.

• Sports trainers use ice bags to treat injuries.

• The given and needed quantities should be stated.

• An ice bag is used.

• To convert the given quantity to the needed quantity, you have to write a plan.

• Determine the needed quantity by setting up the problem.

• 125 g of water is placed in an ice cube tray.

• It's called "dry" because it doesn't form a liquid as it warms.
• The snow does not melt in cold areas.

• When frozen foods are left in the freezer for a long time, there is a lot of water.

• Water Vapor forms ice crystals on the surface of freezer bags and frozen food when they are deposition.

• For camping and hiking, freeze-dried foods are convenient.

• The dried food needs only water to be eaten.
• Freeze-dried foods do not need to be refrigerated.

• A reverse process takes place when heat is removed.

• boiling and condensation occur at the same temperature.
• When you take a hot shower, the water droplets form on a mirror, and con Try Practice Problems 3.47 densation occurs.

• Evaporation happens at the surface of a liquid.
• There are bubbles of gas in the liquid.

• 540 cal is needed to convert 1 g of water to liquid.

• When 1 g of water vapor changes to liquid at 100 degrees, the same amount of heat is released.

• The mass in grams is used to determine the heat needed to boil a sample of water.
• If the water is boiling, there is no temperature change in the calculation.

• The heating or cooling of a substance can be illustrated visually.

• The warming of a solid can be seen in the first diagonal line.
• A horizontal line indicates that the solid is melting.

• As Try Practice Problems 3.51 heat is added, a heating curve diagrams the temperature increases and changes of state.

• Adding more heat will increase the tempera ture of the liquid, which is shown as a diagonal line.
• When the liquid reaches its boiling point, a horizontal line shows that the liquid will change to gas.
• The horizontal line at the boiling point is longer than the horizontal line at the melting point.
• Adding more heat increases the temperature of the gas.

• A cooling curve is a diagram in which the temperature goes down.

• Water gas can form a liquid.

• We have calculated one step in a heating or cooling curve.
• Some problems require a combination of steps that include a temperature change and a change of state.
• The heat is calculated for each step separately and then added together to find the total energy, as seen in Sample Problem 3.9.

• Charles is doing more exercise.
• He had a sore arm after using weights.
• 125 g of ice is in an ice bag.

• The given and needed quantities should be stated.

• To convert the given quantity to the needed quantity, you have to write a plan.

• Determine the needed quantity by setting up the problem.

• Hot water can cause burns and damage to the skin.

• It's even more dangerous if you get steam on the skin.
• The temperature of the water will drop to body temperature if 25 g of hot water falls on a person's skin.

• Severe burns were caused by 64 000 J of heat released.

• The amount of heat released from steam is ten times greater than the amount of hot water.

• The same amount of steam to liquid releases more heat.
• The heat released when steam condenses can be calculated using the heat of vaporization, which is 2260 J/g.

• The total heat released is calculated by combining the heat from condensation at 100 degC and the heat from cooling the steam from 100 degC to 37 degC.
• Most of the heat comes from the condensation of steam.

• 2 260 J or 540 cal is released when 1 g of steam condenses.

• The energy was taken up by 0 degC.

• The water becomes solid at 0 degrees.

• The clouds have water in them.

• Dry ice becomes gas.

• Clothes are wet on a clothesline.

• The steam forms when lava flows into the ocean.

• There is snow on the ground.

• 125 g of liquid water has heat removed.

• The water in a pan can change to steam.

• The water is ready for tea.

• Draw a heating curve for a sample of ice that is heated and then cooled to 150 degrees.

• The amount of heat warms to body temperature can be calculated using the values for the heat of fusion, specific heat of water, and heat of vaporization.

• Daniel will keep a diary of his weight if Charles consumes 1800 kcal per day.

• The mixture should be identified.

• Pure substances are classified as mixtures.

• Pure substances are elements, compounds, liquid, and gas.

• When physical properties change, but not methods, a physical change occurs.

• There are 180 units between the freezing liquids and gases, and the reezing point and the boiling point of water.
• The energy was released or absorbed.

• C + 32.

• C + 273.

• Evaporation occurs when particles in a liquid state absorb enough potential to break apart and form gaseous particles.

• A boiling point is the point at which liquid becomes liquid.
• The amount of heat needed to convert 1 g of air into 1 g of liquid is called the heat of vaporization.

• 540 cal (2260 J) is needed to vaporize 1 g of water or the energy of motion.

• The cal, kcal, and j are the common units of energy.

• The number of calories is equal to 4.184 J.

• The calories from Fat 40 is 130 calories for every 500 kJ of energy.

• The amount of calories in a food is called the energy of a food.

• The temperature at which a liquid changes to gas with a definite composition can be broken down into boiling and gas changes to liquid.

• As heat is removed, one state of matter is transformed into another.

• A pure substance containing only one type of matter can't be broken down by chemical methods.

• The ability to work.

• To change into a new substance, the kilojoules are obtained per gram.

• Mass and energy particles from the surface of a liquid are what makes up a substance.

• The state is changed from liquid to solid.

• The temperature at which a solid becomes a solid is known as the freezing temperature.

• It's the same temperature as the freezing point.

• A state of matter that does not have a definite shape.

• The motion of particles in a substance has an energy associated with it.

• A change in the physical properties of a sub.
• It is necessary to melt stance change but its identity stays the same.

• When 1 g of water is frozen, 80. cal is released.

• The identity of a substance is not affected by the amount of energy required.

• 540 cal of a substance is given off by 1 g of steam and 1 g of liquid.

• A type of matter with a definite composition.

• A state of matter with its own shape and volume.

• The SI unit of heat energy is 4.184 J.

• The particles have energy.

• A solid is transformed into a volume.

• C is the identity of a substance.

• Chemical properties describe the ability of a substance to change into a new substance.

• Equalities for energy units include 1 cal and ance changes, but its composition remains the same.

• Each equality for energy units can be written as two conversions into a new substance, which has different physical and chemical properties.

• There is a gas in a balloon.

• It smells like rotten eggs.

• We start with the given property using the conversion factors above.

• 45 000 J should be converted to kilo calories.

• When methane burns, it changes to different substances with new properties, which is a chemical property.

• The smell of hydrogen sulfide is a physical property.

• The heat equation is used to convert.

• When the specific heat of a substance Celsius toKelvin is used, heat, in calories, is obtained.

• The J/g degC is used.

• For temperature change, C + 32.

• You can convert 355 K to degrees Celsius.

• The heat equation is made up of the known values and the boiling/condensation point heat.

• For example, 2260 J of heat is needed to boil (condense) g degC exactly 1 g of water/steam at its boiling (condensation) point.

• 104 kJ 1 g of ice is at its melting point.

• If you want to convert the temperature to Fahrenheit, you need to state it on the thermometer.

• Grass clippings, kitchen scraps, and dry leaves can be used to make compost.

• A mixture of salicylic acid and methanol was heated for two hours in a chemical reaction.

• Use Table 3.7 to calculate the total kilocalories for each iron and copper, each with a volume of 100.0 cm3 from 25 degC food type in this meal.
• Based on your location.

• Determine the total kilo calories for the meal.

• Table 3.10 shows the number of hours of sleep needed to burn off the kilo calories in this meal.

• Table 3.10 shows the number of hours needed to burn off the kilo calories in this meal.

• A friend of yours has a slice of pizza, a soft drink, and ice cream.

• A person had a quarter-pound cheeseburger, french fries, and a chocolate shake.

• Determine the number of hours of sitting needed to burn off the kilo calories in this meal.

• Table 3.10 shows the number of hours needed to burn off the kilo calories in this meal.

• There is a silvery shiny appearance to Mercury.

• There is a liquid in the room.

• The heterogeneous volume of mercury is used as a thermometric liquid.

• A red solid is formed when Mercury reacts with yellow sulfur.

• After cutting, apples turn brown.

• An embryo is created by a fertilized egg.

• Under the sun, clothes are dried.

• Egg white is set.

• Aspirin is broken in half.

• Carrots can be used in a salad.

• Beer is made through the process of beer making.

• A copper pipe is green.

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• In Rodgers Pass, Montana, on January 20, 1954.

• On July 21, 1983, the world's lowest temperature was recorded in Vostok.

• A sample of vegetable oil is placed in a calorimeter.

• 18.9 kJ is given off when the sample is burned.

• A sample of rice is placed in a calorimeter.
• 22 kJ is given off when the sample is burned.

• On a hot day the sand gets hot but the water stays cool.

• 140 g of compound Z water stays cool because of the absorption of 11.2 kcal of energy.

• The metal chair is very hot and the melting point of benzene is very cold.
• Do you think the specific is 80.1 degC?

• There are problems related to the topics in this chapter.

• A sample of steam is coming from a volcano.

• It condenses, cools, and falls as snow.
• A sample of water is added to a piece of ice at 0.0 degrees Centigrade and the metal is 29.2 degrees Centigrade.
• The steam boiler heating system in the large building uses oil.

• The amount of oil that can be burned is 1.0 lbs.

• It is thought that a metal is silver or iron.

• 11 kcal is released when 1.0 g of gasoline burns.

• The metal is thought to be gold or titanium.
• When 1.0 gal of gaso absorbs 30.8 cal, its temperature rises by 50 degC.

• The temperature is equivalent to 39 degrees.

• Potential energy changes as it descends.

• The amount of heat added increases.
• Solid to liquid or melting of the substance.

• The liquid state is represented by C. The horizontal line D shows the change from liquid to gas.

• Charles should be losing weight.

• Native gold can be found in streams and mines.

• It is 35 miles per gallon.

• The particles are moving at a slower pace in the diagram.

• It will take a long time for the energy bar's label to be released.

If the density of gasoline is 0.74 g/mL, what is the mass?

• 47 kJ of energy is released when 1.00 g of gasoline burns.

• What are the kilojoules for the animal.

• There are 75 iron nails in one box.

• A hot tub has 450 gal of water.

• The iron density is 7.86 g/ cm3.
• The heat of iron is 3.4, 3.5 and 0.452 J/g.
• The melting point of iron is 1535 degrees.