temperature definition instrument scales temperature is associated with heat but it is not heat. it...
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• Temperature • Definition• Instrument• Scales
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TEMPERATURE
• Is associated with heat but it is NOT HEAT. IT IS NOT A FORM OF ENERGY!!!!
• ( Heat is)
• Review: What is KINETIC ENERGY?
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KINETIC ENERGY (KE)
• Is associated with movement. • If an object is moving fast has high KE• If an object is moving slowly it has low KE
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Temperature• In scientific
measurements, the Celsius and Kelvin scales are most often used.
• The Celsius scale is based on the properties of water.□ 0C is the freezing point of
water.□ 100C is the boiling point
of water.
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Temperature:
A measure of the average kinetic energy of the particles in a sample.
If an object is at HIGH temperature its particles are moving FAST
At LOW temperature particles move SLOWLY
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Instrument to measure temperature
THERMOMETER
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FIXED POINTS OF A THERMOMETER
• BOILING POINT OF WATER
• FREEZING POINT OF WATER
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Temperature
• The Kelvin is the SI unit of temperature.
• It is based on the properties of gases.
• There are no negative Kelvin temperatures.
• K = C + 273.15
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Temperature
• The Fahrenheit scale is not used in scientific measurements.
• F = 9/5(C) + 32• C = 5/9(F − 32)
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2. SI unit for temp. is the Kelvin
a. K = C + 273 (10C = 283K)
b. C = K – 273 (10K = -263C)
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DO NOW
1. What is 35ºC in Kelvin?
2. What is 10 K in ºC?
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What is the temperature of the beakers?
• Which one needs more heat to boil?
• What is the difference between heat and temperature?
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• What is the relationship between heat and temperature?
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1. Temperature is the average kinetic energy of the particles in a substance.
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Heat and Temperature
• The temperature of an object tells us how HOT the object is. It is measured in degrees Celsius - °C, with a thermometer.
• Temperature is NOT a form of energy.• HEAT IS A FORM OF ENERGY!!!
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So how temperature and heat are related?
• Temperature is NOT the same as HEAT ENERGY although the two quantities are related.
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They are both a the same temperature. Which contains more
heat?
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• Types of energy
• POTENTIAL ENERGY :
STORED ENERGY. The energy inside the substance.
• KINETIC ENERGY : Associated with motion.
Average KE = TEMPERATURE
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HEAT
• The form of ENERGY that flows between two samples of matter due to their difference in temperature.
• It is measured in Joules. Other units are calories and kJ.
• It cannot be measured directly!
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Heat
Heat always flows from warmer (HIGH T) to cooler(LOW T) objects.
Ice gets warmer while hand gets cooler
Cup gets cooler while hand gets warmer
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Energy
• The ability to do work.• Energy is measured in Joules (J)• Any change re quires energy. Changes can
be Exothermic or Endothermic• Exothermic changes- release or give off
heat while they occur. (condensation, freezing)
• Endothermic changes Absorb heat as they occur (melting, boiling)
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ENERGY AND CHEMICAL REACTIONS
• EXOTHERMIC REACTIONS: reactions that RELEASE heat as they occur. Example: any combustion.
• ENDOTHERMIC REACTIONS: reactions that ABSORB heat energy as they occur.
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Heating and Cooling
• If an object has become hotter, it means that it has gained heat energy.
• If an object cools down, it means it has lost energy
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6. Specific Heat
a. Some things heat up or cool down faster than others.
Land heats up and cools down faster than water
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HEAT CAPACITY
• The amount of heat needed to increase the temperature of a material by 1oC. It depends on the MASS and the CHEMICAL COMPOSITION of the material.
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SPECIFIC HEAT CAPACITY
• The amount of heat needed to increase the temperature of 1 g of substance by 1 C.
• Depends only on the chemical composition.
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SPECIFIC HEAT CAPACITY
MATERIAL SPECIFIC HEAT J/g C
Water 4.18
Alcohol 2.43
Aluminum 0.90
Iron 0.45
Lead 0.13
Sand 0.83
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Why does water have such a high specific heat?
Water molecules form strong bonds with each other; therefore it takes more heat energy to break them. Metals have weak bonds
and do not need as much energy to break them.
water metal
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How to calculate changes in HEAT
The heat absorbed or released in a chemical reaction
Q = m x T x CpQ = HEAT
m = mass of substance
T = change in temperature (Tf – Ti)
Cp = specific heat of substance
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Calorimeter
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Bomb Calorimetry
A more sophisticated model is the bomb calorimeter, it has a chamber where a chemical reaction takes place and a device to start the reaction.
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HW answers• 1) 42000 J• 2) 6300J• 3) 5 C• 4) 20 C• 5) 336 g• 6) 14700 J =14.7 kJ• 7) 14.24 %• 8) b • 9)b 10 7J (d)
1) 1
2) 4
3) 3
4) 4
5) 3
6) 3
7) 2
8) 2
9) 4
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Aim: How to determine the melting point of a substance?
Challenge: To determine the melting point of water.
Your write up should include the following components: I. TITLE
II. PURPOSE
III. MATERIALS-
IV. PROCEDURE
V. DATA
VI. CALCULATIONS/GRAPH
VII.CONCLUSION (including a discussion of sources of error.)
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What is the freezing point of water?
• How would the mass of the sample affect the melting point? Explain.
• Describe the steps needed to determine the boiling point of water.
• Describe the phase changes that take place as water melts and as water boils.
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Vocabulary
• condensation• deposition• freezing• fusion• gaseous phase• heat• heat of fusion• heat of vaporization• kinetic molecular theory
• sublimation• temperature• vaporization• solidification• melt• solid phase• liquid phase
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October 17
• Objective: What are the characteristics of each state of matter?
• How to determine the amount of heat needed to change state?
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Phases of Matter
• The structure and arrangement of particles and their interactions determine the physical state of a substance at a given temperature and pressure.
• The three phases of matter (solids, liquids, and gases) have different properties.
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States of Matter
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States of Matter.
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Particle diagrams
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Phase Change
• DURING A PHASE CHANGE TEMPERATURE REMAINS CONSTANT
• Phase changes• Melting or Fusion: Phase change from
solid to liquid. Endothermic.• Vaporization – Phase change from liquid to
gas. It occurs during boiling. Endothermic.
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Phase Changes
• Evaporation: from liquid to gas. It occurs at all temperatures and ONLY at the surface of the liquid. Endothermic.
• Condensation: From gas to liquid. Exothermic.
• Freezing, solidification or crystallization: from liquid to gas. Exothermic.
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Special Phase Changes
• Sublimation: from solid directly to gas without changing to liquid first.
• Dry Ice CO2 (s) --> CO2 (g)
• Iodine I2 (s) --> I2 (g)
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Special Phase Changes
• Deposition: From gas to solid without going to liquid state.
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Special Phase Changes
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HEAT OF FUSION FOR WATER (TABLE B)
• Amount of heat needed to completely melt 1g of water (ice!).
• 334 J/g• 334 Joules of heat are necessary to
completely melt 1 g of water.• HOW MUCH HEAT IS NEEDED TO
MELT 10 g OF WATER?
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HEAT OF VAPORIZATION FOR WATER (TABLE T)
• The amount of heat needed to completely vaporize one g of water at its boiling point.
• 2260 J/g
• Water needs 2260 J of heat per gram to convert to gas!
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Summarizing
When there is a change in temperature use
Q = m x C x T
While the substance is melting/freezing use
Q = m x H f
While the substance is boiling/condensing use
Q = m x H vap
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Do now!
• How much heat is needed to completely melt 10 g of ice at 0 0 C ?
• How much heat is needed to vaporize 10 g of water at 100 0 C ?