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Questions and Answers
During a phase change, such as melting ice, what happens to the temperature of the substance as energy is continuously added?
During a phase change, such as melting ice, what happens to the temperature of the substance as energy is continuously added?
- The temperature fluctuates randomly as the substance transitions between phases.
- The temperature increases linearly with the added energy.
- The temperature remains constant as the energy is used for the phase transformation. (correct)
- The temperature decreases until the phase change is complete.
If Substance A has a higher specific heat capacity than Substance B, what does this indicate about the energy required to raise their temperatures?
If Substance A has a higher specific heat capacity than Substance B, what does this indicate about the energy required to raise their temperatures?
- Substance A requires more energy to achieve the same temperature change. (correct)
- Substance A requires less energy to achieve the same temperature change.
- The energy requirement is solely dependent on the mass of the substances, not the specific heat capacity.
- Substance A and B require equal amounts of energy to achieve the same temperature change.
A metal block requires 5000 J of energy to raise its temperature by 2°C. If the block's mass is 5 kg, what is the specific heat capacity of the metal?
A metal block requires 5000 J of energy to raise its temperature by 2°C. If the block's mass is 5 kg, what is the specific heat capacity of the metal?
- 1000 J/kg⋅K
- 1250 J/kg⋅K
- 250 J/kg⋅K
- 500 J/kg⋅K (correct)
Which of the following best describes 'specific latent heat of fusion'?
Which of the following best describes 'specific latent heat of fusion'?
During the melting of a solid, what happens to the energy supplied to the substance?
During the melting of a solid, what happens to the energy supplied to the substance?
If 334,000 J of energy is required to melt 1 kg of ice at 0°C, what is the specific latent heat of fusion of ice?
If 334,000 J of energy is required to melt 1 kg of ice at 0°C, what is the specific latent heat of fusion of ice?
In which state of matter do particles have the weakest intermolecular forces?
In which state of matter do particles have the weakest intermolecular forces?
What is the main difference between latent heat of fusion and latent heat of vaporization?
What is the main difference between latent heat of fusion and latent heat of vaporization?
Flashcards
States of Matter
States of Matter
Solid, liquid, and gas. Determined by molecule separation, intermolecular force and kinetic energy.
Internal Energy
Internal Energy
The sum of all potential and kinetic energy of all particles in a substance.
Specific Heat Capacity
Specific Heat Capacity
Energy needed to raise 1 kg of a substance by 1 degree Celsius.
Specific Heat Capacity Formula
Specific Heat Capacity Formula
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Specific Latent Heat of Fusion
Specific Latent Heat of Fusion
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Latent Heat of Fusion Formula
Latent Heat of Fusion Formula
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Flat Section on Time-Temperature Graph
Flat Section on Time-Temperature Graph
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Specific Latent Heat of Vaporization
Specific Latent Heat of Vaporization
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Study Notes
- There are three states of matter: solids, liquids, and gases.
- Each state of matter has unique properties.
- Separation between molecules, intermolecular force, and available kinetic energy determine a substance's state.
- Solids have closely packed particles and the strongest intermolecular force.
- Gases have the weakest intermolecular force.
- Matter can transition between states.
- Temperature remains constant during a state change as energy is used for the transformation.
- Internal energy is the sum of all potential and kinetic energy of all particles in a substance.
Thermal Energy Transfers (Specific Heat Capacity)
- Different materials have different heat capacities.
- Specific heat capacity is used to compare heat capacities.
- Specific heat capacity is the energy transfer needed to raise the temperature of 1 kg of a substance by one degree.
Specific Heat Capacity Formula
- c = Q / mΔT
- m = mass of the substance.
- c = specific heat capacity of the substance.
- ΔT = the difference in temperature (final temperature minus initial temperature).
- Specific heat capacity is measured in J/kg K (Joules per kilogram-kelvin).
Thermal Energy Transfers (Specific Latent Heat of Fusion)
- Specific latent heat of fusion is the energy transferred when 1 kg of a substance changes phase.
Latent Heat of Fusion Formula
- L = Q/m
- L = specific latent heat of fusion
- Q = energy transferred
- m = mass of the substance
- Latent heat is measured in J/kg
Activities Example
- When crushed ice at -10°C is heated in a container, temperature is recorded over time.
- A flat section on a time-temperature graph indicates a change of state, such as ice to water.
- The heat supplied changes ice from solid to liquid, breaking bonds between molecules during the phase change.
- Fusion applies to phase changes between solid to liquid and liquid to solid.
Thermal Energy Transfers (Specific Latent Heat of Vaporization)
- Specific latent heat of vaporization is the energy transferred when 1 kg of a substance changes from one phase to another.
Latent Heat of Vaporization Formula
- L = Q/m
- L is the specific latent heat of vaporization.
- Q is the energy transferred.
- m is the mass of the substance.
Thermal Energy Transfer
- Thermal energy transfers from hot to cooler areas through conduction, convection, and radiation.
Conduction
- Energy transfer mainly takes place without the actual movement of atoms.
- Conduction occurs through atomic vibrations and free electron collisions.
- Metals are good conductors because of the high number of de-localized electrons.
Convection
- Energy transfer occurs with the actual movement of atoms due to variation in density.
- Convection explains land and sea breezes.
- Winds are driven by the uneven heating of the Earth's surface.
Radiation
- Radiation is the only method of thermal energy transfer that doesn't require matter.
- Radiation involves the transfer of heat by electromagnetic radiation, generally in the infrared region.
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Description
Explore the three states of matter—solids, liquids, and gases—and their unique properties. Learn how intermolecular forces and kinetic energy influence these states. Understand the concept of specific heat capacity and its formula for calculating energy transfer in materials.
