Thermal Energy Quiz

<p>Temperature is related to the average kinetic energy of the molecules. (C)</p> Signup and view all the answers

<p>The sum of all kinetic and potential energies within a substance. (D)</p> Signup and view all the answers

<p>Chemical or nuclear potential energy in bonds. (D)</p> Signup and view all the answers

<p>Conduction (A)</p> Signup and view all the answers

<p>Joules (J) (B)</p> Signup and view all the answers

<p>The direct transfer of kinetic energy through particle collisions. (C)</p> Signup and view all the answers

<p>Hotter fluids are less dense and rise, while colder fluids are more dense and sink. (D)</p> Signup and view all the answers

<p>Radiation does not require physical contact or a fluid medium, while conduction and convection do. (B)</p> Signup and view all the answers

<p>The theoretical point where molecules have the lowest energy, absolute zero. (C)</p> Signup and view all the answers

<p>It allows heat to move through it easily. (A)</p> Signup and view all the answers

<p>Convection involves a net transfer of matter, while conduction does not. (C)</p> Signup and view all the answers

<p>Radiation (A)</p> Signup and view all the answers

<p>They both have the same magnitude. (B)</p> Signup and view all the answers

<p>Either degrees Celsius (°C) or Kelvin (K) (D)</p> Signup and view all the answers

<p>Latent heat (C)</p> Signup and view all the answers

<p>The temperature remains constant (D)</p> Signup and view all the answers

<p>The intermolecular bonding energy (C)</p> Signup and view all the answers

<p>The heat energy released or absorbed per unit mass during a phase change (C)</p> Signup and view all the answers

<p>The latent heat of vaporization or fusion (C)</p> Signup and view all the answers

<p>Energy is released as intermolecular bonds form (C)</p> Signup and view all the answers

<p>Break the intermolecular bonds between the molecules (B)</p> Signup and view all the answers

<p>Q = mL (D)</p> Signup and view all the answers

<p>Both Q = mL and Q = mcΔT (D)</p> Signup and view all the answers

<p>5000 J (D)</p> Signup and view all the answers

<p>Q = mcΔT for ice heating, then Q = mL for melting (A)</p> Signup and view all the answers

<p>Qlost = Qgained (D)</p> Signup and view all the answers

<p>Its resistance to changes in temperature. (C)</p> Signup and view all the answers

<p>The temperature difference between initial and final states. (B)</p> Signup and view all the answers

<p>It requires a large amount of heat to cause a temperature change. (A)</p> Signup and view all the answers

<p>Q in Joules, m in kilograms, c in J/kg°C, and ΔT in °C or kelvin. (C)</p> Signup and view all the answers

<p>Heat transfer causes a change in the average kinetic energy of the molecules, which results in a temperature change. (A)</p> Signup and view all the answers

<p>10 K (D)</p> Signup and view all the answers

<p>$c = \frac{1}{\text{gradient} \times \text{mass}}$ (A)</p> Signup and view all the answers

<p>Either degrees Celsius (°C) or kelvins (K) (C)</p> Signup and view all the answers

<p>$\Delta U = Q + W$ (C)</p> Signup and view all the answers

<p>Negative (-W) (B)</p> Signup and view all the answers

<p>600 J (C)</p> Signup and view all the answers

<p>Its total energy remains constant over time. (C)</p> Signup and view all the answers

<p>450 J (A)</p> Signup and view all the answers

The theory stating that all matter is composed of tiny, constantly moving particles that collide and exchange energy.

The average kinetic energy of the particles within a substance. Measured in Celsius (°C) or Kelvin (K).

The transfer of thermal energy between two systems at different temperatures that come into contact.

The total energy of a substance, including kinetic and potential energy of its molecules. Does not include chemical or nuclear energy.

The total kinetic and potential energy of the moving atoms and bonds within an object. Does not include chemical or nuclear potential energy.

The transfer of heat through direct contact between particles of matter.

Heat transfer through electromagnetic waves, which can travel through a vacuum. All objects with heat energy emit these waves.

The SI unit for thermodynamic temperature. It starts at absolute zero, the point where molecules have the lowest energy.

The absolute zero point, where the molecules of a substance have the lowest energy.

The difference between the freezing and boiling points of water on the Celsius or Kelvin scale.

The quantity of heat required to raise the temperature of a substance by one degree Celsius.

The degree Celsius, symbol °C, is a unit of temperature equal in magnitude to the Kelvin (K). Temperature differences or intervals can be expressed in either Kelvin or degrees Celsius.

The formula that converts Celsius (TC) to Kelvin (TK): TK = TC + 273

When a system gains or loses heat energy, the average kinetic energy of its molecules changes, leading to a change in temperature unless there is a phase change.

Specific heat capacity describes a material's ability to store internal energy. It's like 'thermal inertia,' resisting changes in temperature.

This equation calculates the heat (Q) absorbed or released by a substance, based on its specific heat capacity (c), mass (m), and temperature change (ΔT).

The change in temperature (ΔT) can be expressed in either Kelvin or degrees Celsius, as they have the same magnitude.

Specific heat capacity (c) is the inverse of the gradient, calculated by dividing 1 by the product of mass and the gradient.

The amount of heat needed to raise the temperature of a cup (250g) of water from 18°C to 87°C can be calculated using the heat calculation equation, considering the specific heat capacity of water (4180 J/kg°C). The answer is approximately 72 kJ.

The amount of energy required to change the state of a substance from solid to liquid (melting) or liquid to gas (boiling) at a constant temperature.

The specific latent heat of fusion is the amount of heat energy required to change 1 kg of a substance from solid to liquid at its melting point.

The specific latent heat of vaporization is the amount of heat energy required to change 1 kg of a substance from liquid to gas at its boiling point.

The energy required to change the state of a substance from solid to liquid (melting) or liquid to gas (boiling) at a constant temperature.

The energy required to change the state of a substance from liquid to gas at a constant temperature.

A phase change occurs when a substance changes state, for example, from solid to liquid (melting) or liquid to gas (boiling).

During a phase change, heat energy is used to break or form intermolecular bonds between molecules. This means the average kinetic energy of the molecules, and therefore the temperature, remains constant.

The formula used to calculate the heat energy (Q) involved in a phase change., Q = mL, where Q is the heat energy (J), m is the mass (kg) and L is the latent heat (J/kg).

The amount of heat required to change the state of 1 kg of a substance without a change in temperature. Think of it as the energy needed to break bonds holding the substance together in a particular state.

During a phase change, the heat energy added or removed is used to change the state of the substance, not its temperature. This is calculated using Q = mL, where Q is the heat energy transferred, m is the mass, and L is the specific latent heat.

When a substance undergoes both a temperature change and a phase change, you need to calculate the heat energy for both processes separately and then add them together to get the total heat energy transferred.

The principle of conservation of energy applied to heat transfer. It states that the total heat energy lost by a system is equal to the total heat energy gained by another system.

A graphical representation of how the temperature of a substance changes over time as heat is added to it. It shows distinct sections for temperature changes and phase changes.

The change in internal energy of a system (ΔU) is equal to the Heat added to the system (Q) plus the work done on the system (W).

The total energy of an isolated system in a given frame of reference remains constant over time. This means energy cannot be created or destroyed, only transformed.

The thermal energy added to a system is positive (+Q), while the thermal energy removed or wasted from a system is represented as negative (-Q).

Work done by a system is negative (-W), and work done on a system is positive (+W). This is related to the direction of energy flow.

The ratio of output work to input heat for engines; expresses the percentage of heat that becomes useful work. Higher thermal efficiency means more useful work output.