Physics Fundamentals Quiz

Properties of objects or phenomena that can be measured.

Fundamental units of measurement in the International System of Units (SI).

A precise and agreed-upon definition or physical representation of the unit of length.

The SI unit of length, originally defined as one ten-millionth of the Earth's quadrant, then by an artifact, lastly by the wavelength of light.

To find and describe the laws governing natural phenomena.

Experimental observation and quantitative measurements.

Fundamental quantities like Length, Mass, and Time.

Quantities that are created from combinations of base units (e.g., velocity = distance/time).

A graphical representation showing the different phases (solid, liquid, gas) of a substance and the conditions under which they exist in equilibrium.

A phase change where the substance expands upon solidifying. Examples include water-bismuth mixtures.

A phase change where the substance contracts upon solidifying. Examples include CO2-O2 mixtures.

A physically distinct portion of a system, separated from other portions by bounding surfaces.

The minimum number of independent species needed to define the composition of all phases.

An equation (F = C - P + 2) that relates the number of degrees of freedom (F), components (C), and phases (P) in a system.

The number of independently variable factors affecting the system's state at equilibrium.

A system with only one degree of freedom: changing one variable affects other variables. In a phase diagram, this is represented by a line.

A system with zero degrees of freedom: all variables are fixed by the system's composition and the nature of the phases. In a phase diagram, this is a point.

Pressure can affect the melting or freezing point. Materials that contract during solidification require pressure to be less to favor solidification. Materials expanding during solidification require pressure to be higher to favor solidification.

The change in length of a material due to a change in temperature.

A material's ability to expand linearly with temperature.

The change in volume of a material due to a change in temperature.

A material's ability to expand in volume with temperature.

Final length = Initial length * (1 + αΔT).

Final volume = Initial volume * (1 + γΔT).

Some materials shrink when heated.

Water's density increases from 0°C to 4°C and then decreases.

A device to correct for thermal expansion effects.

Water's density reaches a maximum at 4°C before decreasing as temperature rises or falls.

Water's density is highest at 4°C, around 1 gram/cubic centimeter.

Certain materials contract when heated and expand when cooled, opposite of the typical behavior.

Issues arising from materials changing size due to temperature changes, like in dental fillings, optical components, and electronics.

Internal stress in a material arising from temperature changes and constraints.

Water molecules in the liquid state move freely.

Ice forms an open hexagonal structure.

Solid carbon dioxide.

Direct transition of a substance from solid to gas phase.

The energy a system possesses due to its temperature. For an ideal gas, internal energy is directly related to the temperature.

Energy transfer between a system and its surroundings. It's a measure of how much energy is put into, or taken out of, a system.

Thermal energy in motion. Heat flow is the transfer of thermal energy between objects of different temperatures.

The amount of heat necessary to raise the temperature of 1 gram of water by 1 degree Celsius (between 14.5 and 15.5°C).

A unit of energy. Applied for one meter of displacement with one newton of force.

The amount of heat transferred per unit of time due to a temperature difference.

Directly related to the internal energy of an ideal gas.

Energy cannot be created or destroyed, only changed from one form to another within a closed system.

A thermodynamic process that happens slowly enough for the system to remain in equilibrium at every step.

The integral of pressure (P) with respect to volume (V) from initial (Vi) to final volume (Vf). W = ∫P dV from Vi to Vf

A thermodynamic process that occurs at constant volume.

Zero. No work is done because the volume isn't changing.

The change in internal energy (ΔU) of a system is equal to the heat added (Q) minus the work done (W). ΔU = Q - W

The work done by a system in an isochoric process is zero.

The change in the total internal energy of a system

A process where no heat transfer occurs between the system and its surroundings.

The amount of heat required to raise the temperature of one mole of a substance by one degree Celsius/Kelvin at constant volume.

The amount of heat required to raise the temperature of one mole of a substance by one degree Celsius/Kelvin at constant pressure.