The kinetic energy of a gas molecule is proportional to its temperature. According to the kinetic theory of gases, the average kinetic energy of gas molecules is directly proportional to the absolute temperature of the gas.
As the gas's temperature increases, its thermal energy also increases. This is because temperature is a measure of the average kinetic energy of the gas particles, and as they move faster (due to higher temperature), they possess more kinetic energy and thus the thermal energy of the gas increases.
The average kinetic energy of a gas is directly proportional to its temperature. This is described by the kinetic theory of gases, which states that the average kinetic energy of gas molecules is directly related to the temperature of the gas. As temperature increases, the average kinetic energy of the gas molecules also increases.
The kinetic energy of a single gas molecule is not proportional to anything. The average kinetic energy of gas molecules is proportional to their absolute temperature.
Total molecular kinetic energy of a gas in a box is the sum of the kinetic energies of all individual gas molecules. Average molecular kinetic energy, on the other hand, is the average kinetic energy per molecule in the gas and is calculated by dividing the total kinetic energy by the number of molecules present in the box.
Its particles acquire greater kinetic energy.
The kinetic energy of a gas molecule is proportional to its temperature. According to the kinetic theory of gases, the average kinetic energy of gas molecules is directly proportional to the absolute temperature of the gas.
As the gas's temperature increases, its thermal energy also increases. This is because temperature is a measure of the average kinetic energy of the gas particles, and as they move faster (due to higher temperature), they possess more kinetic energy and thus the thermal energy of the gas increases.
The average kinetic energy of a gas is directly proportional to its temperature. This is described by the kinetic theory of gases, which states that the average kinetic energy of gas molecules is directly related to the temperature of the gas. As temperature increases, the average kinetic energy of the gas molecules also increases.
The kinetic energy of a single gas molecule is not proportional to anything. The average kinetic energy of gas molecules is proportional to their absolute temperature.
The particles of the substance gain kinetic energy as they absorb heat energy. Eventually there is enough kinetic energy for the particles to escape the liquid phase, forming the gas phase.
The particles of the substance gain kinetic energy as they absorb heat energy. Eventually there is enough kinetic energy for the particles to escape the liquid phase, forming the gas phase.
Kinetic energy of gas molecules is proportional to temperature.
Total molecular kinetic energy of a gas in a box is the sum of the kinetic energies of all individual gas molecules. Average molecular kinetic energy, on the other hand, is the average kinetic energy per molecule in the gas and is calculated by dividing the total kinetic energy by the number of molecules present in the box.
As atoms move from solid to liquid to gas, their kinetic energy increases. In the solid phase, atoms vibrate in fixed positions with low kinetic energy. In the liquid phase, atoms have more freedom to move around and their kinetic energy increases. In the gas phase, atoms have even more kinetic energy as they move freely and rapidly.
the pressure decreases D:
Kinetic energy increases when a liquid changes to a gas because the molecules in a gas have higher average kinetic energy compared to those in a liquid. When a liquid evaporates and becomes a gas, the molecules gain more energy and move faster, increasing their kinetic energy.