The speed of monatomic gas particles is directly proportional to their temperature. As the temperature of a gas increases, the average speed of its particles also increases. This is known as the "kinetic theory of gases."
The equation for the relationship between gas speed and temperature is known as the "Maxwell-Boltzmann distribution." It states that the average speed of gas particles (v) is equal to the square root of (3RT/M), where R is the gas constant, T is the temperature in Kelvin, and M is the molar mass of the gas.
Changing the temperature of a gas will directly impact the average speed of its particles. As the temperature increases, the particles will move faster, and as the temperature decreases, the particles will slow down.
No, the relationship between gas speed and temperature varies depending on the type of gas. It is different for monatomic, diatomic, and polyatomic gases, as well as for gases with different molar masses.
The size of gas particles does not affect their speed and temperature relationship. This relationship is solely dependent on the temperature and molar mass of the gas particles, not their size or shape.