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When the volume of an "ideal gas" increases AND the amount (number of moles*) of gas remains constant, the temperature of the gas will decrease.
One relevant assumption for an "ideal gas" is that it is "dry" - no water vapor (humidity) in the sample
One relevant equation is the Ideal Gas Law P*V = n*R*T
When P = pressure in atmospheres
V = volume in liters
n = amount of the Ideal Gas, in moles
R = the ideal, or universal, gas constant = 0.08206 L*atm / mol * K
which is read as "liter-atmospheres per mole-Kelvin"
T = the absolute temperature in K, "Kelvins"
*A "mole" is 6.022×1023 atoms or molecules of a substance.
This is known as "Avogadro's Number"
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