A sample of helium gas has a volume of `500 cm^(3)` at `373 K`. Calculate the temperature at which the volume become `260 dm^(3)`. Assume that pressure id kept constant.

Explanation

From the given data : `V_(1) = 500 cm^(3)` , `V_(2) = 260 cm^(3)`
`T_(1) = 373 K , T_(2) = ?`
Since the pressure of the gas is constant, Charles's law is applicable. Therefore,
`(V_(1))/(V_(2)) = (T_(1))/(T_(2))` or `T_(2) = (T_(1) xx V_(2))/(V_(1)) = ((373 K) xx (260 cm^(3)))/((500 cm^(3))) = 193.96 K`