To what temperature should 2.3L of a gas at 25degree Celsius be heated in order to expand its volume to 4 L under constant pressure

518.52K

Explanation:

Charles law, which describes the direct relationship between the volume and the temperature of a gas when the pressure is constant, will be used for this question. The Charles law equation is:

V1/T1 = V2/T2

Where; V1 is the volume of the gas at an initial state (Litres)

T1 is the absolute temperature of the gas at an initial state (Kelvin)

V2 is the volume of the gas at a final state (Litres)

T2 is the absolute temperature of the gas at a final state (Kelvin)

According to the question, V1 = 2.3L, T1 = 25°C, V2 = 4L, T2 = ?

We need to convert the temperature to the absolute temperature unit in Kelvin (K) i.e.

T(K) = T(°C) + 273.15

T(K) = 25°C + 273.15

T1 (K) = 298.15K

To find for T2 in the equation, we make T2 the subject of the formula:

T2 = V2 × T1 / V1

T2 = 4 × 298.15 / 2.3

T2 = 1192.6/2.3

T2 = 518.52

Thus, the temperature must be heated to 518.52K in order to expand to a volume of 4L. This answer is in accordance to Charles law that the volume increases with increase in temperature and vice versa.

if the temperature drops and becomes cool

then the atmosphere can be freezing as the water vapor in the air is at maximum (100%) and can be severely cold

also can be snowing lightly as the moisture in the air will start to solidify

and btw this is not chemistry but