Question

A gas occupies a volume of 40.0 milliliters at 20°C. If the volume is increased to 80.0 milliliters at constant pressure, the resulting temperature will be equal to ?

Answer 1

Knowing that volume is directly proportional to Kelvin temperature and that, in this situation, the final volume is double the initial volume, the final temperature (in Kelvin) should be double the initial temperature (in Kelvin).

`20\textdegree\text{ C}=2\overline93.15 \text{ K}\\2(2\overline93.15 \text{ K})=5\overline86.3 \text{ K}=3\overline13.15\textdegree\text{ C}=310\textdegree\text{ C}`

Answer 2

Answer : The resulting temperature of gas will be, 580 K

Explanation :

Charles' Law : It is defined as the volume of gas is directly proportional to the temperature of the gas at constant pressure and number of moles.

`V\propto T`

or,

`(V_1)/(V_2)=(T_1)/(T_2)`

where,

`V_1` = initial volume of gas = 40.0 mL

`V_2` = final volume of gas = 80.0 mL

`T_1` = initial temperature of gas =
`20.0^oC=273+20.0=293K`

`T_2` = final temperature of gas = ?

Now put all the given values in the above formula, we get the final temperature of the gas.

`(40.0mL)/(80.0mL)=(290K)/(T_2)`

`T_2=580K`

Therefore, the resulting temperature of gas will be, 580 K