Question

If a gas sample has a pressure of 30.7 kpa at 0.00, by how many degrees celsius does the temperature have to increase to cause the pressure to double?

Answer 1

Answer: The temperature has to increase by
`273^0C`.

Step-by-step explanation:

Gay-Lussac's Law: This law states that pressure is directly proportional to the temperature of the gas at constant volume and number of moles.

`P\propto T` (At constant volume and number of moles)

`(P_1)/(T_1)=(P_2)/(T_2)`

where,

`P_1` = initial pressure of gas = 30.7 kPa

`P_2` = final pressure of gas =
`2* 30.7=61.4kPa`

`T_1` = initial temperature of gas =
`0^0C=(0+273)K=273K`

`T_2` = final temperature of gas = ?

`(30.7)/(273)=(61.4)/(T_2)`

`T_2=546K=(546-273)^0C=273^0C`

Therefore, the temperature has to increase by
`273^0C` to increase to cause the pressure to double.