Question

at 20°C , the volume of chlorine gas is 15 dm3 . Compute for the resulting volume if the temperature is adjusted to 318 K provided that the pressure remains the same

Answer 1

applying boyles' Combined gas Law:
(P1)(V1) / T1= (P2)(V2)/T2
T1= 20°C=20°+273= 293K
T2=318K
V1=15 dm^3
V2=?
the pressure remains the same, that means P1 = P2
so (P1)(V1) / T1= (P2)(V2)/T2 implies (V1) / T1= (V2)/T2 (P1 and P2 are simplified)
finally V2= V1 x T2/ T1= 15*318/293=16.27dm^3

Answer 2

Answer:
`16.28dm^3`

Explanation: Charles' Law: This law states that volume is directly proportional to the temperature of the gas at constant pressure and number of moles.

`V\propto T` (At constant pressure and number of moles)

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

where V= volume

T= temperature in Kelvin

Given:

`V_1=15 dm^3`

`T_1=20^0C=20+273K=293K`

`V_2`=?

`T_1=318K`

`(15dm^3)/(293K)=(V_2)/(318K)`

`V_2=16.28dm^3`