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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

Verified Answer :

Nirina7

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: \(16.28dm^3\)

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)

\(\frac{V_1}{T_1}=\frac{V_2}{T_2}\)

where V= volume

T= temperature in Kelvin

Given:  

\(V_1=15 dm^3\)

\(T_1=20^0C=20+273K=293K\)

\(V_2\)=?

\(T_1=318K\)

\(\frac{15dm^3}{293K}=\frac{V_2}{318K}\)

\(V_2=16.28dm^3\)


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