Question

consider a gas at 0 degree C.at what temp. will be the volume doubled if the pressure is kept constant.

Answer 1

we know,
PV= nRT
According to question, P and n is constant and Temperature changes 0 degree C or 273K To temperature T, and V changes to 2V
So, V1=V, V2=2V, T1= 273K, T2=?
V1/V2=T1/T2
or, V/ 2V = 273K/ T2
or, T2= 2×273K = 546K = 273degree C

Answer 2

The volume will double at 546 K

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

$V_1$ = initial volume of gas = v

$V_2$ = final volume of gas = 2v

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

$T_2$ = final temperature of gas = ?

Now put all the given values in the above equation, we get the final pressure of gas.

$\frac{v}{273}=\frac{2v}{T_2}$

$T_2=546K=(573-273)^0C=273^0C$

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