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A rigid plastic container holds 1.00 l methane gas at 660 torr pressure when the temperature is 22.0 degrees Celsius. How much pressure will the gas exert if the temperature is raised to 44.6 degrees Celsius?

Respuesta :

Pikaismylife
 PV/T = P'V'/T' 
660 x 1.00/295.2 = P' x 1.00/317.8 
P'=710.5 torr

Answer : The final pressure of the gas will be, 710.56 torr

Explanation :

According to the Charles' Law, the pressure of the gas is directly proportional to the temperature of the gas at constant volume and the number of moles of gas.

[tex]P\propto T[/tex]

or,

[tex]\frac{P_1}{P_2}=\frac{T_1}{T_2}[/tex]

where,

[tex]P_1[/tex] = initial pressure of the gas = 660 torr

[tex]P_2[/tex] = final pressure of the gas = ?

[tex]T_1[/tex] = initial temperature of the gas = [tex]22^oC=273+22=295K[/tex]

[tex]T_2[/tex] = final temperature of the gas = [tex]44.6^oC=273+44.6=317.6K[/tex]

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

[tex]\frac{660torr}{P_2}=\frac{295K}{317.6K}[/tex]

[tex]P_2=710.56torr[/tex]

Therefore, the final pressure of the gas will be, 710.56 torr

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