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. In an industrial process, nitrogen is heated to 500 K in a vessel of constant volume. If it enters the vessel at 100 atm and 300 K, (a) what pressure would it exert at the working temperature if it behaved as an ideal gas

Respuesta :

Answer: 60 atm

Explanation:

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

[tex]P\propto T[/tex]     (At constant volume and number of moles)

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

where,

[tex]P_1[/tex] = initial pressure of gas  = ?

[tex]P_2[/tex] = final pressure of gas= 100 atm

[tex]T_1[/tex] = initial temperature of gas  = 500 K

[tex]T_2[/tex] = final temperature of gas  = 300 K

[tex]{P_1\times 500}={100\times 300}[/tex]

[tex]P_1=60atm[/tex]

Therefore, the pressure it would exert at the working temperature if it behaved as an ideal gas is 60 atm.

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