Answer:- 4.6 atm.
Solution:- In this problem, the volume is constant and the pressure is changing as the temperature is changed. It's based on Gay-Lussac's law which states that, "At constant volume, pressure of the gas is directly proportional to the kelvin temperature."
The equation used for solving the problems based on this law is:
[tex]\frac{P_1}{T_1}=\frac{P_2}{T_2}[/tex]
Where, [tex]P_1[/tex] is initial pressure and [tex]P_2[/tex] is final pressure.
Similarly, [tex]T_1[/tex] is initial temperature and [tex]T_2[/tex] is final temperature.
[tex]P_1[/tex] = 3.0 atm
[tex]T_1[/tex] = 100.0 + 273 = 373 K
[tex]T_2[/tex] = 300.0 + 273 = 573 K
[tex]P_2[/tex] = ?
Let's plug in the values in the equation and solve it for final pressure:
[tex]\frac{3.0atm}{373K}=\frac{P_2}{573K}[/tex]
[tex]P_2=\frac{(3.0atm*573K)}{373K}[/tex]
[tex]P_2=4.6atm[/tex]
So, the pressure of the gas at higher temperature is 4.6 atm.
