Answer:
P1 = 5.76 atm
Explanation:
To find the initial pressure of the gas you use the equation for ideal gases, for both temperatures and pressures:
[tex]P_1V=nRT_1\\\\P_2V=nRT_2\\\\[/tex]
T1: initial temperature = 30°C = 303.15K
T2: final temperature = 45°C = 318.15K
P1: initial pressure = ?
P2: final pressure = 6atm
n: number of moles
R: ideal gas constant
The number of moles and R are constant, you can dive the first equation into the second and solve for P1:
[tex]\frac{P_1V}{P_2V}=\frac{nRT_1}{nRT_2}\\\\\frac{P_1}{P_2}=\frac{T_1}{T_2}[/tex]
[tex]P_1=\frac{T_1P_2}{T_2}[/tex]
Finally, you replace the values of T1, P2 and T2:
[tex]P_1=\frac{(303.15K)(6atm)}{318.15K}=5.71atm[/tex]
hence, the initial pressure of the gas was 5.71 atm
