Respuesta :
Answer: Total pressure of the gas will be 0.716atm.
Explanation: We are given a gas having initial conditions as
V = 27L
T = 32°C = 305K
P = 2.5atm
As the gas remains same, number of moles of a gas will also be same for initial and final conditions. To calculate the number of moles, we use ideal gas equation, which is,
[tex]PV=nRT[/tex] .......(1)
where, R = gas constant = [tex] \text{0.08206 L atm }mol^{-1} K^{-1}[/tex]
For calculating number of moles:
[tex]n=\frac{PV}{RT}[/tex]
Putting the values of initial condition in this equation, we get
[tex]n=\frac{(2.5atm)(27L)}{\text{(0.08206 L atm }mol^{-1} K^{-1})(305K)}[/tex]
n = 2.696 mol
Now, the final conditions are,
V = 88.0L
T = 12°C = 285K
n = 2.696 mol (calculated above)
P = ? atm
Again using equation 1, we get
[tex]P=\frac{nRT}{V}[/tex]
[tex]P=\frac{(2.696mol)(\text{0.08206 L atm }mol^{-1} K^{-1})(285K)}{88.0L}[/tex]
P = 0.716atm.
ideal gas law P1*V1/T1 = P2*V2/T2
so P2= P1*V1/T1 * T2/V2
P1: 2.5, V1: 27L, T1: 32C=305K
P2: ? , V2: 88L, T2: 12C=285K
P2= 2.5*27/305 * 285/88
= 0.72 atm
