Respuesta :
Answer:
(a) 0.25 mol
(b) 0.11 mol
(c) 8.77 mol
Explanation:
(a)
We use the equation given by ideal gas which follows:
[tex]PV=nRT[/tex]
where,
P = pressure of the gas = 1.00 atm
V = Volume of the gas = 6.0 L
T = Temperature of the gas = 298 K
R = Gas constant = [tex]0.0821\text{ L.atm }mol^{-1}K^{-1}[/tex]
n = number of moles = ?
Putting values in above equation, we get:
[tex]1.00 atm\times 6.0L=n\times 0.0821\text{ L.atm }mol^{-1}K^{-1}\times 298K\\\\n=\frac{1.00\times 6.0}{0.0821\times 298}=0.25mol[/tex]
(b)
We use the equation given by ideal gas which follows:
[tex]PV=nRT[/tex]
where,
P = pressure of the gas = 0.296 atm
V = Volume of the gas = 6.0 L
T = Temperature of the gas = 200 K
R = Gas constant = [tex]0.0821\text{ L.atm }mol^{-1}K^{-1}[/tex]
n = number of moles = ?
Putting values in above equation, we get:
[tex]0.296 atm\times 6.0L=n\times 0.0821\text{ L.atm }mol^{-1}K^{-1}\times 200K\\\\n=\frac{0.296\times 6.0}{0.0821\times 200}=0.11mol[/tex]
(c)
We use the equation given by ideal gas which follows:
[tex]PV=nRT[/tex]
where,
P = pressure of the gas = 30 atm
V = Volume of the gas = 6.0 L
T = Temperature of the gas = 250 K
R = Gas constant = [tex]0.0821\text{ L.atm }mol^{-1}K^{-1}[/tex]
n = number of moles = ?
Putting values in above equation, we get:
[tex]30 atm\times 6.0L=n\times 0.0821\text{ L.atm }mol^{-1}K^{-1}\times 250K\\\\n=\frac{30\times 6.0}{0.0821\times 250}=8.77mol[/tex]
