Answer:
Explanation:
1) Data:
a) V = 10.0 l
b) He, m₁ = 48.5 g
c) CO₂, m₂ = 94.6 g
d) T = 398 K
e) p = ?
2) Formulae:
a) ideal gas equation: pV = nRT
b) Number of moles, n: n = mass in grams / molar mass
3) Solution:
a) Number of moles of He:
b) Number of moles of CO₂:
c) Total number of moles of the gas mixture:
d) Pressure, p:
Pressure of gas mixture : P tot = 46,588 atm
Dalton's law of partial pressures states that the total pressure of a mixture of gases is equal to the sum of the partial pressures of the component gases
Can be formulated:
The partial pressure is the pressure of each gas in a mixture
Since the gas mixture consists of He and CO₂, we determine the pressure of each gas then we add them together to get the total pressure
We assume the ideal gas, so we use the formula:
[tex] \large {\boxed {\bold {PV = nRT}}} [/tex]
where
P = pressure, atm, N / m²
V = volume, liter
n = number of moles
R = gas constant = 0.082 l.atm / mol K (P = atm, v = liter), or 8.314 J / mol K (P = Pa or N / m2, v = m³)
T = temperature, Kelvin
n = N / No
n = mole
No = Avogadro number (6.02.10²³)
n = m / m
m = mass
M = relative molecular mass
M = 4 g / mol
m = 48.5 g
n = m: M
n = 48.5: 4
n = 12,125 mole
PV = nRT
[tex]\rm P=\dfrac{nRT}{V}\\\\P=\dfrac{12.125\times 0.082\times 398}{10}\\\\P=\boxed{39,571\:atm}}[/tex]
2. CO₂
M = 44 g / mol
m = 94.6 g
n = m: M
n = 94.6: 44
n = 2.15 mole
PV = nRT
[tex]\rm P=\dfrac{nRT}{V}\\\\P=\dfrac{2.15\times 0.082\times 398}{10}\\\\P=\boxed{7.0167\:atm}}[/tex]
P tot = P He + P CO₂
P tot = 39,571 + 7.0167
P tot = 46,588 atm
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