Respuesta :
Answer:
A) partial pressure of diethylether = 0.206 atm
B) Total pressure = 1.164 atm
Explanation:
Given: Density of diethylether = 0.7134 g/mL, Volume of diethylether= 5.10 mL, Total volume = 6 L
Molar mass of diethylether = 74.12 g/mol
A) As we know, Density = given mass ÷ volume
⇒ given mass of diethylether = density × volume = 0.7134 g/mL ×5.10 mL = 3.64 g
As the number of moles of diethylether = given mass ÷ molar mass = 3.64 g ÷ 74.12 g/mol = 0.049 mol
To find out the pressure of diethylether, we use the ideal gas equation:
PV = nRT
Here, P is the partial pressure of the gas, n is the number of moles of gas = 0.049 mol, V is the total volume = 6 L, R is the gas constant = 0.08206 L·atm/(mol·K) and T is the temperature = 35°C = 35 + 273 = 308 K (0 °C = 273 K)
⇒ P = nRT ÷ V = (0.049 mol × 0.08206 L·atm/(mol·K) × 308 K) ÷ 6 L
⇒ P = 0.206 atm = partial pressure of diethylether : pC₂H₅OC₂H₅
B) Given: partial pressure of: pN₂= 0.752 atm, pO₂ = 0.206 atm and pC₂H₅OC₂H₅ = 0.206 atm
As the Total pressure of all the gases = sum of partial pressure of the gases
⇒ Total pressure = pN2 + pO₂ + pC₂H₅OC₂H₅ = 0.752 atm + 0.206 atm 0.206 atm = 1.164 atm
Explanation:
(A) The given data is as follows.
Volume of diethyl ether = 5.10 ml
Density of diethyl ether = 0.7134 g/ml
Partial pressure of nitrogen = 0.752 atm
Partial pressure of oxygen = 0.206 atm
Temperature = [tex]35^{o}C[/tex] = (35 + 273) K = 308 K
As, Density = [tex]\frac{mass}{volume}[/tex]
0.7134 g/ml = [tex]\frac{mass}{5.10 ml}[/tex]
mass = 3.63 g
Also, No. of moles = [tex]\frac{mass}{\text{molar mass}}[/tex]
Hence, moles of diethyl ether will be as follows.
No. of moles = [tex]\frac{mass}{\text{molar mass}}[/tex]
= [tex]\frac{3.63 g}{74.12 g/mol}[/tex]
= 0.0489 mol
Hence, using the ideal gas equation we will find the partial pressure of diethyl ether as follows.
PV = nRT
[tex]P \times 6 L = 0.0489 \times 0.0821 L atm/mol K \times 308 K[/tex]
P = 0.206 atm
Hence, the partial pressure of diethyl ether is 0.206 atm.
(B) As it is known that total pressure of a mixture of gases is equal to the sum of partial pressures of all the gases present in the mixture.
Therefore, we will calculate the total pressure as follows.
[tex]P_{total} = P_{N_{2}} + P_{O_{2}} + P_{C_{2}H_{5}OC_{2}H_{5}}[/tex]
= 0.752 atm + 0.206 atm + 0.206 atm
= 1.164 atm
Hence, the total pressure in the container is 1.164 atm.
