If a gaseous mixture is made of 2.41 g of He and 2.79 g of Ne in a evacuated 1.04-L container at 25 degrees Celcius, what will be the partial pressure of each gas and the total pressure in the container?

Convert 2.41 g He to moles.

Convert 2.79 g Ne to moles.
Use PV = nRT to calculate partial pressure of each.

To find the partial pressure of each gas and the total pressure in the container, we can use the ideal gas law equation:

PV = nRT

Where:
P = Pressure
V = Volume
n = Number of moles
R = Ideal gas constant
T = Temperature

First, we need to calculate the number of moles for each gas using their respective masses and molar masses. The molar mass of helium (He) is approximately 4 g/mol, and the molar mass of neon (Ne) is approximately 20 g/mol.

For helium (He):
n(He) = mass(He) / molar mass(He)
n(He) = 2.41 g / 4 g/mol
n(He) = 0.6025 mol

For neon (Ne):
n(Ne) = mass(Ne) / molar mass(Ne)
n(Ne) = 2.79 g / 20 g/mol
n(Ne) = 0.1395 mol

Now, let's calculate the partial pressure of each gas using the formula:

Partial Pressure = (n * R * T) / V

For helium (He):
Partial Pressure(He) = (n(He) * R * T) / V

Substituting the given values:
Partial Pressure(He) = (0.6025 mol * 0.0821 L·atm/mol·K * 298 K) / 1.04 L
Partial Pressure(He) = 14.255 atm

For neon (Ne):
Partial Pressure(Ne) = (n(Ne) * R * T) / V

Substituting the given values:
Partial Pressure(Ne) = (0.1395 mol * 0.0821 L·atm/mol·K * 298 K) / 1.04 L
Partial Pressure(Ne) = 3.334 atm

The total pressure in the container is the sum of the partial pressures of the gases:

Total Pressure = Partial Pressure(He) + Partial Pressure(Ne)
Total Pressure = 14.255 atm + 3.334 atm
Total Pressure = 17.589 atm

So, the partial pressure of helium (He) is approximately 14.255 atm, the partial pressure of neon (Ne) is approximately 3.334 atm, and the total pressure in the container is approximately 17.589 atm.

To find the partial pressure of each gas and the total pressure in the container, we can use the ideal gas law equation: PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature.

Step 1: Calculate the number of moles of each gas.
To find the number of moles, we use the formula: moles = mass / molar mass.

The molar mass of helium (He) is approximately 4.00 g/mol, and the molar mass of neon (Ne) is approximately 20.18 g/mol.

Moles of helium (He) = mass / molar mass = 2.41 g / 4.00 g/mol = 0.6025 mol
Moles of neon (Ne) = mass / molar mass = 2.79 g / 20.18 g/mol = 0.1382 mol

Step 2: Calculate the partial pressure of each gas.
The partial pressure of each gas is calculated using the formula: P = (n * R * T) / V.

Given:
R = 0.0821 L⋅atm/(mol⋅K) (ideal gas constant)
T = 25 degrees Celsius = 298 K (convert to Kelvin)
V = 1.04 L (volume)

Partial Pressure of helium (He) = (0.6025 mol * 0.0821 L⋅atm/(mol⋅K) * 298 K) / 1.04 L = 14.45 atm (rounded to two decimal places)

Partial Pressure of neon (Ne) = (0.1382 mol * 0.0821 L⋅atm/(mol⋅K) * 298 K) / 1.04 L = 3.32 atm (rounded to two decimal places)

Step 3: Calculate the total pressure.
The total pressure is the sum of the partial pressures of each gas.

Total Pressure = Partial Pressure of helium (He) + Partial Pressure of neon (Ne) = 14.45 atm + 3.32 atm = 17.77 atm (rounded to two decimal places)

Therefore, the partial pressure of helium is 14.45 atm, the partial pressure of neon is 3.32 atm, and the total pressure in the container is 17.77 atm.