If a gaseous mixture is made of 2.37 g of He and 2.73 g of Ne in an evacuated 1.19 L container at 25°C, what will be the partial pressure of each gas and the total pressure in the container?
Given the following sets of values for three of the gas variables, calculate the unknown.
P = ? mm Hg; V = 26.0 mL; n = 0.007826 mol; T = 15.6°C
Use PV = nRT for He (n = gram/molar mass) and solve for pHe.
Do the same for Ne, then add the partial pressures to obtain total pressure.
#2 use PV = nRT
To find the partial pressure of each gas and the total pressure in the container, we need to use the ideal gas law equation, which states:
PV = nRT
Where:
P = pressure
V = volume
n = number of moles of gas
R = ideal gas constant
T = temperature
First, we need to find the number of moles of each gas using their molar masses.
The molar mass of helium (He) is approximately 4 g/mol.
The molar mass of neon (Ne) is approximately 20 g/mol.
To find the number of moles, we divide the mass of each gas by its respective molar mass.
For helium:
Number of moles = mass / molar mass = 2.37 g / 4 g/mol
For neon:
Number of moles = mass / molar mass = 2.73 g / 20 g/mol
Next, we need to calculate the total number of moles of gas present in the container by adding the moles of each gas.
Total number of moles = moles of helium + moles of neon
Now, we can calculate the partial pressure of each gas using the equation:
Partial pressure = (number of moles / total number of moles) * total pressure
Since the gases are in an evacuated container, the total pressure will be equal to the sum of the partial pressures of each gas.
To convert the temperature from Celsius to Kelvin, we add 273.15 to the given temperature of 25°C.
Now we have all the necessary information to calculate the partial pressure of each gas and the total pressure in the container.