Question

If a gaseous mixture is made of 2.29 g of he and 2.67 g of ne in an evacuated 1.06 l container at 25°c, what will be the partial pressure of each gas and the total pressure in the container?

Answer 1

To find the partial and total pressures of He and Ne in a container, convert their masses to moles, apply the ideal gas law to find the partial pressures, and sum the partial pressures for the total pressure.

Step-by-step explanation:

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

First, convert the mass of helium (He) and neon (Ne) to moles using their molar masses (He = 4.00 g/mol, Ne = 20.18 g/mol). For helium: moles of He = 2.29 g / 4.00 g/mol = 0.5725 mol. For neon: moles of Ne = 2.67 g / 20.18 g/mol = 0.1323 mol.

Then, apply the ideal gas law individually for each gas to find their partial pressures. With R = 0.0821 atm·L/(mol·K) and T = 25°C = 298K:

Partial pressure of He (PHe): PHe = (nHeRT)/V = (0.5725 mol * 0.0821 atm·L/(mol·K) * 298K) / 1.06 L

Partial pressure of Ne (PNe): PNe = (nNeRT)/V = (0.1323 mol * 0.0821 atm·L/(mol·K) * 298K) / 1.06 L

Finally, the total pressure in the container is the sum of the partial pressures of helium and neon.