Question

A gas mixture contains each of the following gases at the indicated partial pressures:

N₂= 215 torr
O₂= 102 torr
He= 117 torr
a) What is the total pressure of the mixture?
b) What mass of each gas is present in a 1.35 L sample of this mixture at 25.0 C ?

Answer 1

The total pressure of the gas mixture is 434 torr. To find the mass of each gas in a 1.35 L sample of the mixture, use the ideal gas law equation and the molar mass of each gas.

Step-by-step explanation:

To find the total pressure of the gas mixture, we need to sum up the partial pressures of each gas. The total pressure is given by the sum of the partial pressures:

Total pressure = PN₂ + PO₂ + PHe

Substituting the given values, we get: Total pressure = 215 torr + 102 torr + 117 torr = 434 torr.

To calculate the mass of each gas in a 1.35 L sample of the mixture, we need to 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.

We can rearrange the equation to solve for the number of moles:

n = (pV) / (RT)

By substituting the given values for each gas and solving for n, we can then calculate the mass using the molar mass of each gas.