Question

78.6 grams of O2 and 67.3 grams of F2 are placed in a container with a volume of 40.6 L. Find the total pressure if the gasses are at a temperature of 43.13 °C.

Answer 1

1) List the known and unknown quantities.

Sample: O2.

Mass: 78.6 g.

Volume: 40.6 L.

Temperature: 43.13 ºC = 316.28 K.

Sample: F2.

Mass: 67.3 g.

Volume: 40.6 L.

Temperature: 43.13 ºC = 316.28 K.

2) Find the pressure of O2.

2.1- List the known and unknown quantities.

Sample: O2.

Mass: 78.6 g.

Volume: 40.6 L.

Temperature: 43.13 ºC = 316.28 K

Ideal gas constant: 0.082057 L * atm * K^(-1) * mol^(-1).

2.2- Convert grams of O2 to moles of O2.

The molar mass of O2 is 31.9988 g/mol.

`mol\text{ }O_2=78.6\text{ }g*\frac{1\text{ }mol\text{ }O_2}{31.9988\text{ }g\text{ }O_2}=2.46\text{ }mol\text{ }O_2`

2.3- Set the equation.

Ideal gas constant: 0.082057 L * atm * K^(-1) * mol^(-1)

`PV=nRT`

2.4- Plug in the known quantities and solve for P.

`(P)(40.6\text{ }L)=(2.46\text{ }mol\text{ }O_2)(0.082057\text{ }L*atm*K^(-1)*mol^(-1))(316.28\text{ }K)`

.

`P_(O_2)=\frac{(2.46\text{ }mol\text{ }O_2)(0.082057\text{ }L*atm*K^(-1)*mol^(-1))(316.28\text{ }K)}{40.6\text{ }L}`
`P_(O_2)=1.57\text{ }atm`

The pressure of O2 is 1.57 atm.

3) Find the pressure of F2.

3.1- List the known and unknown quantities.

Sample: F2.

Mass: 67.3 g.

Volume: 40.6 L.

Temperature: 43.13 ºC = 316.28 K.

Ideal gas constant: 0.082057 L * atm * K^(-1) * mol^(-1).

3.2- Convert grams of F2 to moles of F2.

The mmolar mass of F2 is 37.9968 g/mol.

`mol\text{ }F_2=67.3\text{ }g\text{ }F_2*\frac{1\text{ }mol\text{ }F_2}{37.9968\text{ }g\text{ }F_2}=1.77\text{ }mol\text{ }F_2`

3.3- Set the equation.

Ideal gas constant: 0.082057 L * atm * K^(-1) * mol^(-1)

`PV=nRT`

3.4- Plug in the known quantities and solve for P.

`(P)(40.6\text{ }L)=(1.77\text{ }mol\text{ }F_2)(0.082057\text{ }L*atm*K^(-1)*mol^(-1))(316.28\text{ }K)`

.

`P_(F_2)=\frac{(1.77molF_2)(0.082057L*atm*K^(-1)*mol^(-1))(316.28K)}{40.6\text{ }L}`
`P_(F_2)=1.13\text{ }atm`

The pressure of F2 is 1.13 atm.

4) The total pressure.

Dalton's law - Partial pressure. This law states that the total pressure of a gas is equal to the sum of the individual partial pressures.

4.1- Set the equation.

`P_T=P_A+P_B`

4.2- Plug in the known quantities.

`P_T=1.57\text{ }atm+1.13\text{ }atm`
`P_T=2.7\text{ }atm`

The total pressure in the container is 2.7 atm.