5.6 g of solid CO2 is put in an empty sealed 4.00 L container at a temperature of
300 K. When all the solid CO2 becomes gas, what will be the pressure in the
container? *
34.5 atm
O
O
0.78 atm
0.006 atrh
None of the other answers

Considering the idea gas law, the correct answer is the second option: when all the solid CO₂ becomes gas, the pressure in the  container will be 0.78 atm.

Ideal gases are a simplification of real gases that is done to study them more easily. It is considered to be formed by point particles, do not interact with each other and move randomly. It is also considered that the molecules of an ideal gas, in themselves, do not occupy any volume.

An ideal gas is characterized by three state variables: absolute pressure (P), volume (V), and absolute temperature (T).

The relationship between them constitutes the ideal gas law, an equation that relates the three variables if the amount of substance, number of moles n, remains constant and where R is the molar constant of the gases:

P× V = n× R× T

In this case, you know:

Replacing in the ideal gas law:

P× 4 L= 0.127 moles× 0.082× 300 K

Solving:

P= 0.78105 atm ≅ 0.78 atm

Finally, the correct answer is the second option: when all the solid CO₂ becomes gas, the pressure in the  container will be 0.78 atm.

Learn more:

0.78 atm

Explanation:

Step 1:

Data obtained from the question. This includes:

Mass of CO2 = 5.6g

Volume (V) = 4L

Temperature (T) =300K

Pressure (P) =?

Step 2:

Determination of the number of mole of CO2.

This is illustrated below:

Mass of CO2 = 5.6g

Molar Mass of CO2 = 12 + (2x16) = 12 + 32 = 44g/mol

Number of mole CO2 =?

Number of mole = Mass/Molar Mass

Number of mole of CO2 = 5.6/44

Number of mole of CO2 = 0.127 mole

Step 3:

Determination of the pressure in the container.

The pressure in the container can be obtained by applying the ideal gas equation as follow:

PV = nRT

The gas constant (R) = 0.082atm.L/Kmol

The number of mole (n) = 0.127 mole

P x 4 = 0.127 x 0.082 x 300

Divide both side by 4

P = (0.127 x 0.082 x 300) /4

P = 0.78 atm

Therefore, the pressure in the container is