Question

5.6 g of solid CO2 is put in an empty sealed 4.00 L container at a temperature of

Answer 1

Answer:

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