A 7. 8-g piece of solid carbon dioxide is placed in a 4. 0-l container that has an air pressure of 740. Torr and a temperature of 355 k. What is the pressure (torr) in the container after all the carbon dioxide vaporizes?.

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19-12-2022
Physics

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A 7. 8-g piece of solid carbon dioxide is placed in a 4. 0-l container that has an air pressure of 740. Torr and a temperature of 355 k. What is the pressure (torr) in the container after all the carbon dioxide vaporizes?.

Answer :

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Qwbox Qwbox · Answer 1 · 2022-12-28T12:13:27-05:00

The pressure of the container after carbon dioxide vaporizes in the container is found to be 261 Torr.

The mass of solid carbon dioxide is 7.8 grams and the volume of the container is 4L and which has a pressure of 740 torr and the temperature is 355K.

Using the ideal gas equation to find the number of moles of CO₂ in the sample,

PV = nRT

Where,

P is pressure,

V is volume,

n is moles,

R is gas constant,

T is temperature.

Putting values,

740 x 4 = n(62.36)(355)

n = 0.13 moles.

Now, we know,

Moles = Mass/Molar mass

Molar mass of CO₂ = 44 g/mol

Mass of CO₂ = 0.13 x 44

Mass of CO₂ = 5.72

Now, the mass of vaporized CO₂ is 2.08 grams.

Now again using the equation,

PV = nRT

P = nRT/V

P = 2.08 x 62.36 x 355/(44 x 4)

P = 261 Torr.

So, the pressure of the container is 261 Torr.

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