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Suppose the gas resulting from the sublimation of 1.00 g carbon dioxide is collected over water at 25.0◦c into a 1.00 l container. What is the total pressure in the container? Express your answer in atmospheres.

Respuesta :

skyluke89

Answer:

0.55 atm

Explanation:

First of all, we need to calculate the number of moles corresponding to 1.00 g of carbon dioxide. This is given by

[tex]n=\frac{m}{M_m}[/tex]

where

m = 1.00 g is the mass of the gas

Mm = 44.0 g/mol is the molar mass of the gas

Substituting,

[tex]n=\frac{1.00 g}{44.0 g/mol}=0.0227 mol[/tex]

Now we can find the pressure of the gas by using the ideal gas law:

[tex]pV=nRT[/tex]

where

p is the gas pressure

V = 1.00 L is the volume

n = 0.0227 mol is the number of moles

R = 0.082 L/(atm K mol) is the gas constant

T = 25.0 C + 273 = 298 K is the temperature of the gas

Solving the formula for p, we find

[tex]p=\frac{nRT}{V}=\frac{(0.0227 mol)(0.082 L/(atm K mol))(298 K)}{1.00 L}=0.55 atm[/tex]

Eduard22sly

The total pressure in the container when the 1 g of carbon dioxide is collected over water at 25 °C is 0.555 atm

How to determine the mole of CO₂

  • Mass of CO₂ = 1 g
  • Molar mass of CO₂ = 44 g/mol
  • Mole of CO₂ =?

Mole = mass / molar mass

Mole of CO₂ = 1 / 44

Mole of CO₂ = 0.0227 mole

How to determine the pressure

  • Volume (V) = 1 L
  • Temperature (T) = 25 °C = 25 +  273 = 298 K
  • Gas constant (R) = 0.0821 atm.L/Kmol
  • Number of mole (n) = 0.0227 mole
  • Pressure (P) =?

Using the ideal gas equation, the total pressure can be obtained as follow:

PV = nRT

P × 1 = 0.0227 × 0.0821 × 298

P = 0.555 atm

Learn more about ideal gas equation:

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