Respuesta :

Answer: 0.0007 moles of [tex]CO_2[/tex] is released when temperature is raised.

Explanation:

To calculate the number of moles, we use the ideal gas equation, which is:

[tex]PV=nRT[/tex]

where,

P = pressure of the gas = 1.01 bar

V = Volume of the gas = 1L

R = Gas constant = [tex]0.08314\text{ L bar }mol^{-1}K^{-1}[/tex]

  • Number of moles when T = 20° C

Temperature of the gas = 20° C = (273 + 20)K = 293K

Putting values in above equation, we get:

[tex]1.01bar\times 1L=n_1\times 0.0814\text{ L bar }mol^{-1}K^{-1}\times 293K\\n_1=0.04146moles[/tex]

  • Number of moles when T = 25° C

Temperature of the gas = 25° C = (273 + 25)K = 298K

Putting values in above equation, we get:

[tex]1.01bar\times 1L=n_2\times 0.0814\text{ L bar }mol^{-1}K^{-1}\times 298K\\n_2=0.04076moles[/tex]

  • Number of moles released = [tex]n_1-n_2=0.04146-0.04076=0.0007moles[/tex]

Hence,  0.0007 moles of [tex]CO_2[/tex] is released when temperature is raised from 20° C to 25° C

Lanuel

The number of moles of [tex]CO_2[/tex] gas released by raising the temperature is 0.0044 moles.

Given the following data:

  • Pressure = 1.01 bar
  • Initial temperature = 20°C
  • Final temperature = 25°C
  • Volume = 1 liter

Change in temperature = [tex]25 - 20 =[/tex] 5°C

Conversion:

Temperature = 5°C to K = [tex]273 + 5=[/tex] 278 Kelvin

Pressure = 1.01 bar to atm = 0.1 atm

Ideal gas constant, R = 0.0821L⋅atm/mol⋅K

To find how many moles (number of moles) of [tex]CO_2[/tex] gas are released, we would use the ideal gas law equation;

[tex]PV = nRT[/tex]

Where;

  • P is the pressure.
  • V is the volume.
  • n is the number of moles of substance.
  • R is the ideal gas constant.
  • T is the temperature.

Making n the subject of formula, we have;

[tex]n = \frac{PV}{RT}[/tex]

Substituting the given parameters into the formula, we have;

Number of moles, n = 0.0044 moles.

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