contestada

2)
If 5.0 moles of O2 and 3.0 moles of N2 are placed in a 30.0 L tank at a temperature of 25°
C, what will the pressure of the resulting mixture of gases be?

Respuesta :

Neetoo

Answer:

Total pressure = 6.55 atm

Explanation:

Given data:

Number of moles of oxygen = 5.0 mol

Number of moles of nitrogen = 3.0 mol

Volume of tank = 30.0 L

Temperature = 25°C (25+273 = 298 K)

Total pressure of mixture = ?

Solution:

Pressure of oxygen:

PV = nRT

P = nRT/V

P = 5.0 mol ×0.0821 atm.L/mol.K × 298 k /30.0 L

P = 122.33 atm /30.0

P = 4.1 atm

Pressure of nitrogen:

PV = nRT

P = nRT/V

P = 3.0 mol ×0.0821 atm.L/mol.K × 298 k /30.0 L

P = 73.4 atm /30.0

P = 2.45 atm

Total pressure = Partial pressure of oxygen + partial pressure of nitrogen

Total pressure =  4.1 atm +  2.45 atm

Total pressure = 6.55 atm

CintiaSalazar

Considering the Ideal Gas Law and Dalton's partial pressure, the pressure of the resulting mixture of gases will be 6.5136 atm.

Ideal gas law

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.

The pressure, P, the temperature, T, and the volume, V, of an ideal gas, are related by a simple formula called the ideal gas law:

P×V = n×R×T

where:

  • P is the gas pressure.
  • V is the volume that occupies.
  • T is its temperature.
  • R is the ideal gas constant. The universal constant of ideal gases R has the same value for all gaseous substances.
  • n is the number of moles of the gas.

Dalton's law

The pressure exerted by a particular gas in a mixture is known as its partial pressure.

So, Dalton's law states that the total pressure of a gas mixture is equal to the sum of the pressures that each gas would exert if it were alone:

[tex]P_{T} =P_{1} +P_{2} +P_{3} +...+P_{n}[/tex]

where n is the amount of gases present in the mixture.

This relationship is due to the assumption that there are no attractive forces between the gases.

Pressure of the resulting mixture of gases

Considering the Ideal Gas Law, it is first necessary to calculate the pressure exerted by the nitrogen and the oxygen. For this you know:

  • Number of moles of oxygen = 5.0 mol
  • Number of moles of nitrogen = 3.0 mol
  • Volume of tank = 30.0 L
  • Temperature = 25°C= 298 K (being 0 °C= 273 K)
  • Constant R= 0.082 [tex]\frac{atmL}{mol K}[/tex]

Substituting in the Ideal Gas Law for each gas, and solving, you get:

  • Pressure of oxygen:

P×V = n×R×T

P×30 L = 5 mol×0.082 [tex]\frac{atmL}{mol K}[/tex]× 298 K

P×30 L = 122.18 atm L

P= (122.18 atm L) ÷ 30 L

P = 4.07 atm

  • Pressure of nitrogen:

P×V = n×R×T

P×30 L = 3 mol×0.082 [tex]\frac{atmL}{mol K}[/tex]× 298 K

P×30 L = 73.308 atm L

P= (73.308 atm L) ÷ 30 L

P = 2.4436 atm

Now, taking Dalton's law into account, you know that:

[tex]P_{T} =P_{O_{2} } +P_{N_{2} }[/tex]

Substituting the corresponding values and solving ​​you get:

[tex]P_{T} =4.07 atm + 2.4436 atm[/tex]

[tex]P_{T} =[/tex]6.5136 atm

Finally, the pressure of the resulting mixture of gases will be 6.5136 atm.

Learn more about

Ideal Gas Law:

https://brainly.com/question/4147359

Dalton's law:

brainly.com/question/14119417

Otras preguntas