Calculate the pressure of 0.76 moles of methane that occupies 2800 cm3 at a temperature of 290 k. a. 0.654 kpa b. 654.12 kpa c. 2664.82 pa d. 60.97 pa

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.

Pressure in this case

In this case, you know:

P= ?
V= 2800 cm³= 2.8 L (being 1 cm³= 0.001 L)
T= 290 K
R= 0.082 [tex]\frac{atmL}{molK}[/tex]
n= 0.76 moles

Replacing in the ideal gas law:

P× 2.8 L = 0.76 moles× 0.082 [tex]\frac{atmL}{molK}[/tex]× 290 K

Solving:

P = (0.76 moles× 0.082 [tex]\frac{atmL}{molK}[/tex]× 290 K)÷ 2.8 L

P= 6.4546 atm= 654.012 kPa (being 1 atm= 101.325 kPa)

Finally, the pressure of 0.76 moles of methane that occupies 2800 cm³ at a temperature of 290 K is 654.012 kPa.

Learn more about the ideal gas law:

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