Question

A(n) 7.26−mol sample of carbon monoxide was stored in a 30.0−L container at 46.0°C. What is the pressure of the carbon monoxide in the container?

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Answer 1

Taking into account about the ideal gas law, the pressure of the carbon monoxide in the container is 6.33 atm.

What is 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. The universal constant of ideal gases R has the same value for all gaseous substances.
• R is the ideal gas constant.
• n is the number of moles of the gas.

Pressure of the carbon monoxide in the container

In this case, you know:

• P= ?
• V= 30 L
• T =46 °C= 319 K (being 0°C= 273 K)
• R= 0.082 $\frac{atmL}{molK}$
• n= 7.26 moles

Replacing in the ideal gas law:

P ×30 L = 7.26 moles ×0.082 $\frac{atmL}{molK}$× 319 K

Solving:

P= (7.26 moles ×0.082 $\frac{atmL}{molK}$× 319 K)÷ 30 L

P= 6.33 atm

Finally, the pressure of the carbon monoxide in the container is 6.33 atm.

Learn more about the ideal gas law:

brainly.com/question/4147359

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