Number of moles of argon plasma to exert X pressure

In summary, the amount of argon gas needed to exert 10,000 psi in a cylinder will be different if it is transformed into plasma. This is because plasma has a higher kinetic energy and excitement level. When heating argon to transform it into plasma, the electric current will provide even more pressure. However, the temperature of plasma for different gases is not always known and can be confusing. Generally, devices that generate plasma have lower pressure than atmospheric pressure to make it easier to create the plasma.
  • #1
ahmed11
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is the amount of argon gas to exert 10,000 psi in cylinder will be the same if argon transformed to plasma or the number of moles will be less as plasma is more excited and have higher kinetic energy?
 
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  • #2
How do you want to convert it to plasma?
Even if we ignore the transition to plasma, what do you expect as result from heating?
 
  • #3
mfb said:
How do you want to convert it to plasma?
Even if we ignore the transition to plasma, what do you expect as result from heating?
sorry for the late reply.
i mean if we connected an electric current to it to transform it to plasma, will that lead to a higher kinetic energy from the electric current which will give out more pressure right?
but i don't get temperatures of plasma for all kind of gases and that's mainly where i would appreciate your help, i always see videos on youtube of argon plasma in glass jars so how does the high temperature of argon plasma doesn't make the glass jar explode, here is a link to the video that got me confused
 
  • #4
Usually those devices have a much lower pressure than atmospheric pressure, as this makes it easier to generate a plasma.
 
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1. How do you calculate the number of moles of argon plasma needed to exert a specific pressure?

The number of moles of argon plasma needed to exert a specific pressure can be calculated using the ideal gas law equation, PV = nRT. P represents pressure in Pascals, V represents volume in liters, n represents the number of moles, R is the universal gas constant (8.314 J/mol*K), and T is temperature in Kelvin. Rearranging the equation, the number of moles (n) can be calculated as n = (PV)/(RT).

2. What is the relationship between the number of moles of argon plasma and the pressure it exerts?

The number of moles of argon plasma and the pressure it exerts are directly proportional. This means that as the number of moles increases, the pressure exerted by the plasma also increases. Similarly, if the number of moles decreases, the pressure exerted by the plasma will also decrease.

3. Can the pressure exerted by argon plasma be controlled by adjusting the number of moles?

Yes, the pressure exerted by argon plasma can be controlled by adjusting the number of moles. According to the ideal gas law, pressure is directly proportional to the number of moles, so increasing or decreasing the number of moles will result in a corresponding change in pressure.

4. What other factors besides the number of moles can affect the pressure exerted by argon plasma?

Other factors that can affect the pressure exerted by argon plasma include the volume of the container, temperature, and the type of gas present. Changing these variables can also result in a change in pressure, even if the number of moles remains constant.

5. How can the number of moles of argon plasma be experimentally determined?

The number of moles of argon plasma can be experimentally determined by measuring the pressure, volume, and temperature of the plasma and then plugging those values into the ideal gas law equation. Alternatively, the number of moles can also be determined by measuring the mass of the gas and using its molar mass to calculate the number of moles using the formula n = m/M, where m is mass in grams and M is the molar mass in grams/mol.

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