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thermo15378
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Homework Statement
two hundred seventy grams of argon at a pressure of 160kpa and a volume of 1.3 m^3.
Homework Equations
pv=nrt
The Attempt at a Solution
(160^3)(1.3) = (.27)(8.31)(t)
208=2.2437t
t=92.7
Not quite. n is the number of moles. How many moles of argon in .27 kg of argon?thermo15378 said:Homework Statement
two hundred seventy grams of argon at a pressure of 160kpa and a volume of 1.3 m^3.
Homework Equations
pv=nrt
The Attempt at a Solution
(160^3)(1.3) = (.27)(8.31)(t)
208=2.2437t
t=92.7
What is the mass of one mole of Argon?thermo15378 said:0.0067 is what i get for moles but when i plug in the formula I am getting 3649.12 and that cannnot be right.
A perfect gas is an idealized model of gas behavior that follows the assumptions of the kinetic theory of gases. It is a hypothetical gas that has the following characteristics: its molecules have negligible volume, there are no attractive or repulsive forces between molecules, and collisions between molecules are completely elastic.
To determine an unknown property of a perfect gas, you can use the ideal gas law, which states that the pressure, volume, and temperature of a gas are related by the equation PV = nRT. By rearranging this equation and plugging in known values, you can solve for the unknown property.
The properties of a perfect gas include pressure, volume, temperature, and number of moles. These properties are interrelated and can be described by the ideal gas law.
No, a real gas cannot behave exactly like a perfect gas because real gases have volume and can experience attractive or repulsive forces between molecules. However, at low pressures and high temperatures, many gases behave similarly to a perfect gas and can be accurately described by the ideal gas law.
According to the ideal gas law, increasing the temperature of a perfect gas will cause an increase in its pressure, assuming the volume and number of moles remain constant. Similarly, increasing the pressure of a perfect gas will cause a decrease in its volume, assuming the temperature and number of moles remain constant.