What is an ideal gas, and what is the real gas that behaves most ideally?
As ideal gas is a theoretical entity that behaves "ideally". Helium gas is a real gas that should best fit this ideal.
Ideal gases are thought to have very little or no molecular interaction; the gas's volume is thought to be insignificant; the molecules in an ideal gas are thought of as tiny, indivisible spheres with perfectly elastic collisions.
At moderate temperatures and pressures, real gases should behave similarly to ideal gases; of course, helium will not behave perfectly at high pressures and low temperatures. At these conditions, helium should behave similarly to ideal gases.
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An ideal gas is a hypothetical gas that follows the ideal gas law. No real gas behaves ideally, but hydrogen at high temperatures and low pressures approaches ideal behavior.
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An ideal gas is a theoretical concept in physics and chemistry that follows the ideal gas law, which states that the pressure ( P ), volume ( V ), and temperature ( T ) of a gas are related by the equation ( PV = nRT ), where ( n ) is the number of moles of gas and ( R ) is the gas constant. Ideal gases are assumed to have particles with negligible volume and no intermolecular forces.
Among real gases, hydrogen gas is often considered to behave most closely to an ideal gas under standard conditions. This is because hydrogen gas molecules are relatively small and have weak intermolecular forces, making their behavior approach that of an ideal gas more closely than many other gases.
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When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
- If water is being split to form two new substances, is it a change of state?
- How are the volatilities of the Group 16, and Group 17 hydrides rationalized?
- How do you read phase diagrams?
- Is it true that the stronger the intermolecular interactions the higher the vapor pressure?
- Would the boiling point of water be higher or lower on the top of a mountain peak? How would the boiling point be affected in a pressurized boiler system?

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