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At what temperature does a real gas obey the ideal gas laws over a wide range of pressure?
Wiki User
∙ 13y ago
Real gases behave most like ideal gases at high temperatures and low pressures.
CASE 1 :- (At Higher Temperatures)
when the temperature is high the kinetic energy of molecules increases and the intermolecular attractions among the atoms decreases.
The volume of the gas molecules become negligible compared to volume of the vessel. therefore the real gases act like ideal At Higher Temperatures.
CASE 2 :- (At Lower Temperatures)
At low temperatures volume of the container is larger. therefore intermolecular attractive forces are negligible and the volume of the particles also become negligible compared with the volume of the vessel.
therefore the real gases act like ideal At Lower Temperatures.
Wiki User
∙ 14y ago
Wiki User
∙ 16y agoI believe that at conditions of high temperature and low pressure then gasses tend to behave more like an ideal gas. Only at lower temperatures, high pressures to the 'messy' degrees of freedom manifest themselves in molecular interactions. But at low pressure and high temperatures there are fewer molecular degrees of freedom, and so the gas becomes 'less complex' and more like the ideal gas. However, once the gas starts to become a plasma--then electromagnetic effects start to play a big role.
Wiki User
∙ 14y agokinetic postulates gas ,the gas molecule has no attraction .at low pressure and high temperature the volume of the gas is very high .so that the kinetic energy is very high.this condition the molecule can not attrac each other.and they behave like a ideal gas.
Wiki User
∙ 11y agoReal gases approach ideal behavior at high temperature and low pressure. In this Condition gases occupy a large volume and molecules are far apart so volume of gas molecules are negligible and intermolecular force of attraction (responsible for non ideal behavior) become low. So gases approach ideal behavior.
Wiki User
∙ 13y agoAt very high temperatures, most gases obey the ideal gas law.
that temperature is called boyle temperature
Wiki User
∙ 7y agoA real gas differs from an ideal gas at all temperatures, but the difference is greatest at high pressures and low temperatures.
Wiki User
∙ 7y agoA real gas differ from an ideal gas at any temperature and pressure.
Wiki User
∙ 13y agoHigh Tempature and Low Pressure
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As the temperature of a fixed volume of a gas increases the pressure will?
decrease
How does temperature and pressure affect the ideal gas?
There are three main gas laws: Boyle's, Charles' and the pressure law. These describe the relationship between pressure, volume and temperature of an ideal gas. Boyle's law: the volume of a gas is inversely proportional to its pressure; i.e. doulbing the pressure applied to a gas will halve the volume it takes up (and vice-versa). Charles' law: the volume of a gas is directly proportional to its temperature; i.e. doulbing the temperature of a gas will double the volume it takes up (and vice-versa). Pressure law: the pressure of a gas is directly proportional to its temperature; i.e. doubling the temperature of a gas will double the pressure placed upon the gas (and vice-versa). These three laws can be combined with another to give the ideal gas law: PV = nRT (where P = pressure, V = volume, n = number of moles, R = universal gas constant and T = temperature in Kelvin). But seriously, next time, just Google it - it'll be faster. Or maybe read a textbook?
How are pressure volume and temperature of gases related?
The temperature, pressure, and volume of gases can be related by the ideal gas equation. PV = nRT where P is pressure, V is volume, n is moles, R is that ideal gas constant, and T is the temperature in Kelvin.
Do the pressure of a gas decreases with increasing temperature?
If the temperature remains constant, decreasing the volume will increase the pressure.
Why Real gases do not obey gas laws?
Real gases do not obey gas laws because these gases contains forces of attractions among the molecules..and the gases which do not contain forces of attraction among their molecules are called ideal gases and they obey gas laws.
What gas conforms to the gas laws at all conditions of temperature and pressure?
The ideal gas law
What will happen if we do not assume idal gas equation in deriving boyle's and charle's law?
Boyle's and Charles' laws where not derived from the Ideal Gas Equation. The opposite is true. Boyle's and Charles' laws and a few other laws are used to derive the Ideal Gas Equation. Boyle's and Charles' laws are based on the authors observations of the behaviour of gases. They give a fair prediction at relative low pressures and high temperatures with respect to the gas Critical Pressure and Temperature. A real gas at a given pressure and temperature range can show a great deviation from the Ideal Gas, and that would also mean deviation from Boyle's and Charles' laws. Now, if what you mean is obtaining a relation between Pressure and Volume at constant Temperature, and another between Temperature and Volume at constant Pressure for a real gas, it can be done. But they won't look as simple and nice as Boyle's and Charles' laws.
What relationship show Charles' laws?
The relationship between absolute temperature and volume of an ideal gas at constant pressure.
The temp at which real gases obey the ideal gas laws over a wide range of pressure what is this temp known as?
boyles temprature
What happens to the gas when temperature drops from 100 degrees to -100 degrees?
You will recall from the Ideal Gas Laws that temperature, pressure, and volume are all connected in terms of the behavior of a gas (especially an ideal gas, but actual gas resembles ideal gas to a certain extent). So, if the gas is in a container of fixed volume, then reducing the temperature will correspondingly reduce the pressure.
As the temperature of a fixed volume of a gas increases the pressure will?
decrease
How does temperature and pressure affect the ideal gas?
There are three main gas laws: Boyle's, Charles' and the pressure law. These describe the relationship between pressure, volume and temperature of an ideal gas. Boyle's law: the volume of a gas is inversely proportional to its pressure; i.e. doulbing the pressure applied to a gas will halve the volume it takes up (and vice-versa). Charles' law: the volume of a gas is directly proportional to its temperature; i.e. doulbing the temperature of a gas will double the volume it takes up (and vice-versa). Pressure law: the pressure of a gas is directly proportional to its temperature; i.e. doubling the temperature of a gas will double the pressure placed upon the gas (and vice-versa). These three laws can be combined with another to give the ideal gas law: PV = nRT (where P = pressure, V = volume, n = number of moles, R = universal gas constant and T = temperature in Kelvin). But seriously, next time, just Google it - it'll be faster. Or maybe read a textbook?
What effect does an increase in temperature have on a gas's volume and pressure?
As indicated by the Ideal Gas Laws, increasing temperature will tend to increase both volume and pressure. Of course, volume can't always increase, that depends upon the flexibility or inflexibility of the container that the gas is in, and if the volume does increase that will counteract the increase in pressure that would otherwise have happened. Temperature, pressure, and volume are all interconnected in a gas.
When a gas is cooled it?
The Ideal Gas Laws describe the relationship of temperature, pressure, and volume for a gas. These three things are all related. At lower temperatures a gas will exert lower pressure if the volume remains the same, or can exert the same pressure but in a smaller volume.
What is the formula that expresses the ideal gas law which three gas laws does it combine?
PV=NKbT Where: P is the pressure V is the volume N is number of molecules T is the temperature in kelvin
How are pressure volume and temperature of gases related?
The temperature, pressure, and volume of gases can be related by the ideal gas equation. PV = nRT where P is pressure, V is volume, n is moles, R is that ideal gas constant, and T is the temperature in Kelvin.
What is the relationship between temperature and pressure?
The relation between temperature and pressure is known as Gay-Lussac's law, one of the gas laws. It states that the pressure exerted on a container's sides by an ideal gas is proportional to the absolute temperature of the gas.As an equation this is P=kTIn words as the pressure in sealed container goes up, the temperature goes up, or as temperature goes up pressure goes up.
