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Gases behave differently at different pressures and temperatures. At low pressures, gases expand to fill the available space. At high pressures, gases become more compact. At low temperatures, gases condense into liquids or solids. At high temperatures, gases expand and exert greater pressure.
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Is Boyle's law true for all gases?
Boyle's law is generally true for ideal gases, which means they behave with perfect elasticity and do not interact with each other. Real gases may deviate from Boyle's law at high pressures or low temperatures due to the presence of intermolecular forces or molecular volume.
Which are incompressible gases?
Incompressible gases are theoretical concepts as, under normal conditions, all gases can be compressed to some degree. However, in practice, gases like helium and hydrogen are considered to behave as incompressible fluids under certain high-pressure conditions, where their density changes very little with pressure. Additionally, at very low temperatures and high pressures, some real gases can approach incompressibility. Generally, liquids are deemed incompressible, while gases are not.
What gas doesn't behave according to the kinetic molecular theory?
Real gases do not always behave according to the kinetic molecular theory, especially at high pressures or low temperatures where intermolecular forces become significant. At these conditions, the volume of the gas particles themselves and the attractions between them become non-negligible, leading to deviations from ideal gas behavior.
What is difference between ideal gas and non ideal gas?
Ideal gases are hypothetical gases that follow the gas laws perfectly under all conditions, exhibiting no intermolecular forces and occupying no volume. In contrast, non-ideal gases deviate from these behaviors due to factors such as intermolecular attractions and the volume occupied by gas molecules, especially at high pressures and low temperatures. These deviations lead to differences in properties like pressure, volume, and temperature relationships, making real gases behave differently from the ideal gas law predictions.
Could carbon be compressed?
Yes, carbon can be compressed under high pressure to form different allotropes such as diamond. Diamond is a crystalline form of carbon that is the result of carbon being compressed at extreme pressures and temperatures deep within the Earth's mantle.
Do real gases behave like ideal gases except at very high temperatures?
Gases behave most ideally at low pressure and high temperatures. At low pressures, the average distance of separation among atoms or molecules is greatest, minimizing interactive forces. At high temperatures, the atoms and molecules are in rapid motion and are able to overcome interactive forces more easily.
Under which conditions does a real gas behave most like an ideal gas?
Real gases behave most like ideal gases under conditions of low pressure and high temperature. At low pressures, the volume of gas molecules is significant compared to the volume of the container, and at high temperatures, intermolecular forces are minimized, allowing the gas molecules to behave more independently.
Which gas will be highest expand by heat?
Different gases will expand at the same rate. At twice the absolute temperature, the volume will also double (assuming the pressure stays the same). At very high pressures or very low temperatures there may be some deviations from this rule, which is part of the general gas law; but under most normal circumstances, most gases behave more or less like an "ideal gas".Different gases will expand at the same rate. At twice the absolute temperature, the volume will also double (assuming the pressure stays the same). At very high pressures or very low temperatures there may be some deviations from this rule, which is part of the general gas law; but under most normal circumstances, most gases behave more or less like an "ideal gas".Different gases will expand at the same rate. At twice the absolute temperature, the volume will also double (assuming the pressure stays the same). At very high pressures or very low temperatures there may be some deviations from this rule, which is part of the general gas law; but under most normal circumstances, most gases behave more or less like an "ideal gas".Different gases will expand at the same rate. At twice the absolute temperature, the volume will also double (assuming the pressure stays the same). At very high pressures or very low temperatures there may be some deviations from this rule, which is part of the general gas law; but under most normal circumstances, most gases behave more or less like an "ideal gas".
Why do gases behave most ideally?
is it true the space between gas particles becomes very large
When do gases deviate from ideal behavior?
Gases deviate from ideal behavior at high pressures and low temperatures.
Is Boyle's law true for all gases?
Boyle's law is generally true for ideal gases, which means they behave with perfect elasticity and do not interact with each other. Real gases may deviate from Boyle's law at high pressures or low temperatures due to the presence of intermolecular forces or molecular volume.
Which are incompressible gases?
Incompressible gases are theoretical concepts as, under normal conditions, all gases can be compressed to some degree. However, in practice, gases like helium and hydrogen are considered to behave as incompressible fluids under certain high-pressure conditions, where their density changes very little with pressure. Additionally, at very low temperatures and high pressures, some real gases can approach incompressibility. Generally, liquids are deemed incompressible, while gases are not.
What gas doesn't behave according to the kinetic molecular theory?
Real gases do not always behave according to the kinetic molecular theory, especially at high pressures or low temperatures where intermolecular forces become significant. At these conditions, the volume of the gas particles themselves and the attractions between them become non-negligible, leading to deviations from ideal gas behavior.
What information can be found in the viscosity table?
The viscosity table provides information about the viscosity of different substances, which is a measure of their resistance to flow. It typically includes data on the viscosity of liquids and gases at various temperatures and pressures.
What is the thermal expansion coefficient of air and how does it affect the behavior of gases in different temperature environments?
The thermal expansion coefficient of air is approximately 0.00367 per degree Celsius. This means that as the temperature of air increases, its volume also increases. In different temperature environments, gases behave differently due to their thermal expansion coefficients. For example, in warmer temperatures, gases expand and occupy more space, while in colder temperatures, gases contract and occupy less space.
Is the ammonia Haber Bosch process dangerous?
Working with gases (especially hydrogen and ammonia) at high temperatures and pressures may be dangerous.
What will happen when two different gases at different pressure mixes in a single pipe?
The pressure will equalise and the two gases will mix.
