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Why is HCl less ideal than CH4, He and N2?
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+ Methane
+ Helium
+ Hydrochloric acid
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Adam Moss
Why is HCl less ideal than CH4, He and N2?
due to hydrogen bonding in HCl it behaves real gases than CH4, He, and N2 as they contain instantaneous dipole interactions as inter-molecular forces so these gases show more ideal behavior than HCl……
it is to be noted that ideal gas does not have inter-molecular forces.
due to hydrogen bonding in HCl it behaves real gases than CH4, He, and N2 as they contain instantaneous dipole interactions as inter-molecular forces so these gases show more ideal behavior than HCl……
it is to be noted that ideal gas does not have inter-molecular forces.
How do we find which gas shows the maximum deviation from the ideal gas behaviour?
An ideal gas is one in which
(a) the particles are merely point masses (the particles have no size or volume), and
(b) there is no interaction (attraction or repulsion) between the particles (atoms or molecules).
Clearly, these theoretical conditions are difficult to obtain in the case of real gases because (1) real molecules do have some size or volume of their own and (2) there will be some attraction or repulsion acting between the particles, especially when the molecules come very close to each other.
Real gases show nearly ideal behavior under following conditions:
(a) when the temperature is very high (This is because at high temperatures the volume occupied the gas will be very large; compared to this large volume, the actual sizes of the molecule will be small and may be neglected. The entire volume of the gas will be available for the molecules to move around. The molecules are far from each other, so any interaction between them is negligible. The molecules then can be treated as point masses satisfying condition (a) for ideal gas).
(b) at very low pressure (at very high pressure, the volume occupied the gas will be very small. The molecules themselves will take up a considerable fraction of this volume. So the volume available for the free movement of the particles will be even lesser. A second reason is that at high pressure when the volume occupied is small, the molecules are very close to each other and effects of attraction or repulsion between them becomes prominent. Thus conditions (a) and (b) for ideal nature cannot exist at high pressure).
How do we find which gas shows the maximum deviation from the ideal gas behaviour?
An ideal gas is one in which
(a) the particles are merely point masses (the particles have no size or volume), and
(b) there is no interaction (attraction or repulsion) between the particles (atoms or molecules).
Clearly, these theoretical conditions are difficult to obtain in the case of real gases because (1) real molecules do have some size or volume of their own and (2) there will be some attraction or repulsion acting between the particles, especially when the molecules come very close to each other.
Real gases show nearly ideal behavior under following conditions:
(a) when the temperature is very high (This is because at high temperatures the volume occupied the gas will be very large; compared to this large volume, the actual sizes of the molecule will be small and may be neglected. The entire volume of the gas will be available for the molecules to move around. The molecules are far from each other, so any interaction between them is negligible. The molecules then can be treated as point masses satisfying condition (a) for ideal gas).
(b) at very low pressure (at very high pressure, the volume occupied the gas will be very small. The molecules themselves will take up a considerable fraction of this volume. So the volume available for the free movement of the particles will be even lesser. A second reason is that at high pressure when the volume occupied is small, the molecules are very close to each other and effects of attraction or repulsion between them becomes prominent. Thus conditions (a) and (b) for ideal nature cannot exist at high pressure).
due to hydrogen bonding in HCl it behaves real gases than CH4, He, and N2 as they contain instantaneous dipole interactions as inter-molecular forces so these gases show more ideal behavior than HCl……
it is to be noted that ideal gas does not have inter-molecular forces.
due to hydrogen bonding in HCl it behaves real gases than CH4, He, and N2 as they contain instantaneous dipole interactions as inter-molecular forces so these gases show more ideal behavior than HCl……
it is to be noted that ideal gas does not have inter-molecular forces.
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How do we find which gas shows the maximum deviation from the ideal gas behaviour?
An ideal gas is one in which
(a) the particles are merely point masses (the particles have no size or volume), and
(b) there is no interaction (attraction or repulsion) between the particles (atoms or molecules).
Clearly, these theoretical conditions are difficult to obtain in the case of real gases because (1) real molecules do have some size or volume of their own and (2) there will be some attraction or repulsion acting between the particles, especially when the molecules come very close to each other.
Real gases show nearly ideal behavior under following conditions:
(a) when the temperature is very high (This is because at high temperatures the volume occupied the gas will be very large; compared to this large volume, the actual sizes of the molecule will be small and may be neglected. The entire volume of the gas will be available for the molecules to move around. The molecules are far from each other, so any interaction between them is negligible. The molecules then can be treated as point masses satisfying condition (a) for ideal gas).
(b) at very low pressure (at very high pressure, the volume occupied the gas will be very small. The molecules themselves will take up a considerable fraction of this volume. So the volume available for the free movement of the particles will be even lesser. A second reason is that at high pressure when the volume occupied is small, the molecules are very close to each other and effects of attraction or repulsion between them becomes prominent. Thus conditions (a) and (b) for ideal nature cannot exist at high pressure).
This is illustrated in the following diagrams:
How do we find which gas shows the maximum deviation from the ideal gas behaviour?
An ideal gas is one in which
(a) the particles are merely point masses (the particles have no size or volume), and
(b) there is no interaction (attraction or repulsion) between the particles (atoms or molecules).
Clearly, these theoretical conditions are difficult to obtain in the case of real gases because (1) real molecules do have some size or volume of their own and (2) there will be some attraction or repulsion acting between the particles, especially when the molecules come very close to each other.
Real gases show nearly ideal behavior under following conditions:
(a) when the temperature is very high (This is because at high temperatures the volume occupied the gas will be very large; compared to this large volume, the actual sizes of the molecule will be small and may be neglected. The entire volume of the gas will be available for the molecules to move around. The molecules are far from each other, so any interaction between them is negligible. The molecules then can be treated as point masses satisfying condition (a) for ideal gas).
(b) at very low pressure (at very high pressure, the volume occupied the gas will be very small. The molecules themselves will take up a considerable fraction of this volume. So the volume available for the free movement of the particles will be even lesser. A second reason is that at high pressure when the volume occupied is small, the molecules are very close to each other and effects of attraction or repulsion between them becomes prominent. Thus conditions (a) and (b) for ideal nature cannot exist at high pressure).
This is illustrated in the following diagrams:
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