Positive deviation from ideal gas behaviour takes place because of- A)...
Introduction
An ideal gas is a theoretical gas that follows the gas laws, and there are no interactions between its molecules. However, in reality, gases deviate from these ideal behaviors under certain conditions. This deviation occurs because of various factors that affect the behavior of gases.
Molecular Interactions
Molecules in real gases interact with each other, leading to deviations from ideal gas behavior. These interactions affect the volume and pressure of the gas. In the case of attractive forces between molecules, the gas has a lower pressure than that predicted by the ideal gas law. Conversely, when there are repulsive forces between molecules, the pressure of the gas is higher than the value predicted by the ideal gas law. The degree of deviation from ideal gas behavior is measured by the compressibility factor (Z). Z is the ratio of the observed pressure to the pressure predicted by the ideal gas law.
Finite Size of Molecules
The ideal gas law assumes that gas molecules have zero volume, which is not the case in real gases. The volume of gas molecules is significant for high-pressure gases and low-temperature gases. As the pressure of the gas increases, the volume of the gas molecules becomes more significant, leading to a decrease in the volume available for the movement of the gas molecules. This decrease in volume leads to a reduction in the pressure of the gas, leading to a deviation from ideal gas behavior.
Conclusion
In conclusion, deviations from ideal gas behavior occur due to molecular interactions and finite size of molecules. These deviations are measured by the compressibility factor (Z), which is the ratio of the observed pressure to the pressure predicted by the ideal gas law. The degree of deviation varies depending on the conditions of the gas.
Positive deviation from ideal gas behaviour takes place because of- A)...
Answer is A .real gasses deviates from ideal behaviour due to two wrong assumption in kinetic theory of gasses.that first gas molecules have no volume and second there is no force of attraction between the gas molecules.due to this a correction term z that is compressibility factor use.when z is greater than one gas show positive deviation. at high pressure.
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