Question

For a real gas, deviations from ideal gas behaviour are maximum at (1) \(10^{\circ} \mathrm{C}\) and \(5 \mathrm{~atm}\) (2) \(10^{\circ} \mathrm{C}\) and \(2 \mathrm{~atm}\) (3) \(0^{\circ} \mathrm{C}\) and \(1 \mathrm{~atm}\) (4) \(100^{\circ} \mathrm{C}\) and \(2 \mathrm{~atm}\)

Short answer

Option (1) 10°C and 5 atm.

Step-by-step solution

Understand Real Gas Behavior

Real gases deviate from ideal gas behavior due to intermolecular forces and the finite volume of gas molecules. The deviation is more pronounced at high pressures and low temperatures.

Analyze Given Conditions

Evaluate the conditions given in the options: (1) 10°C, 5 atm; (2) 10°C, 2 atm; (3) 0°C, 1 atm; (4) 100°C, 2 atm.

Identify the Extreme Conditions

Note that deviations from ideal gas behavior are maximum when the gas is either at high pressure or low temperature.

Compare All Options

Compare each condition based on temperature and pressure. The condition with the highest pressure and lowest temperature should show the greatest deviation.

Conclusion

Identify 10°C and 5 atm as the conditions with the highest pressure among the given options, likely showing the maximum deviation from ideal gas behavior.

Key concepts

Ideal Gas Deviation

Ideal gases are a theoretical concept where gas particles move independently and do not interact with each other. Real gases, however, exhibit deviations from this behavior due to two main reasons: the intermolecular forces between gas molecules and the finite volume of the gas molecules themselves. According to the ideal gas law, the equation is represented as If.interactive.forces are.most of the behavior as to the finite volume. Additionally, an .=i. { other.real.gases. units of temperature and pressure in an ideal manner. Conversely, deviations include the volume of the gas as being finite as the temperature of the molecule and K< applications.gases < may.deviation will of from lit.

High Pressure Gas

When dealing with a high-pressure gas, the close proximity of the gas molecules means that the effects of intermolecular forces become more pronounced. Accordingly, because of these interactions, they cannot be ignored as they can significantly alter the behavior of the gas from an ideal gas. High pressure forces the gas molecules closer together, increasing the effect of repulsive forces due to the finite volume of the molecules. This scenario is critical in understanding why gases at high pressure deviate the most from ideal behavior.

High pressure can thus impact gas behavior in the following ways:

• Increased intermolecular collisions
• Pronounced repulsive forces
• Alteration in compressibility

Recognizing these impacts can help you in identifying how gas properties change and why they need to be accounted for in real-world applications.

Low Temperature Gas

At low temperatures, the kinetic energy of gas molecules decreases. This slowing down of molecules makes the attractive forces between them more significant relative to their motion. When the molecules lose energy and move more sluggishly, the effects of attraction can no longer be ignored, causing the gas to deviate from ideal behavior. This condition is particularly true for gases approaching liquefaction.

Key points regarding gases at low temperature:

• Reduced kinetic energy
• Increased significance of attractive forces
• Greater deviation from ideal gas behavior

Understanding the behavior at low temperatures is crucial for studying real gas properties, making it easier to identify and predict how gases will behave under different temperature conditions.