Two liquids X and Y boil at 110 0 c and 1300 c respectively which one of them has higher vapour pressure at 500 c ?

To determine which liquid, X or Y, has a higher vapor pressure at 500 °C, we need to consider the relationship between boiling points and vapor pressures. Generally, a liquid's vapor pressure increases with temperature, and it is also influenced by the boiling point of the liquid. Let's break this down step by step.

Understanding Vapor Pressure

Vapor pressure is the pressure exerted by a vapor in equilibrium with its liquid or solid form. It indicates how readily a substance evaporates. The higher the vapor pressure at a given temperature, the more volatile the substance is, meaning it can transition from liquid to gas more easily.

Boiling Point and Vapor Pressure Relationship

The boiling point of a liquid is the temperature at which its vapor pressure equals the atmospheric pressure. Therefore, a liquid with a lower boiling point will generally have a higher vapor pressure at a given temperature compared to a liquid with a higher boiling point. In this case:

• Liquid X boils at 110 °C.
• Liquid Y boils at 130 °C.

Analyzing the Scenario

At 500 °C, both liquids are well above their boiling points. This means that both X and Y will be in the vapor phase, but their vapor pressures will still depend on their boiling points. Since liquid X has a lower boiling point (110 °C) compared to liquid Y (130 °C), it will have a higher vapor pressure at 500 °C.

Conclusion

In summary, liquid X, which boils at 110 °C, will have a higher vapor pressure at 500 °C than liquid Y, which boils at 130 °C. This is because substances with lower boiling points tend to have higher vapor pressures at elevated temperatures, making them more volatile. Thus, at 500 °C, liquid X is the more volatile of the two.