Is it true that water boils at higher temperature at higher pressure? Explain your reasons with the aid of the T-v diagram. The diagram should include the saturated liquid/vapor line, the saturated temperature and pressure, proper labeling on the axis.

Question

Accepted Answer

∻Solution∻ ‖ a ⋮ Yes, it is true that water boils at a higher temperature at higher pressure. This is because the boiling point of a liquid is the temperature at which its vapor pressure equals the external pressure. As pressure increases, the temperature required for the vapor pressure to match this external pressure also increases. This relationship can be illustrated on a T-v diagram, where the saturated liquid/vapor line shows the phase change between liquid and vapor. ‖ ‖ b ⋮ In the T-v diagram, the x-axis represents temperature (T) and the y-axis represents specific volume (v). The saturated liquid line (left) and the saturated vapor line (right) define the phase boundaries. As pressure increases, the entire curve shifts upward, indicating that at higher pressures, the corresponding boiling temperature increases. The critical point is where the saturated liquid and vapor lines meet, beyond which the distinction between liquid and vapor disappears. ‖ ∻Answer∻ ⚹ Water boils at a higher temperature at higher pressure. ⚹ ∻Key Concept∻ ⚹ Boiling Point and Vapor Pressure: The boiling point of a liquid is the temperature at which its vapor pressure equals the external pressure. As external pressure increases, the boiling point also increases. This is represented in phase diagrams, particularly the T-v diagram. ⚹ ∻Explanation∻ ⚹ The relationship between pressure and boiling point is crucial in understanding phase changes in fluids. Higher pressure requires higher temperatures for the vapor pressure to equal the external pressure, thus raising the boiling point. ⚹

Sia