The question asks about the characteristics of a system at equilibrium in a physical process. Equilibrium is a state where opposing processes occur at equal rates, resulting in no net change in the system's macroscopic properties.
Correct Option: D) Rate of forward process equals rate of reverse process
This statement accurately defines dynamic equilibrium. At equilibrium, the forward and reverse processes continue to occur, but their rates are equal, leading to no net change in the macroscopic properties of the system (like concentration, temperature, pressure, etc.).
The question asks to identify the type of equilibrium between ice and water at 273 K and 1 atm. This involves understanding the states of matter involved in the equilibrium.
C) Solid-liquid equilibrium. This is correct because ice is the solid form of water, and water is its liquid form. The coexistence of these two phases at 273 K (0°C) and 1 atm pressure represents a phase equilibrium between the solid and liquid states.
The question asks for the specific term describing the temperature at which a pure substance's solid and liquid phases coexist in equilibrium at atmospheric pressure. This is a fundamental concept in thermodynamics and phase transitions.
D) Normal melting point is the temperature at which the solid and liquid phases of a pure substance are in equilibrium at atmospheric pressure. This is the standard definition for this phase transition under specified conditions.
The equilibrium vapour pressure of a liquid is a fundamental property that describes the pressure exerted by its vapour when it is in thermodynamic equilibrium with its condensed phase (liquid) in a closed system. We need to identify the factors that influence this intrinsic property.
The boiling point of a liquid is directly related to its vapor pressure. We need to understand this relationship to determine which characteristic leads to the lowest boiling point.
Correct Option: D) The one with the highest vapour pressure at a given temperature.
A liquid with a high vapor pressure at a given temperature means its molecules readily escape into the gas phase. This implies that less additional energy (heat) is needed to raise its vapor pressure to meet the external atmospheric pressure, thus resulting in a lower boiling point.
The question asks why equilibrium cannot be reached in an open system for a liquid-vapour transition. This requires understanding the conditions for dynamic equilibrium, particularly in the context of phase transitions.
D) Vapour molecules disperse into the surroundings, so rate of condensation cannot equal rate of evaporation. This accurately describes why equilibrium cannot be reached. The continuous loss of vapour molecules prevents the build-up of vapour concentration required for the condensation rate to match the evaporation rate.