The increase of pressure on ice ? water at a constant temperature will cause
- water to vaporize
- water to freeze
- no change
- ice to melt
The Correct Option is D
Solution and Explanation
To understand the effect of pressure on the phase transition from ice to water at constant temperature, we should consider the phase diagram of water. The phase diagram illustrates the state of water (solid, liquid, or gas) under different conditions of temperature and pressure.
According to the phase diagram of water, an increase in pressure can lead to the transition from one phase to another. In the case of ice, when pressure is increased at constant temperature, the process can be understood as follows:
- Phase Diagram Explanation: At temperatures below 0°C, water is usually in the solid phase, known as ice. The phase diagram shows that the melting curve for ice has a negative slope. This is a unique property of water.
- Effect of Pressure: For most substances, an increase in pressure usually supports the solid phase. However, because the ice melting curve has a negative slope, increasing pressure at a constant temperature actually favors the liquid phase (water). This means that ice will melt into water under increased pressure.
- Reasoning: The unusual behavior of water is due to the fact that ice is less dense than liquid water. When pressure is applied, it makes it energetically more favorable for ice to convert into liquid water, which occupies a smaller volume.
Therefore, the correct answer to the question is that an increase in pressure on ice at a constant temperature will cause the ice to melt.
This phenomenon is also the reason why ice skates glide smoothly over ice. The pressure exerted by the skate's blade causes a thin layer of ice to melt, creating a slippery surface.
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Concepts Used:
Equilibrium
An equilibrium represents a state in a process when the observable properties such as color, temperature, pressure, concentration etc do not show any change.
The word equilibrium means ‘balance’ which indicates that a chemical reaction represents a balance between the reactants and products taking part in the reaction. The equilibrium state is also noticed in certain physical processes such as the melting point of ice at 0℃, both ice and water are present at equilibrium.
In the case of physical processes such as the melting of solid, dissolution of salt in water etc., the equilibrium is called physical equilibrium while the equilibrium associated with chemical reaction is known as chemical equilibrium.
Equilibrium in Chemical changes
The chemical equilibrium in a reversible reaction is the state at which both forward and backward reactions occur at the same speed.
The stage of the reversible reaction at which the concentration of the reactants and products do not change with time is called the equilibrium state.
Read More: Calculating Equilibrium Concentration
Types of Chemical Equilibrium
There are two types of chemical equilibrium:
- Homogeneous Equilibrium
- Heterogeneous Equilibrium
Homogenous Chemical Equilibrium
In this type, the reactants and the products of chemical equilibrium are all in the same phase. Homogenous equilibrium can be further divided into two types: Reactions in which the number of molecules of the products is equal to the number of molecules of the reactants. For example,
- H2 (g) + I2 (g) ⇌ 2HI (g)
- N2 (g) + O2 (g) ⇌ 2NO (g)
Reactions in which the number of molecules of the products is not equal to the total number of reactant molecules. For example,
- 2SO2 (g) + O2 (g) ⇌ 2SO3 (g)
- COCl2 (g) ⇌ CO (g) + Cl2 (g)
Heterogeneous Chemical Equilibrium
In this type, the reactants and the products of chemical equilibrium are present in different phases. A few examples of heterogeneous equilibrium are listed below.
- CO2 (g) + C (s) ⇌ 2CO (g)
- CaCO3 (s) ⇌ CaO (s) + CO2 (g)
Thus, the different types of chemical equilibrium are based on the phase of the reactants and products.
Check Out: Equilibrium Important Questions