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In thermodynamics, which one of the following properties is not an intensive property? (a) Pressure (b) Temperature (c) Volume (d) Density

Short Answer

Expert verified
Volume (c) is not an intensive property; it is an extensive property.

Step by step solution

01

Define Intensive Properties

Intensive properties are those properties of a system that do not depend on the mass or the size of the system. Examples of intensive properties include pressure, temperature, and density.
02

Identify Extensive Properties

Extensive properties are those that do depend on the system size or the amount of substance present. The value of an extensive property is proportional to the mass or size of the system.
03

Analyze the Given Options

By definition, we know that pressure, temperature, and density are intensive properties, as they do not change with the amount of substance. Volume, on the other hand, is an extensive property because it depends on the quantity of material.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Thermodynamics
Thermodynamics is a branch of physics that studies the relationships between heat, work, temperature, and energy. In essence, it investigates how thermal energy is converted to and from other forms of energy and how it affects matter.

The laws of thermodynamics dictate how and why energy is transferred, and these principles have paramount importance in fields such as engineering, chemistry, and environmental science. Understanding these concepts is crucial to grasp how the physical world operates, especially when analyzing systems in terms of temperature, heat, and energy flow.
Pressure
Pressure is an intensive property defined as force per unit area. It represents the amount of force applied to an area and is independent of the amount of material in the system. In thermodynamic terms, the pressure can be thought of as the molecular impacts per unit area on the walls of a container.

In applications ranging from weather systems to the functioning of engines and the design of aerodynamic objects, understanding pressure is crucial. It’s measured in units such as pascals (Pa) or pounds per square inch (psi) and can be expressed through the equation \( P = \frac{F}{A} \) where \( P \) is pressure, \( F \) is force, and \( A \) is area.
Temperature
Temperature is a measure of the average kinetic energy of particles in a substance and is another intensive property, which means it's not dependent on the amount of substance present. It quantifies the degree of heat or cold in a system.

Temperature is most commonly measured in degrees Celsius (°C), Fahrenheit (°F), or Kelvin (K). It plays a vital role in thermodynamics by defining the direction in which heat energy will flow—naturally from a hotter object to a colder one, until equilibrium is reached.
Density
Density is defined as the mass per unit volume of a substance and is an intensive property. It informs us about how tightly matter is packed within a certain volume. This property is particularly helpful for identifying substances and understanding their buoyancy in a fluid.

The formula for density is \( \rho = \frac{m}{V} \) where \( \rho \) is density, \( m \) is mass, and \( V \) is volume. Different substances have different densities, which is why objects made of one material will sink or float when placed in a fluid of another material.
Volume
Volume, in contrast to the intensive properties we've discussed, is an extensive property that depends on the amount of substance in a system. It represents the three-dimensional space occupied by a substance or an object.

Volume is crucial in thermodynamics for understanding how gases expand and contract with changes in temperature and pressure. It's also essential in applications such as dosing chemicals, designing containers, or calculating fluid flow. Volume is usually measured in liters (L), cubic meters (m³), or gallons (gal), among other units.

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Most popular questions from this chapter

At \(373 \mathrm{~K}\), steam and water are in equilibrium and \(\Delta H=40.98 \mathrm{~kJ} \mathrm{~mol}^{-1}\). What will be \(\Delta S\) for conversion of water into steam? \(\mathrm{H}_{2} \mathrm{O}_{(l)} \rightarrow \mathrm{H}_{2} \mathrm{O}_{(g)}\) (a) \(109.8 \mathrm{JK}^{-1} \mathrm{~mol}^{-1}\) (b) \(31^{-1} \mathrm{JK}^{-1} \mathrm{~mol}^{-1}\) (c) \(21.93 \mathrm{~J} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}\) (d) \(326 \mathrm{~J} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}\)

Match the following columns and mark the appropriate choice. \(\begin{array}{|l|l|l|l|} \hline {\text { Column I }} & & {\text { Column II }} \\ \hline \text { (A) } & \text { Exothermic } & \text { (i) } & \Delta H=0, \Delta E=0 \\ \hline \text { (B) } & \text { Spontaneous } & \text { (ii) } & \Delta G=0 \\ \hline \text { (C) } & \text { Cyclic process } & \text { (iii) } & \Delta H \text { is negative. } \\ \hline \text { (D) } & \text { Equilibrium } & \text { (iv) } & \Delta G \text { is negative. } \\ \hline \end{array}\) (a) \((\mathrm{A}) \rightarrow(\mathrm{ii}),(\mathrm{B}) \rightarrow(\mathrm{iii}),(\mathrm{C}) \rightarrow(\mathrm{i}),(\mathrm{D}) \rightarrow(\mathrm{iv})\) (b) \((\mathrm{A}) \rightarrow(\mathrm{iv}),(\mathrm{B}) \rightarrow(\mathrm{i}),(\mathrm{C}) \rightarrow(\mathrm{iii}),(\mathrm{D}) \rightarrow\) (ii) (c) (A) \(\rightarrow\) (i), (B) \(\rightarrow\) (ii), (C) \(\rightarrow\) (iv), (D) \(\rightarrow\) (iii) (d) \((A) \rightarrow(i i i),(B) \rightarrow(i v),(C) \rightarrow(i),(D) \rightarrow(i i)\)

System in which there is no exchange of matter, work or energy from surroundings is (a) closed (b) adiabatic (c) isolated (d) isothermal

At what temperature liquid water will be in equilibrium with water vapour? \(\Delta H_{v a p}=40.73 \mathrm{~kJ} \mathrm{~mol}^{-1}, \Delta S_{v a p}=0.109 \mathrm{~kJ} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}\) (a) \(282.4 \mathrm{~K}\) (b) \(373.6 \mathrm{~K}\) (c) \(100 \mathrm{~K}\) (d) \(400 \mathrm{~K}\)

What is the entropy change when 1 mole oxygen gas expands isothermally and reversibly from an initial volume of \(10 \mathrm{~L}\) to \(100 \mathrm{~L}\) at \(300 \mathrm{~K} ?\) (a) \(19.14 \mathrm{JK}^{-1}\) (b) \(109.12] \mathrm{K}^{-1}\) (c) \(29.12 \mathrm{JK}^{-1}\) (d) \(10 \mathrm{~K}^{-1}\)

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