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The second law of thermodynamics introduccd the concept of (1) third law of thermodynamics (2) work (3) entropy (4) internal energy

Short Answer

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The second law of thermodynamics introduced the concept of entropy.

Step by step solution

01

Identify the Second Law of Thermodynamics

The second law of thermodynamics states that in any cyclic process, the entropy will either increase or remain the same. It is a rule about the natural tendency of systems to move towards disorder or randomness.
02

Understand Key Concepts Related to the Question

Interpret the answers: 1. Third law of thermodynamics discusses absolute zero temperature.2. Work is related to energy transfer. 3. Entropy is a measure of disorder in a system.4. Internal energy is the total energy contained within a system.
03

Match Concept to Correct Answer

Based on the second law of thermodynamics, which introduces the concept that entropy increases in spontaneous processes, identify the correct answer as the concept of entropy.

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Key Concepts

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

Entropy
The term 'entropy' often seems complicated, but it’s essentially about disorder or randomness. Imagine a tidy room where everything is in its place. If someone starts messing up the room, it becomes disorganized. This increase in disorder is similar to how entropy works in a system.

Entropy quantifies the level of disorder. The second law of thermodynamics states that the total entropy of an isolated system can never decrease over time. Instead, it either increases or remains constant. This rule indicates that natural processes tend to move towards greater disorder. For instance, heat naturally flows from a hot object to a cold one, increasing the overall entropy.
  • Higher entropy means more disorder and randomness.
  • Total entropy of a closed system either increases or stays the same.
  • Processes that increase disorder are naturally favorable.
By understanding entropy, we grasp why certain processes occur spontaneously and why energy transformations are not entirely reversible.
Cyclic Processes
Cyclic processes are fundamental in thermodynamics, helping us understand how systems exchange energy. These processes consist of a series of steps that return the system to its initial state. Picture a piston in a car engine. After the piston completes one cycle (compression, ignition, expansion, and exhaust), it goes back to its starting position and the cycle starts over.

According to the second law of thermodynamics, during such cyclic processes, the entropy of the system will either increase or, in an ideal case, stay the same. This principle makes it clear why perpetual motion machines, which claim to operate indefinitely without energy input, are impossible. They would require a system where entropy decreases, violating natural laws.
  • A cyclic process returns a system to its original state.
  • During cyclic processes, entropy does not decrease.
  • This principle explains the direction of natural processes.
Cyclic processes help in creating mechanical work and understanding the efficiency of engines and other machinery.
Disorder
Disorder, in scientific terms, often refers to the concept of entropy. In our daily experiences, we see disorder in multiple ways. A deck of cards, when shuffled, transitions from an ordered state to a disordered one. Similarly, if you mix milk into coffee, it seamlessly blends, increasing the system’s disorder.

The second law of thermodynamics explains why this happens: systems naturally evolve towards states with higher disorder. This trend towards randomness is universal, affecting everything from small particles to vast galaxies. It’s why we don’t see eggs unbreaking or coffee separating from milk spontaneously.
  • Disorder equates to higher entropy.
  • Systems naturally progress towards higher entropy.
  • This principle explains irreversibility in natural processes.
Grasping the idea of disorder helps us understand a vast array of natural phenomena and reveals the inevitable nature of change and complexity in our universe.

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Most popular questions from this chapter

A gaseous reaction was carried out first keeping the volume constant and next keeping the pressure constant, In the second experiment, there was an increase in volume. The heats of reactions were different becanse (1) In the first ease, the energy was spent to keep the volume constant. (2) In the second case, the energy was spent to expand the gases. (3) Specific heats of compressed gases are more. (4) Specific heats of rarefied gases are more.

Equal volumes of \(1 \mathrm{M} \mathrm{HCl}\) and \(1 \mathrm{M} \mathrm{H}_{2} \mathrm{SO}_{4}\) are neutralized by dilute \(\mathrm{NaOH}\) solution and \(\mathrm{X}\) and \(\mathrm{Y}\) kcal of heat are liberated, respectively. Which of the following is true? (1) \(\mathrm{X}=\mathrm{Y}\) (2) \(\mathrm{X}=0.5 \mathrm{Y}\) (3) \(\mathrm{X}=0.4 \mathrm{Y}\) (4) None

Energy can be transferred from a system to its surroundings as work if (1) there is thermal equilibrium between system and surroundings (2) there is mechanical equilibrium between system and surroundings (3) if pressure of system \(>\) atmospheric pressure (4) if pressure of system \(<\) atmospheric pressure

Identify the correct statement regarding entropy (1) \Lambdat absolute zero of temperature, the entropy of perfectly crystalline substance is taken to be zaro. (2) At absolute zero of temperature, the cntropy of a perfoctly crystalline substance is taken to be zero. (3) At \(0^{\circ} \mathrm{C}\), the entropy of a perfoctly crystalline substance is taken to be zero. (4) \Lambdat absolute zcro of temperature, the entropy of all crystalline substances is taken to be zcro.

The wrong statement among the following is (1) The heat change for the reaction \(\mathrm{II}_{2} \mathrm{O}(1) \rightarrow\) \(\mathrm{II}_{2} \mathrm{O}(\mathrm{g})\) is known as heat of vapourisation. (2) The heat change in the reaction \(\mathrm{C}(\mathrm{s})+2 \mathrm{~S}(\mathrm{~s}) \rightarrow\) \(\mathrm{CS}_{2}\) (1) is called heat of formation of \(\mathrm{CS}_{2}\). (3) The standard heat cnthalpy of diamond is zero. (4) The enthalpy change \(\mathrm{C}_{(\mathrm{s})} \rightarrow \mathrm{C}_{(\mathrm{g})}\) is known as cnthalpy of sublimation.

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