In an adiabatic change, a thermodynamic process occurs without any heat exchange between the system and its surroundings, meaning the heat remains unchanged. This is achieved by perfectly insulating the system. Despite no heat transfer, the temperature of the system can change as a result of work beRead more
In an adiabatic change, a thermodynamic process occurs without any heat exchange between the system and its surroundings, meaning the heat remains unchanged. This is achieved by perfectly insulating the system. Despite no heat transfer, the temperature of the system can change as a result of work being done on or by the system. For example, in an adiabatic expansion, the system does work on the surroundings, leading to a decrease in temperature, while in adiabatic compression, work is done on the system, causing an increase in temperature. This principle is crucial in understanding processes like the expansion of gases in engines or atmospheric phenomena. The conservation of energy still applies, but the energy change manifests solely as changes in internal energy, not heat transfer. Therefore, in an adiabatic change, the correct answer is [A] Heat remains unchanged.
The concept of internal energy is fundamentally derived from the first law of thermodynamics, which is also known as the law of energy conservation. This law states that energy cannot be created or destroyed, only transformed from one form to another within a closed system. Internal energy refers toRead more
The concept of internal energy is fundamentally derived from the first law of thermodynamics, which is also known as the law of energy conservation. This law states that energy cannot be created or destroyed, only transformed from one form to another within a closed system. Internal energy refers to the total energy contained within a system, encompassing both the kinetic energy of particles and the potential energy arising from intermolecular forces. The first law of thermodynamics provides a comprehensive framework for understanding how energy is stored, transferred, and conserved within a system. It articulates that the change in internal energy of a system is equal to the heat added to the system minus the work done by the system on its surroundings. This foundational principle is crucial for analyzing thermodynamic processes and systems in various scientific and engineering applications. Therefore, the correct answer is [B] First law.
The first law of thermodynamics, or the law of energy conservation, is fundamental in physics and thermodynamics. It asserts that the total energy in an isolated system remains constant. This means energy can neither be created nor destroyed; it can only change forms, such as from kinetic to potentiRead more
The first law of thermodynamics, or the law of energy conservation, is fundamental in physics and thermodynamics. It asserts that the total energy in an isolated system remains constant. This means energy can neither be created nor destroyed; it can only change forms, such as from kinetic to potential energy, or from chemical energy to thermal energy. The principle does not directly address momentum, which is conserved in a different context under Newton’s laws of motion. The conservation of energy applies universally across all processes, ensuring that the total energy before and after any transformation or transfer remains equal. This law underpins much of modern physics and engineering, dictating how energy systems are analyzed and designed. Thus, while momentum conservation is a crucial concept in its own right, it is the conservation of energy that is explicitly protected by the first law of thermodynamics. Therefore, the correct answer is [B] Energy.
Steam burns hands more severely than boiling water due to the latent heat it contains; option [A]. Latent heat is the extra energy required to change water from liquid to vapor without changing its temperature. When steam comes into contact with the skin, it condenses back into liquid water, releasiRead more
Steam burns hands more severely than boiling water due to the latent heat it contains; option [A]. Latent heat is the extra energy required to change water from liquid to vapor without changing its temperature. When steam comes into contact with the skin, it condenses back into liquid water, releasing this stored latent heat. This process transfers a significant amount of energy to the skin, which is much more than what boiling water would transfer at the same temperature. Boiling water only transfers heat at 100°C, but when steam condenses, it releases additional heat as it changes phase from gas to liquid. This results in a higher amount of energy being delivered to the skin, causing more severe burns. Therefore, the presence of latent heat in steam is the primary reason it causes more intense burns than boiling water.
The latent heat of vaporization of water is 536 Cal/g, which is the amount of heat needed to convert 1 gram of water at its boiling point (100°C) into steam without any change in temperature. This latent heat is crucial in understanding why steam causes more severe burns than boiling water. When steRead more
The latent heat of vaporization of water is 536 Cal/g, which is the amount of heat needed to convert 1 gram of water at its boiling point (100°C) into steam without any change in temperature. This latent heat is crucial in understanding why steam causes more severe burns than boiling water. When steam condenses on the skin, it releases this latent heat, transferring a substantial amount of energy to the skin. This energy transfer is significantly higher than that of boiling water at the same temperature, leading to more severe burns. Therefore, the correct answer to the latent heat of vaporization of water is [A] 536 Cal/g. This concept is essential in various fields, including thermodynamics and medical treatment of burns, highlighting the importance of understanding the thermal properties of substances.
What happen in Adiabatic Change
In an adiabatic change, a thermodynamic process occurs without any heat exchange between the system and its surroundings, meaning the heat remains unchanged. This is achieved by perfectly insulating the system. Despite no heat transfer, the temperature of the system can change as a result of work beRead more
In an adiabatic change, a thermodynamic process occurs without any heat exchange between the system and its surroundings, meaning the heat remains unchanged. This is achieved by perfectly insulating the system. Despite no heat transfer, the temperature of the system can change as a result of work being done on or by the system. For example, in an adiabatic expansion, the system does work on the surroundings, leading to a decrease in temperature, while in adiabatic compression, work is done on the system, causing an increase in temperature. This principle is crucial in understanding processes like the expansion of gases in engines or atmospheric phenomena. The conservation of energy still applies, but the energy change manifests solely as changes in internal energy, not heat transfer. Therefore, in an adiabatic change, the correct answer is [A] Heat remains unchanged.
See lessThe concept of internal energy is derived from which law of thermodynamics?
The concept of internal energy is fundamentally derived from the first law of thermodynamics, which is also known as the law of energy conservation. This law states that energy cannot be created or destroyed, only transformed from one form to another within a closed system. Internal energy refers toRead more
The concept of internal energy is fundamentally derived from the first law of thermodynamics, which is also known as the law of energy conservation. This law states that energy cannot be created or destroyed, only transformed from one form to another within a closed system. Internal energy refers to the total energy contained within a system, encompassing both the kinetic energy of particles and the potential energy arising from intermolecular forces. The first law of thermodynamics provides a comprehensive framework for understanding how energy is stored, transferred, and conserved within a system. It articulates that the change in internal energy of a system is equal to the heat added to the system minus the work done by the system on its surroundings. This foundational principle is crucial for analyzing thermodynamic processes and systems in various scientific and engineering applications. Therefore, the correct answer is [B] First law.
See lessThe first law of thermodynamics protects
The first law of thermodynamics, or the law of energy conservation, is fundamental in physics and thermodynamics. It asserts that the total energy in an isolated system remains constant. This means energy can neither be created nor destroyed; it can only change forms, such as from kinetic to potentiRead more
The first law of thermodynamics, or the law of energy conservation, is fundamental in physics and thermodynamics. It asserts that the total energy in an isolated system remains constant. This means energy can neither be created nor destroyed; it can only change forms, such as from kinetic to potential energy, or from chemical energy to thermal energy. The principle does not directly address momentum, which is conserved in a different context under Newton’s laws of motion. The conservation of energy applies universally across all processes, ensuring that the total energy before and after any transformation or transfer remains equal. This law underpins much of modern physics and engineering, dictating how energy systems are analyzed and designed. Thus, while momentum conservation is a crucial concept in its own right, it is the conservation of energy that is explicitly protected by the first law of thermodynamics. Therefore, the correct answer is [B] Energy.
See lessSteam burns hands more than boiling water because
Steam burns hands more severely than boiling water due to the latent heat it contains; option [A]. Latent heat is the extra energy required to change water from liquid to vapor without changing its temperature. When steam comes into contact with the skin, it condenses back into liquid water, releasiRead more
Steam burns hands more severely than boiling water due to the latent heat it contains; option [A]. Latent heat is the extra energy required to change water from liquid to vapor without changing its temperature. When steam comes into contact with the skin, it condenses back into liquid water, releasing this stored latent heat. This process transfers a significant amount of energy to the skin, which is much more than what boiling water would transfer at the same temperature. Boiling water only transfers heat at 100°C, but when steam condenses, it releases additional heat as it changes phase from gas to liquid. This results in a higher amount of energy being delivered to the skin, causing more severe burns. Therefore, the presence of latent heat in steam is the primary reason it causes more intense burns than boiling water.
See lessLatent heat of vapor is
The latent heat of vaporization of water is 536 Cal/g, which is the amount of heat needed to convert 1 gram of water at its boiling point (100°C) into steam without any change in temperature. This latent heat is crucial in understanding why steam causes more severe burns than boiling water. When steRead more
The latent heat of vaporization of water is 536 Cal/g, which is the amount of heat needed to convert 1 gram of water at its boiling point (100°C) into steam without any change in temperature. This latent heat is crucial in understanding why steam causes more severe burns than boiling water. When steam condenses on the skin, it releases this latent heat, transferring a substantial amount of energy to the skin. This energy transfer is significantly higher than that of boiling water at the same temperature, leading to more severe burns. Therefore, the correct answer to the latent heat of vaporization of water is [A] 536 Cal/g. This concept is essential in various fields, including thermodynamics and medical treatment of burns, highlighting the importance of understanding the thermal properties of substances.
See less