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.
The latent heat of melting of ice is 80 Cal/g. This is the amount of heat required to convert 1 gram of ice at 0°C into liquid water at the same temperature, without any temperature change. This energy is necessary to overcome the molecular forces holding the ice crystals together. Understanding theRead more
The latent heat of melting of ice is 80 Cal/g. This is the amount of heat required to convert 1 gram of ice at 0°C into liquid water at the same temperature, without any temperature change. This energy is necessary to overcome the molecular forces holding the ice crystals together. Understanding the latent heat of melting is crucial in various scientific and engineering applications, such as climate studies, refrigeration, and the design of thermal energy storage systems. It explains why ice takes a significant amount of time and energy to melt compared to heating water by a similar amount. Therefore, the correct answer to the value of the latent heat of melting of ice is [C] 80 Cal/g. This fundamental concept is key to numerous processes involving phase changes and energy calculations in thermodynamics.
The heat required to change a unit mass of a solid substance from solid to liquid at its melting point is referred to as the latent heat of melting of solid. This specific amount of energy is needed to overcome the intermolecular forces holding the solid structure together, allowing the solid to traRead more
The heat required to change a unit mass of a solid substance from solid to liquid at its melting point is referred to as the latent heat of melting of solid. This specific amount of energy is needed to overcome the intermolecular forces holding the solid structure together, allowing the solid to transition into a liquid state without any change in temperature. Understanding this concept is vital in fields such as material science, thermodynamics, and various engineering applications. For instance, when ice melts to form water at 0°C, the energy input used to achieve this phase change without increasing the temperature is the latent heat of melting. Therefore, the correct answer is [C] Latent heat of melting of solid. This principle is essential for accurately calculating energy requirements in processes involving phase changes.
The emitted or absorbed heat which changes the state of the substance without causing any change in temperature is known as latent heat. This energy is crucial for phase transitions, such as melting, freezing, boiling, or condensation. During these processes, the temperature of the substance remainsRead more
The emitted or absorbed heat which changes the state of the substance without causing any change in temperature is known as latent heat. This energy is crucial for phase transitions, such as melting, freezing, boiling, or condensation. During these processes, the temperature of the substance remains constant while the latent heat either breaks or forms the molecular bonds necessary for the phase change. For example, when ice melts into water or water boils into steam, the temperature remains stable at the melting or boiling point, respectively, despite continuous heat input. This absorbed or released energy, termed latent heat, is fundamental in understanding various natural and industrial processes involving phase changes. Therefore, the correct answer is [D] Latent heat. This concept is pivotal in fields such as meteorology, refrigeration, and thermal management systems.
Steam 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 lessThe value of latent heat of melting of ice is
The latent heat of melting of ice is 80 Cal/g. This is the amount of heat required to convert 1 gram of ice at 0°C into liquid water at the same temperature, without any temperature change. This energy is necessary to overcome the molecular forces holding the ice crystals together. Understanding theRead more
The latent heat of melting of ice is 80 Cal/g. This is the amount of heat required to convert 1 gram of ice at 0°C into liquid water at the same temperature, without any temperature change. This energy is necessary to overcome the molecular forces holding the ice crystals together. Understanding the latent heat of melting is crucial in various scientific and engineering applications, such as climate studies, refrigeration, and the design of thermal energy storage systems. It explains why ice takes a significant amount of time and energy to melt compared to heating water by a similar amount. Therefore, the correct answer to the value of the latent heat of melting of ice is [C] 80 Cal/g. This fundamental concept is key to numerous processes involving phase changes and energy calculations in thermodynamics.
See lessThe heat required to change a unit mass of a solid substance from solid to liquid at its melting point is called
The heat required to change a unit mass of a solid substance from solid to liquid at its melting point is referred to as the latent heat of melting of solid. This specific amount of energy is needed to overcome the intermolecular forces holding the solid structure together, allowing the solid to traRead more
The heat required to change a unit mass of a solid substance from solid to liquid at its melting point is referred to as the latent heat of melting of solid. This specific amount of energy is needed to overcome the intermolecular forces holding the solid structure together, allowing the solid to transition into a liquid state without any change in temperature. Understanding this concept is vital in fields such as material science, thermodynamics, and various engineering applications. For instance, when ice melts to form water at 0°C, the energy input used to achieve this phase change without increasing the temperature is the latent heat of melting. Therefore, the correct answer is [C] Latent heat of melting of solid. This principle is essential for accurately calculating energy requirements in processes involving phase changes.
See lessThe emitted or absorbed heat which changes the state of the substance, but does not cause any change in temperature, is called
The emitted or absorbed heat which changes the state of the substance without causing any change in temperature is known as latent heat. This energy is crucial for phase transitions, such as melting, freezing, boiling, or condensation. During these processes, the temperature of the substance remainsRead more
The emitted or absorbed heat which changes the state of the substance without causing any change in temperature is known as latent heat. This energy is crucial for phase transitions, such as melting, freezing, boiling, or condensation. During these processes, the temperature of the substance remains constant while the latent heat either breaks or forms the molecular bonds necessary for the phase change. For example, when ice melts into water or water boils into steam, the temperature remains stable at the melting or boiling point, respectively, despite continuous heat input. This absorbed or released energy, termed latent heat, is fundamental in understanding various natural and industrial processes involving phase changes. Therefore, the correct answer is [D] Latent heat. This concept is pivotal in fields such as meteorology, refrigeration, and thermal management systems.
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