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With increase of pressure, the latent heat of steam
- a)Remains same
- b)Increases
- c)Decreases
- d)Behaves unpredictably
Correct answer is option 'C'. Can you explain this answer?
Verified Answer
With increase of pressure, the latent heat of steam a)Remains sameb)In...
Prresure increases at 100 degree latent heat of vapourisation also increases while as pressure increases latent heat of condensation decreases. When temperature of the water in the beaker increases, the bond b/w molecules releases and water starts vaporizing.
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With increase of pressure, the latent heat of steam a)Remains sameb)In...
Effect of Pressure on the Latent Heat of Steam
Introduction:
The latent heat of steam refers to the amount of heat energy required to change a unit mass of water at its boiling point into steam without changing its temperature. It is a property that depends on the phase change from liquid to gas. The latent heat of steam is commonly used in various industrial and engineering applications, such as power generation, heating, and cooling systems.
Explanation:
Increase in Pressure:
When the pressure on the steam increases, it has a significant impact on its latent heat. The latent heat of steam decreases with an increase in pressure. This can be attributed to the fact that as pressure increases, the boiling point of water also increases. As a result, the difference between the boiling point and the temperature at which steam condenses decreases.
Intermolecular Forces:
The latent heat of vaporization, which is the heat required to convert a liquid into a gas, is influenced by the intermolecular forces between the molecules of the substance. In the case of water, hydrogen bonding plays a crucial role. As pressure increases, the intermolecular forces between water molecules become stronger due to the reduced spacing between them. This leads to a decrease in the energy required to break these intermolecular forces and convert water into steam.
Boiling Point Elevation:
The boiling point of water increases with an increase in pressure. This occurs because at higher pressures, the external pressure must be overcome by the vapor pressure of the liquid in order for it to boil. As a result, more heat energy is required to reach the increased boiling point, leading to a decrease in the latent heat of steam.
Conclusion:
In summary, the latent heat of steam decreases with an increase in pressure. This is due to the increased intermolecular forces between water molecules at higher pressures and the corresponding elevation in the boiling point of water. It is important to consider these effects when designing and operating systems that involve the use of steam, as they can impact the efficiency and performance of such systems.
Introduction:
The latent heat of steam refers to the amount of heat energy required to change a unit mass of water at its boiling point into steam without changing its temperature. It is a property that depends on the phase change from liquid to gas. The latent heat of steam is commonly used in various industrial and engineering applications, such as power generation, heating, and cooling systems.
Explanation:
Increase in Pressure:
When the pressure on the steam increases, it has a significant impact on its latent heat. The latent heat of steam decreases with an increase in pressure. This can be attributed to the fact that as pressure increases, the boiling point of water also increases. As a result, the difference between the boiling point and the temperature at which steam condenses decreases.
Intermolecular Forces:
The latent heat of vaporization, which is the heat required to convert a liquid into a gas, is influenced by the intermolecular forces between the molecules of the substance. In the case of water, hydrogen bonding plays a crucial role. As pressure increases, the intermolecular forces between water molecules become stronger due to the reduced spacing between them. This leads to a decrease in the energy required to break these intermolecular forces and convert water into steam.
Boiling Point Elevation:
The boiling point of water increases with an increase in pressure. This occurs because at higher pressures, the external pressure must be overcome by the vapor pressure of the liquid in order for it to boil. As a result, more heat energy is required to reach the increased boiling point, leading to a decrease in the latent heat of steam.
Conclusion:
In summary, the latent heat of steam decreases with an increase in pressure. This is due to the increased intermolecular forces between water molecules at higher pressures and the corresponding elevation in the boiling point of water. It is important to consider these effects when designing and operating systems that involve the use of steam, as they can impact the efficiency and performance of such systems.
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Community Answer
With increase of pressure, the latent heat of steam a)Remains sameb)In...
The latent heat of steam decreases with an increase in pressure.
Explanation:
1. Latent Heat of Steam:
The latent heat of steam refers to the amount of heat energy required to convert one unit mass of water at its boiling point into steam at the same temperature and pressure. It is a measure of the energy absorbed or released during the phase change.
2. Effect of Pressure on Latent Heat:
When pressure increases, the boiling point of water also increases. This means that water requires a higher temperature to boil and convert into steam. As a result, the latent heat of steam decreases.
3. Relationship between Pressure and Boiling Point:
Pressure and boiling point are directly related. At higher pressures, the boiling point of water increases, and at lower pressures, the boiling point decreases. This relationship is explained by the Clausius-Clapeyron equation.
The Clausius-Clapeyron equation states that the natural logarithm of the vapor pressure of a substance is inversely proportional to its boiling point temperature. Mathematically, it can be represented as:
ln(P2/P1) = ΔHvap/R * (1/T1 - 1/T2)
Where P1 and P2 are the initial and final pressures, T1 and T2 are the initial and final temperatures (boiling points), ΔHvap is the enthalpy of vaporization, and R is the gas constant.
4. Decrease in Latent Heat with Increasing Pressure:
As the pressure increases, the boiling point of water increases. According to the Clausius-Clapeyron equation, if the boiling point temperature increases, the natural logarithm of the vapor pressure also increases. This implies that the enthalpy of vaporization (latent heat) decreases.
The decrease in latent heat can be understood by considering the energy balance during the phase change. At higher pressures, the water molecules are held more tightly due to increased intermolecular forces. Therefore, less energy is required to break these forces and convert water into steam. Consequently, the latent heat decreases.
Conclusion:
In summary, the latent heat of steam decreases with an increase in pressure. This is due to the relationship between pressure and boiling point, as explained by the Clausius-Clapeyron equation. As pressure increases, the boiling point of water increases, leading to a decrease in the enthalpy of vaporization (latent heat).
Explanation:
1. Latent Heat of Steam:
The latent heat of steam refers to the amount of heat energy required to convert one unit mass of water at its boiling point into steam at the same temperature and pressure. It is a measure of the energy absorbed or released during the phase change.
2. Effect of Pressure on Latent Heat:
When pressure increases, the boiling point of water also increases. This means that water requires a higher temperature to boil and convert into steam. As a result, the latent heat of steam decreases.
3. Relationship between Pressure and Boiling Point:
Pressure and boiling point are directly related. At higher pressures, the boiling point of water increases, and at lower pressures, the boiling point decreases. This relationship is explained by the Clausius-Clapeyron equation.
The Clausius-Clapeyron equation states that the natural logarithm of the vapor pressure of a substance is inversely proportional to its boiling point temperature. Mathematically, it can be represented as:
ln(P2/P1) = ΔHvap/R * (1/T1 - 1/T2)
Where P1 and P2 are the initial and final pressures, T1 and T2 are the initial and final temperatures (boiling points), ΔHvap is the enthalpy of vaporization, and R is the gas constant.
4. Decrease in Latent Heat with Increasing Pressure:
As the pressure increases, the boiling point of water increases. According to the Clausius-Clapeyron equation, if the boiling point temperature increases, the natural logarithm of the vapor pressure also increases. This implies that the enthalpy of vaporization (latent heat) decreases.
The decrease in latent heat can be understood by considering the energy balance during the phase change. At higher pressures, the water molecules are held more tightly due to increased intermolecular forces. Therefore, less energy is required to break these forces and convert water into steam. Consequently, the latent heat decreases.
Conclusion:
In summary, the latent heat of steam decreases with an increase in pressure. This is due to the relationship between pressure and boiling point, as explained by the Clausius-Clapeyron equation. As pressure increases, the boiling point of water increases, leading to a decrease in the enthalpy of vaporization (latent heat).
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