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∙ 9y agoTo calculate the heat given off, you would use the formula Q = mcΔT, where m is the mass of the water (10 g), c is the specific heat capacity of water (4.18 J/g°C), and ΔT is the change in temperature (50°C - 40°C = 10°C). Plugging the values into the formula, Q = 10g * 4.18 J/g°C * 10°C = 418 J. Therefore, 418 joules of heat are given off when 10 grams of water are cooled from 50°C to 40°C.
When water vapor is cooled to its dew point, the heat energy is released as latent heat, causing the water vapor to condense into liquid water. This latent heat is the energy required for the phase change from gas to liquid, and is released back into the surrounding environment during condensation.
The specific heat of water is 4.18 J/g°C. To melt water from solid to liquid, it requires 334 J/g. Given 4500 J of heat, divide it by the heat of fusion to find the mass: 4500 J / 334 J/g = 13.47 grams of water.
To calculate the grams of ice formed from 100 grams of steam, we need to consider the heat exchange involved in the phase changes. First, the steam needs to lose heat to condense into water, then cool further to freeze into ice. Given the specific heat capacities and enthalpies of fusion/vaporization of water, you can determine the final mass of ice formed.
Water vapor becomes liquid water when it is cooled. This process is known as condensation, where the vapor loses heat and transforms from a gaseous state to a liquid state.
To solve this problem, you can use the principle of conservation of energy: Heat gained by the metal = heat lost by the metal + heat gained by the water Plug in the given values and use the specific heat capacity of metal and water to calculate the initial temperature of the metal before mixing.
Air cooled, water cooled and ground cooled
Heat can be deposited in the cooling water flowing through the condenser tubes and in the surrounding environment through air or another medium used for cooling.
The idea here is to: * Look up the specific heat of water. * Multiply the mass, times the temperature difference, times the specific heat of water. You may need to do some unit conversions first; specifically, if the specific heat is given per kilogram, you can convert the grams to kilograms.
The amount of heat released can be calculated using the formula: Q = mcΔT, where Q is the heat released, m is the mass (50g), c is the specific heat (4.2 J/g°C for water), and ΔT is the change in temperature (50°C - 10°C). Substituting the values, we get Q = 50g * 4.2 J/g°C * (50°C - 10°C) = 8400 J (or 8.4 kJ) of heat released.
The heat gets removed from the H2O
Heat moves from the water to its surroundings when water is cooled below 0 degrees Celsius. This causes the temperature of the water to decrease further until it reaches its freezing point, at which point it will freeze into ice.
When water vapor is cooled to its dew point, the heat energy is released as latent heat, causing the water vapor to condense into liquid water. This latent heat is the energy required for the phase change from gas to liquid, and is released back into the surrounding environment during condensation.
The specific heat of water is 4.18 J/g°C. To melt water from solid to liquid, it requires 334 J/g. Given 4500 J of heat, divide it by the heat of fusion to find the mass: 4500 J / 334 J/g = 13.47 grams of water.
Water-cooled condensers typically have lower head pressure compared to air-cooled condensers. Water-cooled systems are more efficient in transferring heat, resulting in lower operating pressures and temperatures. This can help in reducing energy consumption and improving overall system performance.
To calculate the grams of ice formed from 100 grams of steam, we need to consider the heat exchange involved in the phase changes. First, the steam needs to lose heat to condense into water, then cool further to freeze into ice. Given the specific heat capacities and enthalpies of fusion/vaporization of water, you can determine the final mass of ice formed.
Perspiration coats the outside of the skin with moisture (water). The water evaporates. Evaporation requires heat to be absorbed by the water (the latent heat of vaporization). Heat is removed from the body surface to provide the water with the latent heat of vaporization.
Water vapor becomes liquid water when it is cooled. This process is known as condensation, where the vapor loses heat and transforms from a gaseous state to a liquid state.