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How much heat is needed to vaporize 7.24 ml of sweat from your skin at twenty five degrees Celsius?
To calculate the heat needed to vaporize sweat, you would need to know the specific heat of vaporization of sweat. Once you have that information, you can use the formula Q = mL, where Q is the heat needed, m is the mass of the substance (converted from volume using its density), and L is the specific heat of vaporization.
How much energy is required to vaporize 1.5 of aluminum?
1650kj
How much heat is necessary to vaporize 500 grams of ice at its freezing point?
The heat required to vaporize 500 grams of ice at its freezing point is the sum of the heat required to raise the temperature of the ice to its melting point, the heat of fusion to melt the ice, the heat required to raise the temperature of water to its boiling point, and finally the heat of vaporization to vaporize the water. The specific heat capacity of ice, heat of fusion of ice, specific heat capacity of water, and heat of vaporization of water are all needed to perform the calculations.
How much energy is needed to vaporize 2 kg of gold?
The energy required to vaporize a material can be calculated using its heat of vaporization. For gold, the heat of vaporization is approximately 330 kJ/mol. Since gold has a molar mass of 196.97 g/mol, 2 kg of gold is equal to 10.15 moles. Therefore, the energy needed to vaporize 2 kg of gold is approximately 3.35 MJ.
How do you obtain ethanol from gasohol?
Ethanol is typically obtained from gasohol by a distillation process that separates the ethanol from the other components in the mixture. This process involves heating the gasohol to vaporize the ethanol, which is then condensed back into a liquid form. The resulting ethanol can then be further purified if needed.
How much heat is needed to boil alcohol?
The amount of heat required to boil alcohol (ethanol) depends on the quantity being heated and its initial temperature. On average, it takes about 207.3 kJ of heat to vaporize 1 mole of ethanol.
How much heat energy is needed to vaporize g of water at its boiling point of K?
1oo calories for 1 g
How much heat is needed to vaporize 7.24 ml of sweat from your skin at twenty five degrees Celsius?
To calculate the heat needed to vaporize sweat, you would need to know the specific heat of vaporization of sweat. Once you have that information, you can use the formula Q = mL, where Q is the heat needed, m is the mass of the substance (converted from volume using its density), and L is the specific heat of vaporization.
How much energy is required to vaporize 1.5 of aluminum?
1650kj
How much heat is necessary to vaporize 500 grams of ice at its freezing point?
The heat required to vaporize 500 grams of ice at its freezing point is the sum of the heat required to raise the temperature of the ice to its melting point, the heat of fusion to melt the ice, the heat required to raise the temperature of water to its boiling point, and finally the heat of vaporization to vaporize the water. The specific heat capacity of ice, heat of fusion of ice, specific heat capacity of water, and heat of vaporization of water are all needed to perform the calculations.
How much energy is needed to vaporize 2 kg of gold?
The energy required to vaporize a material can be calculated using its heat of vaporization. For gold, the heat of vaporization is approximately 330 kJ/mol. Since gold has a molar mass of 196.97 g/mol, 2 kg of gold is equal to 10.15 moles. Therefore, the energy needed to vaporize 2 kg of gold is approximately 3.35 MJ.
How do you obtain ethanol from gasohol?
Ethanol is typically obtained from gasohol by a distillation process that separates the ethanol from the other components in the mixture. This process involves heating the gasohol to vaporize the ethanol, which is then condensed back into a liquid form. The resulting ethanol can then be further purified if needed.
How much heat is absorbed for 1 kg of liquid gets vapourised into boiling point?
The amount of heat absorbed by 1 kg of liquid to vaporize it depends on what that liquid is, (water?), and what the temperature of the liquid is at the start of the process. Obviously, it will take more heat to vaporize 1 kg of liquid that is at 0º than it will to vaporize 1 kg of liquid that is at, say, 30º.
How much heat is needed to vaporize 100g of water at 100 degrees C?
Heat of vaporization at 100 degrees C is 40.65 kJ/mol. 100g water * 1mol/18.015g = 5.55 mol 40.65*5.55 = 225.6452956 = 226 kJ if three sig figs.
How much energy is released when 1.56 kg of ethanol 46.0 g mol freezes The heat of fusion of ethanol is 4.94 kJ mol?
To calculate the energy released when 1.56 kg of ethanol freezes, first convert the mass of ethanol to moles using its molar mass. Then, use the heat of fusion of ethanol to determine the energy released using the formula: Energy released = moles of ethanol x heat of fusion.
Most methods of large scale desalinization are not cost effective because?
too much energy is needed to vaporize water
If 20.6 grams of ice at -35c are heated and vaporized to all gas at 110c how much energy is required?
To calculate the energy required to heat and vaporize the ice, you need to consider the heat needed for each step: Heat the ice from -35°C to 0°C (specific heat of ice). Melt the ice at 0°C (heat of fusion). Heat the water at 0°C to 100°C (specific heat of water). Vaporize the water at 100°C (heat of vaporization). Heat the steam from 100°C to 110°C (specific heat of steam). Adding all these energies together will give you the total energy required.
