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How much heat is needed to vaporize 7.24 ml of sweat from your skin at 25 degree c?
If you assume that the density of sweat is the same as that of water (1g/ml) and that the specific heat of sweat is the same as that of water (4.184 J/g/deg), then one can estimate the heat required to evaporate 7.24 ml of sweat at 25 degrees Cheat to raise 7.24 ml from 25º to 100º = q = mC∆T = (7.24g)(4.184 J/g/deg)(75deg) = 2272 J
heat to evaporate 7.24 ml = q = m∆Hvap = (7.24g)(2260 J/g) = 16,362 J
Total heat = 2272 J + 16,362 J = 18,634 J = 18.6 kJ
What else can I help you with?
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 heat is needed to vaporize 7.24 ml of sweat from your skin at twenty five degrees Celsius Assume sweat is only water. Density 0.9970 g ml twenty five degrees Celsius.?
The first step is to determine the mass of 7.24 ml of sweat by using its density of 0.9970 g/ml. The mass can be calculated as 7.24 ml * 0.9970 g/ml = 7.22 g. Next, we can use the heat of vaporization of water, which is 2260 J/g, to find the total heat required. Therefore, the amount of heat needed to vaporize 7.24 ml of sweat would be 7.22 g * 2260 J/g = 16367.2 J.
How many joules of heat are needed to completely vaporize 24.40 grams of water at its boiling point?
The heat of vaporization of water is 40.79 kJ/mol. First, determine the number of moles in 24.40 grams of water. Then, convert moles to joules using the molar heat of vaporization. This will give you the amount of heat needed to vaporize 24.40 grams of water.
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 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.
Why cotton clothes are soothing in summer?
cotton allows sweat to vaporize and it absorbs heat.
How much heat is needed to vaporize 7.24 ml of sweat from your skin at twenty five degrees Celsius Assume sweat is only water. Density 0.9970 g ml twenty five degrees Celsius.?
The first step is to determine the mass of 7.24 ml of sweat by using its density of 0.9970 g/ml. The mass can be calculated as 7.24 ml * 0.9970 g/ml = 7.22 g. Next, we can use the heat of vaporization of water, which is 2260 J/g, to find the total heat required. Therefore, the amount of heat needed to vaporize 7.24 ml of sweat would be 7.22 g * 2260 J/g = 16367.2 J.
Why the time needed to vaporize a sample is greater than the time needed to melt a sample?
The amount of time depends on the latent heat of vaporisation and the latent heat of melting.
How many joules of heat are needed to completely vaporize 24.40 grams of water at its boiling point?
The heat of vaporization of water is 40.79 kJ/mol. First, determine the number of moles in 24.40 grams of water. Then, convert moles to joules using the molar heat of vaporization. This will give you the amount of heat needed to vaporize 24.40 grams of water.
Why is more heat needed to vaporize water than gasoline?
Gasoline has a less boiling point (72 degree Celsius) While water has a bigger boiling point (100 degree Celsius)
How much energy is required to vaporize 1.5 of aluminum?
1650kj
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 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.
What is the amount of energy needed to vaporize one gram of a liquid?
The amount of energy needed to vaporize one gram of a liquid is known as the heat of vaporization. It varies for different substances and can be calculated using the formula Q = m * Hv, where Q is the energy required, m is the mass of the substance (in this case, 1 gram), and Hv is the heat of vaporization of the specific substance.
What happens to the human body if you are running in 85 degree Fahrenheit weather?
you sweat to stay cool. The heat of the sun is used to turn your sweat to water vapor, rather than to heat up your body.
How much heat is needed to vaporize 1.25 kg of ethanol?
The heat of vaporization of ethanol is approximately 840 kJ/kg. To find the total heat required to vaporize 1.25 kg of ethanol, you can multiply the mass by the heat of vaporization: 1.25 kg * 840 kJ/kg = 1050 kJ.
