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How many calories of heat is available when a hot water bottle containing 750g of water at 65 degrees cools to body temperature?
To calculate the calories of heat available when the water cools to body temperature, you need to consider the specific heat capacity of water. The specific heat capacity of water is 4.18 J/g°C. By using the formula Q = mcΔT, where Q is the heat energy, m is the mass, c is the specific heat capacity, and ΔT is the temperature change, you can find the answer.
Calculate the amount of heat released when 50 g of steam at 100 celsius hits the skin condenses and cools to a body temperature of 37 celsius?
water's specific heat is 1 calorie/mL/degree celsius. if you assume the density is 1 g/mL then we have 50 mL of material going from 100 to 37 degrees C. So take Mass X Change in Temp X Specific heat and that is your answer.
How many calories are needed to vaporize 1 gram of boiling water at 100 degrees?
To vaporize 1 gram of boiling water at 100 degrees Celsius, it would require approximately 2260 joules, which is equivalent to about 0.54 calories. This energy is needed to break the intermolecular bonds holding water molecules together, allowing them to escape into the gas phase.
What happens to a sample of water vapor at 101 and degree's Celsius as it cools?
As the water vapor cools at 101 degrees Celsius, it will undergo a phase change and condense into liquid water. This is because the cooling causes the water vapor to lose energy and come together to form liquid droplets.
Water decreases in volume when its temperature drops from 38 to 32 F. is this true or false?
False. Water expands when it cools from 38 to 32 degrees Fahrenheit. However, it contracts as it freezes below 32 degrees Fahrenheit.
How many calories are released during the process of condensation?
To transform 1 gram of ice at 0 degrees Celsius to 1 gram of water vapor at 100 degrees Celsius, 720 calories are added (absorbed). There are no calories released during the process.
How much heat is released when 250 g of water at 10 degrees Celsius freezes into ice and cools to -10 degrees Celsius?
250g of water at 10C needs to lose 1 cal/g/C or 2500 calories to drop temperature to zero. The latent heat of fusion of water is 80 calories per gram at 0C so, the water needs to lose 20,000 calories to turn to ice at 0C Finally, the ice needs to lose 0.316 cal/g/C or 790 calories to drop to -10C The total heat released is then 2500 + 20,000 + 790 = 23,290 calories
Does water that cools from 4 degrees celsius to 0 degrees celsius remain the same in density?
No, water's density decreases as it cools. Water reaches its maximum density at around 4 degrees Celsius, and as it cools further, the water molecules form a crystalline structure, causing the density to decrease.
How many calories of heat is available when a hot water bottle containing 750g of water at 65 degrees cools to body temperature?
To calculate the calories of heat available when the water cools to body temperature, you need to consider the specific heat capacity of water. The specific heat capacity of water is 4.18 J/g°C. By using the formula Q = mcΔT, where Q is the heat energy, m is the mass, c is the specific heat capacity, and ΔT is the temperature change, you can find the answer.
How many calories does it take to heat a 100.0 g sample of water from 24.5 degrees to 38.2 degrees?
1370 calories
How many SI calories does it take to raise one liter if water 6 degrees Celsius?
It takes 6 SI calories to raise one liter of water by 6 degrees Celsius.
How many joules released when 10 g of steam at 110 degrees cools to produce water at -5?
To calculate the energy released when the steam cools to water, you need to consider the specific heat capacity of water and steam. The equation Q = mcΔT can be used, where Q is the energy released, m is the mass, c is the specific heat capacity, and ΔT is the change in temperature. Once you have the energy released, you can convert it to joules.
How many calories are released when1g of 100degees water cool to 0 degrees?
Ittakes 1 calorie for every degree C change of 1 gram of water answer: 100
How many calories to heat 10 ml of water from 25 degrees to 35 degrees C?
100
Water is said to be when it cools below 0 degrees C without freezing?
super-cooled
Calculate the amount of heat released when 50 g of steam at 100 celsius hits the skin condenses and cools to a body temperature of 37 celsius?
water's specific heat is 1 calorie/mL/degree celsius. if you assume the density is 1 g/mL then we have 50 mL of material going from 100 to 37 degrees C. So take Mass X Change in Temp X Specific heat and that is your answer.
How many calories of heat would it take to raise the temperature of 256 grams of water from 20 degrees to 99 degrees?
A calorie is the amount of heat you need to raise the temperature of one gram of water by one degree Celsius. Assuming you are raising the temperature of the water from twenty degrees Celsius to ninety-nine degrees Celsius, it would take 20,000 calories. To calculate this, subtract 20 from 99. This is the amount of degrees you need to raise the temperature of the water by. Then multiply that number by 256, the amount of water in grams. You should get 20,244 calories. In significant digits, your answer should be 20,000 calories.
