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How many joules of energy are necessary to heat a sample of water with a mass of 46 g?
Wiki User
∙ 12y ago
46 calories (or 192, 464 joules) for each Celsius degree.
Wiki User
∙ 12y ago
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A sample of H20 with a mass of 46.0 grams has a temperature of 100 c How many joules of energy are necessary to boil the water?
The heat of vaporization is about 2258 joules/gram46 x 2258 = 103,868 J ~ 103.9 kJ(Using the rounded value 2260 joules per gram, about 104 kJ)it is already at boiling point so in theory zero energy is required.I think the question is asking what energy is required to free the water from its liquid state to the vapour state.At 101325Pa, (1 atmosphere in old money), the latent heat of evaporation of water is 2256.7 J/g.So 2256.7 * 46 = 103808 Joules
How much energy is required to heat 955 g of water from 20 degrees C to 100 degrees C?
4.1858 joules of energy will raise the temperature of 1 g of water by 1oC. Thus, 4.1858 * 955 * 80 = 319795.12 joules of energy is required to raise the temperature of 955 g of water by 1oC.
When 418 joules of heat energy are added to 10 grams of water at 20C the final temperature of the water will be?
21
How many joules of energy are necessary to heat a sample of water with a mass of 46.0 grams from 0.0 degrees celsius to 100 degrees celsius?
42 J
How many joules of energy are necessary to heat a sample of water with a mass of 46.0 grams from 0.0 and Atilde and nbspC to 100.0 and Atilde and nbspC?
q = mC∆Twhere q = heat; m = mass; C = neat capacity; ∆T = change in temperatureq = (46.0 g)(4.184 J/g/deg)(100 deg)q = 19.246 J = 19.2 kJ
How many joules of energy are necessary to heat a sample of water with a mass of 46.0 grams for 0.0?
46 calories (or 192, 464 joules) for each Celsius degree.
How many joules of energy are necessary to heat a sample of water with a mass of 46.0 grams from 0.0 celsius to 100.0?
419.1 Joules are required to heat one gram of liquid water from 0.01 degC to 100 deg C. So the answer is 419.1*46 = 19278.6
How many joules are necessary to heat a sample of water with a mass of 46.0 grams from 0.0?
46 calories (or 192, 464 joules) for each Celsius degree.
How much energy is needed to melt 0.25 moles of water?
The necessary heat is 9,22 joules.
A sample of H20 with a mass of 46.0 grams has a temperature of 100 c How many joules of energy are necessary to boil the water?
The heat of vaporization is about 2258 joules/gram46 x 2258 = 103,868 J ~ 103.9 kJ(Using the rounded value 2260 joules per gram, about 104 kJ)it is already at boiling point so in theory zero energy is required.I think the question is asking what energy is required to free the water from its liquid state to the vapour state.At 101325Pa, (1 atmosphere in old money), the latent heat of evaporation of water is 2256.7 J/g.So 2256.7 * 46 = 103808 Joules
How many joules of energy are necessary to heat a sample of water with a mass of 4.60 grams from 0.0 to 100.0?
Assuming no state change:ΔH = mCΔTm = 4.60 gC = 4.184 J/(g * K)ΔT = 100.0 KΔH = 1920 J = 1.92 kJ
How much energy is required to heat 955 g of water from 20 degrees C to 100 degrees C?
4.1858 joules of energy will raise the temperature of 1 g of water by 1oC. Thus, 4.1858 * 955 * 80 = 319795.12 joules of energy is required to raise the temperature of 955 g of water by 1oC.
A sample of h2o with a mass of 46.0 grams has a temperature of 100 c how many joules of energy are necessary to boil the water?
Using 2260 J/g as the ∆Hvaporizationq = 46.0 g x 2260 J/g = 103,960 J = 104 kJ (to 3 sig. figs)
How many joules are needed to melt 2 grams of water?
2,26 Kj are necessary
How many joules of energy are necessary to heat sample of water with a mass of 46.0 grams from 0.0 to 100 C?
Assuming the water is liquid, the specific heat is about 4.186 joule/gram·°C, so to heat 46 grams of water would take about 192.556 joules/°C. The specific heat of ice is about 2.100 Joules/g·°C so heating 46 g of frozen water would take about 96.6 joules/°C. The specific heat of steam is about 2.020 Joules/g·°C so heating 46 g of water vapor would take about 92.2 joules/°C.
When 1 gram of water at 0 degrees Celsius freezes to form ice how many total joules of heat are lost by the water?
It's necessary to remove 540 calories from a gram of water in order to freeze it. That's about 2260 joules. The amount of energy used by a freezer to do this depends on the efficiency of the freezer.
How many watts of energy are in a gallon of salt water?
A watt is a unit of power (Joules/second: energy / time). I guess it depends on what method you are using to get energy out of the water, as to how much energy is in it.
