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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?
Wiki User
∙ 13y ago
42 J
Wiki User
∙ 7y ago
Wiki User
∙ 13y agoUse this formula.
q(in Joules) = mass * specific heat of water * change in temp.(final - initial )
q = nCT
q = (46.0 grams)(4.180 J/gC)(100 C - 0 C)
= 19228 Joules
correct for significant figures
Wiki User
∙ 11y agoQ = mCΔt, where Q is energy added or lost in Joules, m is mass in grams, C is specific heat, Δtis change in temperature in oC.
m = 2.0g
Δt = 5.0 oC
CH2O = 4.186 Joules/gram oC
Q = 2.0g x 4.180J/g•oC x 5.0 oC = 42 Joules (rounded to two significant figures)
Wiki User
∙ 10y agoFor each Celsius degree of heating, you must add 4.184 joules per gram,
or 192.4 joules for the 46 gram sample.
Wiki User
∙ 12y ago1 calories (or 4,184 joule) for 1 g and for each Celsius degree.
Wiki User
∙ 12y agoQ (heat) = mass*Cp*Temp. Change (where Cp is specific heat)
Q = 5.0 grams * 4.18 J/goC * (30-20oC)
=5*4.18*10 = 209 J
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How many joules of energy are necessary to heat a sample of water with a mass of 46 g?
46 calories (or 192, 464 joules) for each Celsius degree.
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Heat is measured in unit of what...
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How many joules of energy are necessary to heat a sample of water with a mass of 46 g?
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 for 0.0?
46 calories (or 192, 464 joules) for each Celsius degree.
Does it it take more energy to heat the water to 100 degrees celsius or boil it?
If by "boil" you mean have it all evaporate, that takes MUCH more energy. For example, to increase the temperature of one gram of water from 20 to 100 degrees Celsius, you need 4.2 joules/gram/degree times 80 degrees = about 336 joules; then, to evaporate all the water, you need an additional 2257 joules.
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How much heat in joules is required to convert 92g of ice at 0.00 degrees Celsius to water vapor at 148 degrees Celsius?
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