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How much heat in joules to heat a 40 g sample of aluminum from 73 degrees f to 142 degrees f?
Wiki User
∙ 11y ago
q( in Joules ) = mass * specific heat * change in temperature [ convert temps--Tf = Tc(1.80) + 32 ]
q = (40 g)(0.90 J/gC)(61.1o C - 22.8o C)
= 1.4 X 103 Joules
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Wiki User
∙ 11y ago
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How many joules of energy are required to raise the temperature of 20g of aluminum from 10 degrees C to 15 degrees C?
Heat energy Q = mass x specific heat capacity x temperature change. Q = m*c*delta T Q = Joules m = kg c (aluminum) = 895.8 J/kg delta T = degr.C temp. change Answer: Q = (20/1000) x 895.8 x 5 = 89.58 Joules (Specific heat capacity of aluminum is obtained by multiplying its specific heat of 0.214 with c of water which is 4186 J/kg = 0.214 x 4186 = 895.8 J/kg).
How much heat is released when 12.4 g of steam at 100 degrees celsius condenses to water at 100 degrees celsius?
The latent heat of condensation of steam is 2260 Joules per gram (539.3 cals/g). So the amount of heat released by 12.4 g = 12.4*2260 Joules = 28,024 Joules or 6687 cals.
Is temp or heat measured in degrees?
If you want to be pedantic, scientists measure temperature in kelvins, not degrees. Heat is energy and is measured in energy units, like joules.
How many joules are absorbed by the water with a mass of 8 kg in order to raise the temperature from 20 degrees to 70 degrees?
q(joules) = mass * specific heat * change in temperature ( 8 kg = 8000 grams ) q = (8000 grams H2O)(4.180 J/gC)(70o C - 20o C) = 1.7 X 106 joules ============
How many calories are required to heat 38.2 grams of aluminum from 102 degrees celsius to 275 degrees celsius?
Specific heat for aluminium = 0.214 Heat required = 38.2 x 0.214 x (275 - 102) = 1414.24 calories
What is the total heat loss if you have 18 grams of aluminum and the temperature changes from 64 degrees Celsius to 48 degrees Celsius?
Approx 4974 Joules.
How much heat energy is needed to raise the temperature of a 055kg sample of aluminum from 22.4 degrees celsius to 94.6 degrees celsius?
mmmm enthalpy
Is heat energy measured in units of joules degrees Celsius and in degrees Fahrenheit?
Heat is measured in unit of what...
How many joules of energy are required to raise the temperature of 20g of aluminum from 10 degrees C to 15 degrees C?
Heat energy Q = mass x specific heat capacity x temperature change. Q = m*c*delta T Q = Joules m = kg c (aluminum) = 895.8 J/kg delta T = degr.C temp. change Answer: Q = (20/1000) x 895.8 x 5 = 89.58 Joules (Specific heat capacity of aluminum is obtained by multiplying its specific heat of 0.214 with c of water which is 4186 J/kg = 0.214 x 4186 = 895.8 J/kg).
How much eat in calories is required to heat a 43 g sample of aluminum from 72 F to 145F?
How much heat (in calories) is required to heat a 43 g sample of aluminum from 72 F to 145F
How many joules does it take to heat up 15.1kg of glass to 15 degrees Celsius to 45 degrees Celsius?
3.8 x 10^5 Joules
A particular sample of iron requires 562 Joules to raise its temperature from 25 degreee Celsius to 50 degrees Celsius. What must be the mass of the sample of iron?
The change in temperature is 25 degrees Celsius, meaning it takes 22.48 joules per degree of change. The specific heat of iron is 0.449 J/g degree Celsius. This means that the mass of iron must be 50.07 grams
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 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.
Is heat is measured in degrees Celsius?
Temperature is measured in celcius.Heat is measured in joules.
How much heat is released when 12.4 g of steam at 100 degrees celsius condenses to water at 100 degrees celsius?
The latent heat of condensation of steam is 2260 Joules per gram (539.3 cals/g). So the amount of heat released by 12.4 g = 12.4*2260 Joules = 28,024 Joules or 6687 cals.
