The specific heat capacity of water is 4186 joules per kilogram. That is to raise 1kg or 1 litre of water by 1 degree you will need to add 4186 joules of energy. So for 15grams over 25 degrees you will need 4186/1000*15*15 joules.
The amount of heat required to heat a given mass of water by 1 deg C is not a constant but depends on the temperature range. The average amount for heating 1 gram of air-free water, at standard atmospheric pressure (101.325 kPa), known as the Mean Calorie, is 4.190 Joules.
So in this example the amount of heat required is 300*60*4.190 =75420 Joules = 75.42 kiloJoules.
q = heat energy gained or lost
C = specific heat in Joules/gram °C
DT = change in temperature
CH2O = 4.186 Joules/gram °C
q = CH2O x m x DT = 4.186 Joules/gram °C x 15g x 25°C = 1569.75 Joules or 1600 Joules with 2 significant figures.
q = m x C x ΔT
q = amount of heat energy gained or lost by substance in Joules
m = mass of sample in grams = 150.0g
C = heat capacity (J/goC) = 4.18 J/goC
Tf = final temperature = 45.0 oC
Ti = initial temperature = 15.0 oC
ΔT = (Tf - Ti) = 30.0 oC
q = 150.0g x 4.18J/goC x 30.0 oC = 18810 Joules
The energy required to raise the temperature is 1570 joules.
1570 joules
375 calories
3142.5 Joules.
The amount of water whose temperature would change by 15 degrees Celsius when it absorbs 2646 joules of heat energy is 42,2g H2O.
4.184 J/g/K = 4.184 x 150 x (318-274) = 27614 Joules
Energy due to temperature is called thermal energy and is measured in Calories or BTU. Kinetic energy is that due to motion of a body and is measured in Joules. There is an equivalence between thermal and mechanical energy, 1 Calorie = 4.2 Joules, 1 BTU = 1055 Joules
You cannot convert Joules to Fahrenheit. They are two different kinds of measurements. Fahrenheit measures temperature and Joules measures energy.
1.3 kg water = 1300 grams. q(Joules-heat energy) = mass * specific heat * change in temperature q = (1300 g)(4.180 J/gC)(100 C - 20 C) = 4.3 X 105 Joules of heat energy ========================
15480.80
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.
The amount of water whose temperature would change by 15 degrees Celsius when it absorbs 2646 joules of heat energy is 42,2g H2O.
If you want to be pedantic, scientists measure temperature in kelvins, not degrees. Heat is energy and is measured in energy units, like joules.
21 Kg = 2100 grams to rise the temperature of this amount of water by 2 degrees Celsius you need 2*2100 = 4200 calories or 17572.8 Joules.
15.37684 joules
Q = 3 000 . 0,444 . ΔT (joules)ΔT is the difference of temperature.
It is 15188 Joules.
Temperature is measured in kelvin, although degrees Celsius are commonly used. Heat is a form of energy, and is measured in joules.
No, Fahrenheit is the Imperial Unit for temperature, not heat. Heat is energy in transit and is measured in joules (in the SI sytem).
4.184 J/g/K = 4.184 x 150 x (318-274) = 27614 Joules
You mean how much heat energy will be lost/transferred as you are losing Joules here. All in steam, so a simple q problem and no change of state. 2.67 kg = 2670 grams q = (2670 grams steam)(2.0 J/gC)(105 C - 282 C) = - 9.45 X 105 Joules ----------------------------------- This much heat energy must be lost to lower the temperature of the steam.