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The temperature of 15 grams of water is increased by 3.0 Celsius degrees How much heat in Joules was absorbed by the water?
To calculate the heat absorbed by the water, you can use the formula: heat = mass * specific heat capacity * temperature change. First, determine the specific heat capacity of water (4.18 J/g°C). Then, plug in the values: heat = 15 g * 4.18 J/g°C * 3.0°C. The heat absorbed by the water is 188.1 Joules.
How much energy is needed to increase the temperature of a kilogram of water 5 degrees?
The specific heat capacity of water is 4.186 J/g°C. Since there are 1000 grams in a kilogram, it would require 20,930 Joules of energy to increase the temperature of a kilogram of water by 5 degrees Celsius.
How much heat in joules would you need to raise the temperature of 1kg of water by 5 and degC?
You would need 20,920 Joules of heat to raise the temperature of 1kg of water by 5°C. This value is calculated using the specific heat capacity of water, which is 4186 J/kg°C.
How much energy is required to raise 21kg of water by 2 degrees Celsius?
The specific heat capacity of water is 4.18 J/g°C. To calculate the energy required to raise 21 kg of water by 2 degrees Celsius, use the formula: Energy = mass x specific heat capacity x temperature change. Plugging in the values, the energy required is 21,084 Joules.
Does it take more energy to heat the water to 100 degrees Celsius or to boil it?
q (heat energy in Joules) = mass * specific heat * change in temp 1st problem: q = (100 g H2O)(4.180 J/gC)(100 C - 50 C) = 20900 Joules ---------------------- 2nd problem: q = (100 g H2O)(4.180 J/gC)(70 C - 60 C) = 4180 Joules --------------------- As you can see from 50 C to 100 C takes much more heat energy as one would intuitively think, 20900 J/4180 J = 5 times as much energy.
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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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.
If you wish to heat water from thirty degrees to one hundred degrees how much heat will be required?
70 calories per gram. (The specific heat capacity of water is 1 calorie per gram per degree C.) This could be converted into Joules if necessary using the conversion factor of 1 calorie = 4.18400 Joules.
How much heat must be lost by 2 grams of water at 0 degrees Celsius to change it to ice?
The heat lost by water at 0 degrees Celsius to change to ice is equal to the heat of fusion of water, which is about 334 joules per gram. So, for 2 grams of water, the heat loss would be 2 * 334 = 668 joules.
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.
How much heat energy would be required to bring a 15 kg block of ice from -20 degrees Celsius to steam at 120 degrees Celsius?
To bring the ice block to 0 degrees Celsius, you would need 150,000 Joules (Q = mcΔT). To melt the ice at 0 degrees Celsius, you would need 3,375,000 Joules (Q = mLf). Heating the water from 0 to 100 degrees Celsius would require 1,500,000 Joules (Q = mcΔT). Turning the water to steam at 100 degrees Celsius would need 10,500,000 Joules (Q = mLv). Finally, heating the steam to 120 degrees Celsius would require 600,000 Joules (Q = mcΔT). In total, you would need 15,125,000 Joules of heat energy.
The temperature of 15 grams of water is increased by 3.0 Celsius degrees How much heat in Joules was absorbed by the water?
To calculate the heat absorbed by the water, you can use the formula: heat = mass * specific heat capacity * temperature change. First, determine the specific heat capacity of water (4.18 J/g°C). Then, plug in the values: heat = 15 g * 4.18 J/g°C * 3.0°C. The heat absorbed by the water is 188.1 Joules.
How much energy must be supplied to turn 1 gram of water at 100 degrees centigrade to steam at 100 degree centigrade?
Heat of vaporization of water is 2.26 x 106 joules per kg. Therefore 1 gram of water will need 2.26 x 103 joules.
How much heat in joules to heat a 40 g sample of aluminum from 73 degrees f to 142 degrees f?
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 =============
How much heat is required to convert 0.3 kilogram of at 0 degrees C to water at the same temperature?
Measured in joules, the process would take 334,584 J to occur completely.
How much energy is needed to melt 0.25 moles of water?
The necessary heat is 9,22 joules.
How much heat is absorbed by water when 250g of iron is heated from 27 degrees Celsius to 300 degrees Celsius?
q = (250 g)(0.46 J/gC)(300 C - 27 C) = 3.1 X 104 Joules -------------------------
