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How many joules of heat are needed to change the temp of 40 g of water?
Wiki User
∙ 12y ago
167.2J if it doesn't have to do with phase changes.
Wiki User
∙ 12y ago
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How many joules of energy are needed to heat 25.0 grams of steam from 100.0 degrees Celsius to 29.25 degrees Celsius?
Use this formula. q(in Joules) = Mass * specific heat * change in temperature I will use specific heat of water at 25 C. You can look up specific heat of steam. You say " heat to " so I assume you have final and initial heat backwards. q = 25.0 grams H2O * 4.180 J/gC * (100.0 C - 29.25 C ) q = 7393 Joules
The temperature of 15 grams of water is increased by 3.0 Celsius degrees How much heat in Joules was absorbed by the water?
I assume you mean 30o Celsius. Use this formula.q(joules) = mass * specific heat * change in temperatureq = (15 grams water)(4.180 J/gC)(40o C - 30o C)= 627 joules==========( perhaps 630 joules to be in significant figures territory )
What is the change in the internal energy of a system that does 400 joules of work and absorbs 700 joules of heat?
400 joules.
What is the heat formula?
the formula for heat is: joules= change in temp* mass* cpby: Professor Thompson
How much heat is generated by 1700 joules of work?
If all 1700 Joules of work get converted into heat, then, of course, you get 1700 Joules of heat.
Approximately how many Joules of heat are needed to completely change 10.0 grams of ice to water at the melting point temperature?
134 joules. You're very welcome for answering your question.
How many joules are required to boil 21.1 g of water at 100 C?
The needed heat is 47,65 Joules.
How much energy is needed to melt 0.25 moles of water?
The necessary heat is 9,22 joules.
Calculate the joules of heat needed to cool 159 g of water at 100oC to water at 65oC?
20 degree c\
How much heat in joules is needed to raise the temperature of 4.0 L of water from 0 degrees Celsius to 70.0 degrees Celsius?
It takes 4.186 Joules to heat one gram of water by 1-degree Celsius. 4.186 * 4000 = 16,744 Joules to heat 4 kilos of water by 1-degree. 16,744 * 70 = 1,172,080 Joules. The above assumes that one litre of water weighs exactly 1 Kilogram.
How many joules of heat are needed to raise the temp of 2.83 kg of water from 38C to 46C?
0.0796
What is the heat change when 55.0g water cools from 60 degree celsius to 25.5?
q(joules) = mass * specific heat * change in temperatureq = (55.0 g H2O)(4.180 J/gC)(25.5o C - 60o C)= (- ) 7932 Joules=============heat change
How many joules of heat are needed to completely vaporize 24.40 grams of water at its boiling point?
The answer is 55,117 kJ.
What is an amount of water whose temperature would change by 15 degrees Celsius when it absorbs 2646 joules of heat energy?
The amount of water whose temperature would change by 15 degrees Celsius when it absorbs 2646 joules of heat energy is 42,2g H2O.
How much energy would be needed to raise the temperature of 10 kilograms of water from 273 to 373 K?
10ml's of water is equal to 10cm3 of water. 10cm3 of water has a mass of 10g. The specific heat of water is 4.134 J/K. The change in temperature is 1 degree Kelvin. Use Q=mC∆T which means Heat= (Mass)(Specific Heat)(Change in Temperature) Q= (10)(4.134)(1) Q=(10)(4.134) Q=41.34 Joules
Suppose you want to heat 40g of water by 20c how many joules of heat are required?
334.8 Joules
If it takes 31500 joules of heat to warm 750 g of water what was the temperature change?
10 degrees Celsius
