How much heat (in Joules) does it take to raise the temperature of 100 g of H2O from 22 ̊C to 98 ̊C?
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How much heat (in Joules) does it take to raise the temperature of 100 g of H2O from 22 ̊C to 98 ̊C?
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- A kettle brings 2.15 kg of water at 34.9˚C to steam at 110˚C. How much heat does this take? The specific heat of water is 4186 J/kg˚C, The specific heat of ice is 2090 J/kg˚C, and the specific heat of steam is 2010 J/kg˚C The latent heat of fusion for water is 3.33 x 105 J/kg and the latent heat of vaporization for water is 2.26 x 106 J/kgHow much heat ? would be needed to completely evaporate 33.5 g of boiling water at a temperature of 100 ∘C? Express the answer in units of joules. The latent heat of vaporization for water at 100 ∘C is 2260 J/g.In an energy-efficient home, a solar collector is used to provide heat energy. If the solar system releases 42,000 cal of heat when it cools from 50 oC to 48 degrees C, what is the mass (kg) of water in the solar collector (specific heat = 1.00 cal / g x degree C)?
- 1) A Sample Of Water That Weigh 25g Absorbs 880J Of Energy. The Water Is Initially At 38.0 'C. What Is The New Temperature Of The Water In Degrees Fahrenheit? 2) A Sample Of Metal, Heated To 110'C, Is Placed Into A Calorimeter Containing 140g Of Water At 15.0'C. The Final Temperature Of The Metal And Water Is 28.0'C. What Is The Mass Of The Metal (m Metal)? Water Q= Cs= 4.184 M = Tfinal F Tinitial = AT = Metal Q= Cs= 0.628 M= Tfinal Tinitial = AT =The specific heat of a certain steel is0.46 J·g−1·K−1 and the specific heat of a “dry” wood is 1.8 J·g−1·K−1. Suppose we add a given amount of energy as heat to 10.0-gram samples of the steel and wood. (a) Which sample will undergo the largest temperature increase? (b) Calculate the ratio of the temperature increase for the two samples. answer: (a) steel, (b) 3.9 = steel/wood19. The following fission reaction (shown below) occurs in a nuclear power plant. There are 1.50 x 1016 uranium-235 atoms that are simultaneously undergoing this reaction. The uranium is surrounded by 17.5 kg of heavy water, which has a specific heat capacity of 4.70 x 10³ J/kg °C. If 90% of the energy released in the nuclear reactions is absorbed as thermal energy by the heavy water, determine the increase in temperature of he heavy water. ✔✔✔✔ 235U+n→ Zr + 139 Te + 3(n) 92 40 52 mzr-94 = 93.906 u MTe-139 = 138.935 u Mu-235 = 235.044 u
- An ice block of mass 1.2000000000000002 kg at an initial temperature of –11 ∘C is put into a copper pot of mass 2.5 kg containing 4.3 L of water at 21 ∘C. If you heat up the pot, what is the amount of energy (in J) you need to convert all the ice and the water into steam? (Assume that no energy is lost from the system.) You may need some or all of the following constants: The specific heat of ice is 2200 J/kg ∘C, the specific heat of copper is 386 J/kg ∘C and the specific heat of water is 4186 J/kg ∘C. The latent heat of fusion of ice is 334000 J/kg and the heat of vaporization for water is 2256000 J/kg .A 63 kg man had a fever of 41.45m ºC (normal body temperature is 37 ºC). Assuming that the human body is mostly water, how much heat was required to raise its temperature that much?Water with a mass of 0.500 kgkg at 15.0∘C∘C is mixed with 0.800 kgkg of water at 35.0∘C∘C. What is the final temperature TfTfT_f of the mixture?