A 250[g] aluminum calorimeter contains 600[g] of water at 20.0[°C]. An aluminum shot with a mass equal to 400[g] is heated to 150.0[°C] and is then placed in the calorimeter. Find the final temperature of the system, assuming that there is no heat transfer to the surroundings. Use cAl-910[Jkg.K] and cwater=4190[Jkg.K] Express your answer in [°C].
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- A cube of ice is taken from the freezer at -8.4°C and placed in a 94 g zinc cup filled with 307 g of water. Both the water & the cup are at 20.1°C. Eventually the system reaches thermal equilibrium at 18.4°C. Determine Qcup Qwater (for the water initially in the cup), Qice, & the mass of the ice. Qcup = Qwater Specific heat Solids (J/kg.K) Aluminum 900 Liquids Specific heat (J/kg.K) Brass 402 Bromine 473 Copper 377 Ethyl 2400 Alcohol Glass 840 Gasoline 2220 Gold 126 Glycerin 2430 Ice 2095 Mercury 140 Iron 461 Water 4186 Qice mice = Lead 130 Nickel 502 Latent Heat Substance (J/kg) Silver 239 Steam water 2,260,000 Styrofoam 1131 Ice water 333,000 Zinc 390x. 62: 1 kg of ice occupies 1.1 × 10 m² al normal pressure. The volume changes to 1.0 x 10 m' when it is melted. Find the internal latent heat of ice. Given : Latent heat of fusion of ice = 80 kcal/kg Density of mercury = 13600 kg/m³, Mechanical equivalent of heat J = 4200 Joules/k cal.A laboratory technician drops a 0.0850 kg sample of unknownsolid material, at 100.0°C, into a calorimeter. The calorimeter can, initiallyat 19.0°C, is made of 0.150 kg of copper and contains 0.200 kgof water. The final temperature of the calorimeter can and contents is26.1°C. Compute the specific heat of the sample.
- °C ST 9. A 730 g piece of copper is heated in a furnace to a temperature T. The copper is then inserted into a 165 g copper calorimeter containing 265 g of water. The initial temperature of the water and calorimeter is 19 °C, and the final temperature after equilibrium is established is 40 °C. When the calorimeter and its contents are weighed, 31.0 g of water are found to have evaporated. What was the J/kg, Ccopper = 387 J/(kg. °C) ssf60 ssf6mperature T?(cw = 4186 J/(kg.°C), Lf=3.35 × 10³ J/kg, Lv=2.26 × 106 £60 ssf60** JSS (9588 ssf60 V9JSS* £60 SSA bar of lead (bar A) is in thermal contact with a bar of silver (bar B) of the same length and area. One end of the compound bar is maintained at Th = 81.0°C while the opposite end is at 30.0°C. Find the temperature at the junction when the energy flow reaches a steady state. °C Th A B 30.0°C InsulationA 0.1375-g sample of magnesium is burned in a constant-volume bomb calorimeter that has a heat capacity of 1769 J °C1. The calorimeter contains exactly 300 g of water, and the temperature increases by 1.126°C. Calculate the heat given off by the burning magnesium, in kJ g-l and in kJ mol-!. The specific heat of water is 4.184 J g1 °C -1.
- A 40.-g block of ice is cooled to -78°C and is then added to 560 g of water in an 80.-g copper calorimeter at a temperature of 25°C. Determine the final temperature of the system consisting of the ice, water, and calorimeter. (If not all the ice melts, determine how much ice is left.) Remember that the ice must first warm to 0°C, melt, and then continue warming as water. (The specific heat of ice is 0.500 cal/g . °C = 2090 J/kg . °C.)A hot lump of 37.4 g of aluminum at an initial temperature of 65.9 °C is placed in 50.0 mL H,O initially at 25.0 °C and allowed to reach thermal equilibrium. What is the final temperature of the aluminum and water, given that the specific heat of aluminum is 0.903 J/(g.°C)? Assume no heat is lost to surroundings. Trinal °CA cylindrical metal boiler of radius 10 cm and thickness 3.14 cm is filled with water and placed on an electric heater. If the water boils at the rate of 50 g s', estimate the temperature of the fila- ment. Thermal conductivity of metal 102 w m K- and latent heat of vaporisation = 2.26 x 10° J g'. = 1.13 × %3D
- How much thermal energy (in J) is required to boil 2.45 kg of water at 100.0°C into steam at 135.0°C? The latent heat of vaporization of water is 2.26 ✕ 106 J/kg and the specific heat of steam is 2010 J kg · °C . HINT JA 7244 gram copper metal is heated to 126°C and dropped into 113.44 gram of ter at an initial temperature of Tw. When equilibrium is reached the temperature of copper-water mixture is 25.3°C. Calculate the initial temperature of water? If the specific heat of copper is 385 J/kg°C and Specific heat of water is 4186 J/kg C. Initial temperature of water in (PC) = hp HEWL ETT-P ACKARDA 1.50-kg iron horseshoe initially at 600°C is dropped into a bucket containing 20.0 kg of water at 25.0°C. The final temperature of water and iron is 29.5 °C. What is the heat capacity of iron? (Ignore the heat capacity of the container and assume that a negligible amount of water boils away.) Find % error. The specific heat of iron is 448 J/kg °C.