Specific HeatEquipment NeededBeaker, 250 mlCup, StyrofoamCylinder Set, DensityHot PlateScale, BalanceString, BlackThermometer, DigitalObjectiveThe purpose of this lab is to determine the specific heats of several different metals.IntroductionIf you mix hot and cold water together, the temperature of the final mixture depends on how much hot water is added to how much cold water. If you throw a hot branding iron into a pail of cool water, you know that the temperature of the iron will go down. You also know that the temperature of the water will rise—but will its rise in temperature be more, less, or the same as the temperature drop of the iron? That is, will the temperature of the water rise as much as the temperature of the iron goes down? Or will the changes of temperature instead depend on the relative masses of the iron and the water?In this experiment, you are going to investigate the quantity of heat per gram per degree (Celsius), known as the specific heat. Water has a specific heat of 1.00 cal/gC--relatively large compared to most substances.The heat (Q) lost by a specimen, say a piece of metal, submerged in water equals the heat (Q) gained by the water and by the container. In this experiment we will neglect the heat absorbed by the Styrofoam container, as it is negligible.Qlost = QgainedHeat, Q = Specific Heat of Substance x Mass of Substance x Change in Temperature. Heat lost by metal block = Heat gained by waterCmMm(Tim - Tf) = CwMw(Tf - Tiw) Equation 1where Cm=specific heat of the metal Mm=mass of metal Tim=initial temperature of the metal Tf=final temperature of metal and water Cw=specific heat of water Mw=mass of water Tiw=initial temperature of water ProcedureBegin by boiling water in a beaker half full of water.Warning: Never set a glass beaker on a hot plate that is already hot.Find the mass of the metal (Mm) and record it in the table.Attach a piece of string to the metal and lower it into the beaker. Be sure the metal is completely immersed in the water. Heat the metal in the water for at least 5 minutes. Our assumption will be that the metal’s temperature is the same as that of the boiling water. Measure and record the temperature of the boiling water. This is equal to the initial temperature of the metal (Tim).Find and record the mass of the empty calorimeter cup. (Mc).Fill the calorimeter cup about one-half full of cold water (about 3 below room temperature) and find the mass of the cup and water (Mcw). Subtract the mass of the cup to obtain the mass of the water in the cup (Mw).Find and record the initial temperature of the water (Tw).Holding the metal block by the string, quickly (but carefully) transfer the metal block into the calorimeter cup.Stir and record the temperature of the water when it reaches its highest point (Tf).Calculate the specific heat of the metal by using Equation 1.Compare the specific heat of the metal by its accepted value. Calculate the percent error.Repeat the above procedure for a different metal.Data TableType of MetalMass of MetalMm (g)Mass of cup + waterMcw (g)Mass of cupMc (g)Mass of WaterMw (g)TimoCTiwoCTf oCSpec.Ht.Experi.(cal/goC)%error1100450501002021.82100450501002024Specific Heats for Laboratory Samples at 20o CFe 0.119cal/g °CCu0.092cal/g °C Sn 0.054 cal/g °C Zn .0925cal/g °CAl 0.214cal/g °CPb 0.0306cal/g °CBrass.0917cal/g °C