\"A sample of silver (106 g) was heated inside a dry test tube in a water bath u

Question

"A sample of silver (106 g) was heated inside a dry test tube in a water bath until the silver was the same temperature as the water. The temperature of the water was found to be 98.6 C. The silver metal was quickly transferred to 50.0 g of room-temperature water (24.5 C) and allowed to transfer its excess heat to this water. At the highest temperature reached, the water and metal sample reached a temperature of 32.4 C. Find the specific heat of silver. The specific heat of water is 4.18 J/g*deg." in the experiment described here, what would be the effect of hot water dripping into calorimeter from the outside of the heated test tube? Would the error introduced into the calculation of a metal's specific heat cause the reported value to be higher or lower than if the experiment were done correctly?

Explanation / Answer

Heat released by the silver block: M(Ag)Cp(Ag)(98.6-32.4) J= 106*(98.6-32.4)Cp(Ag) J. Heat accepted by water: 50*4.18*(32.4-24.5)J. These are equal, assuming no heat ;loss to the surroundings,we have,equating these quantities,Cp(Ag)= 0.2353 J/gm*C

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