An insulated container is used to hold 43.40 g of water at 18.20 degree C. A sam

Question

An insulated container is used to hold 43.40 g of water at 18.20 degree C. A sample of copper weighing 14.90 g is placed in a dry test tube and heated for 30 minutes in a boiling water bath at 100.10 degree C. The heated test tube is carefully removed from the water bath with laboratory tongs and inclined so that the copper slides into the water in the insulated container. Given that the specific heat of solid copper is 0.385 J/(g. degree C), calculate the maximum temperature of the water in the insulated container after the copper metal is added.

Explanation / Answer

Heat lost by copper= heat gained by water

let T= Equilibrium temperature

Heat lost by copper= mass of copper* specific heat* temperature difference= 14.9*0.385*(100.10-T)

high thermal conductivity of copper ensures in copper reaching 100.10deg.c

Heat gained by water= 43.4*4.18*(T-18.2)

14.9*0.395*(100.10-T)= 43.4*4.18*(T-18.2)

14.9*0.395*100.10- 14.9*0.395T= 43.4*4.18T- 43.4*4.18*18.2

589.14- 5.9T= 181.4T- 3301.7

T*(181.4+5.9) =589.14+3301.7

187.3T= 3890.84

T= 20.77 deg.c

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