A 720 g piece of copper is heated in a furnace to a temperature T . The copper i

Question

A 720 g piece of copper is heated in a furnace to a temperature T. The copper is then inserted into a 130 g copper calorimeter containing 295 g of water. The initial temperature of the water and calorimeter is 14 °C, and the final temperature after equilibrium is established is 37 °C. When the calorimeter and its contents are weighed, 30.0 g of water are found to have evaporated. What was the temperature T?(cw = 4186 J/(kg.°C), Lf=3.35 × 105 J/kg, Lv=2.26 × 106J/kg, ccopper = 387 J/(kg.°C)

*the answer is NOT 431.47

Explanation / Answer

Here ,

mass of water left , mW = 295 - 30

mW = 265 gm

mass of copper , mC = 720 gm

mass of calorimeter , mc = 130 gm

Now,

heat lost by copper piece = heat gain by water and calorimeter

mC*Ccu *(T - 37) = mW * Cw (37 - 14) + mc * Ccu *(37 - 14) + 30 * Lv

720 *(0.387) *(T - 37) = 265 * 4.186 * 23 + 130 * 0.387 * 23 + 30 *( (100 - 14)* 4.186 + 2.26 *20^3)

solving for T

T = 2118 degree C

the initial temperature of copper was 2118 degree C

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