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A 75 g piece of gold (Au) at 1000 K is dropped into 200 g of H2O at 300K in an insulated container at 1 bar. Calculate the temperature of the system once the equilibrium has been reached. Assume that CP,m for Au and H2O are constant and its value for 298 K throughout the temperature range of interest.

Respuesta :

Answer:

The temperature of the system once the equilibrium has been reached = 372.55K

Explanation:

Heat capacity of gold = 129 J/Kg*c.

Heat capacity of water

4,184 J/Kg*c.

Mass of gold = 75g = 0.075Kg

Mass of water = 200g = 0.2Kg

From conservation of energy

m1×C1×(t11 - t2) = m2×C2×(t2- t21)

Substituting we have

0.075 × 129×(1000-t2) = 0.2× 4184×( t2 -300) =solving for t2, we have

933.55×t2 = 347790

or t2 = 372.55K

The temperature of the system once the equilibrium has been reached = 372.55K

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