In the previous question you were provided with an extra piece of information: Y

Question

In the previous question you were provided with an extra piece of information: You were told that only liquid water would be present once equilibrium was established. If the final state of a system is not given, it is still possible to determine it from the initial temperatures and masses. The next few parts will help illustrate this point. Suppose that in an insulated container, 0.100 kg of water at 20.0C is mixed with 1.500kg of ice at 15.0C. You are asked to find the final temperature Tf of the system, but you are not told what the final phase of the system in equilibrium is. Find the amount of heat Qh it would take to bring all of the ice to its melting point, 0C.

Explanation / Answer

Amount of heat needed to bring ice at melting point,

Qh = 1.500 x 2.108 x 10^3 x ( 0 - (-15))

Qh = 47430 J ........Ans

amount of heat released by water,

Q1 = 0.100 x 4186 x 20 = 8372

heat released to convert water into ice,

Q2 = 0.100 x 333.55 x 10^3 = 33355 J

total heat released = 41727 J

41727 + (0.10 x 2108 x T ) = 1.50 x 2108 x (15 - T )

3372.8 T = 5703

T = 1.71 deg C

hence equilibrium temp is - 1.71 deg C . ...........Ans

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