# Calorimetry: mix of ice, water vapor inside a copper container

**1. The problem statement, all variables and given/known data**

We insert into a copper container (weighing 1.5 Kg) 3 Kg of water vapour at 100 ºC. Inside the container there are 10 Kg of ice at -10ºC. Find the ΔT when the system reaches the equilibrium.

Known data: the specific heats of water, copper and ice and the latent heat of ice and water vapour.

**2. Relevant equations**

Q=mcΔT

**3. The attempt at a solution**

We know that ΔT is equal for all the components when the equilibrium point is reached, therefore:

[itex]\left\{\begin{matrix}Q_{absCopp}+Q_{absIce}=Q_{relsVapour}

\\ \Delta T=\frac{Q_{abs(Copp)}}{m_{Cu}c_{Cu}}=\frac{Q_{abs(Ice)}}{m_{ice}c_{ice} }=\frac{Q_{rels(Vapour)}}{m_{vapor}c_{vapor}}

\end{matrix}\right.[/itex]

I don’t know how to proceed. The changes of state confuse me. Please give me some clues.

Have a nice day.

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