# Thermal Equilibirum Calorimeter

Question

A copper calorimeter can with mass 0.100 kg contains 0.160 kg of water and 0.018 kg of ice in thermal equilibrium at atmospheric pressure.

If 0.750 kg of lead at a temperature of 255 degrees C is dropped into the calorimeter can, what is the final temperature? Assume that no heat is lost to the surroundings.

Related Formula

$$Q_1 + Q_2 + Q_3 = 0$$

$$Q = mc\Delta T$$

$$\Delta T = T_{initial} - T_{final}$$

The initial temperature of the Ice/Water/Container, so I am not quite sure what the best way to start this question is.

Any suggestions?

TFM

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Hootenanny
Staff Emeritus
Gold Member

As for your question, I offer you a hint: what is the temperature at which ice and water exists at thermal equilibrium?

Sorry, I htought there was something different Feel free to move to 'Homework and Coursework: Introductory Physics' Category.

Would this be at the Triple point, which I is 0.0098 degrees Celcius, 273.1598 Kelvin. This must be the intial Temperature?

Hootenanny
Staff Emeritus