A 600 g lump of copper at 80.0oC is placed in 70.0 g of water at 10.0oC

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A 600 g lump of copper at 80.0oC is placed in 70.0 g of water at 10.0oC in an insulated container. (See Table 18-3 for specific heats.)

(a) What is the equilibrium temperature of the copper-water system? What entropy changes do?

(b) The copper,

(d) The copper-water system undergo in reaching the equilibrium temperature?

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Fundamentals of Physics

ISBN: 978-0471758013

8th Extended edition

Authors: Jearl Walker, Halliday Resnick

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Question Posted: Jan 19, 2011 06:47 AM

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A 600 g lump of copper at 80.0oC is placed in 70.0 g of water at 10.0oC

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a Starting from Q0 for calorimetry problems we can derive ...View the full answer

Fundamentals of Physics

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