A hot lump of 35.8 g of copper at an initial temperature of 70.7 °C is placed in 50.0 mL H2O initially at 25.0 °C and allowed to
reach thermal equilibrium. What is the final temperature of the copper and water, given that the specific heat of copper is 0.385 J/(g·°C)? Assume no heat is lost to surroundings.
1 answer:
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