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A hot lump of 43.0 g of iron at an initial temperature of 62.6 °C is...

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Chemistry

A hot lump of 43.0 g of iron at an initial temperature of 62.6°C is placed in 50.0 mL of H2O initially at 25.0 °C and allowed toreach thermal equilibrium. What is the final temperature of theiron and water given that the specific heat of iron is 0.449J/(g·°C)? Assume no heat is lost to surroundings.

Answer & Explanation Solved by verified expert
4.2 Ratings (572 Votes)
Let t be the equilibrium temperature attained by the system Heat gained by water Heat lost by iron mcdt    See Answer
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