A 1.50-kg iron horseshoe initially at 660°C is dropped into a bucket containing 22.5 kg of water at 21.0°C.What is the final temperature of the water-horseshoe system? Ignore the heat capacity of the container andassume a negligible amount of water boils away.Step 1The water will gain the energy lost by the iron. Using the expressions for the quantity of heat exchanged bythe two materials, the change in water temperature can be found. The specific heat of iron is 448 J/kg-°C andthe specific heat of water is 4,186 J/kg.°C.We assume that the water-horseshoe system is thermally isolated (insulated) from the environment for theshort time required for the horseshoe to cool off and the water to warm up. Then the total energy input fromthe surroundings is zero, as expressed by the equationQiron + Qwater = 0.The energy Q transferred between a sample of mass m of a material and its surroundings with a temperaturechange AT is given byQ = mcAT.Substituting the expressions for iron and water into the energy equation, we have(mcAT)iron + (mcAT) water = 0or, with T as the final temperature of both the iron and the water,'iron iron]°c) + mwater water|ec) = 0.Note that the first term in this equation results in a negative number of joules, representing energy lost bythe originally hot horseshoe, and the second term is a positive number with the same absolute value,representing energy gained in heat by the colder water.

The heat lost by the iron will be the heat gained by the water. Let Tf be defined as the final…

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A 1.50-kg iron horseshoe initially at 660°C is dropped into a bucket containing 22.5 kg of water at 21.0°C. What is the final temperature of the water-horseshoe system? Ignore the heat capacity of the container and assume a negligible amount of water boils away.