Early pioneers would to reheat their coffee by placing an iron poker from the fi

Question

Early pioneers would to reheat their coffee by placing an iron poker from the fire directly into their cup. If the cup initially held 0.500 L of coffee at 20.1°C, what would be the final temperature of the coffee when a 5.00 x 102 g iron poker at 402.3 °C was placed in it? Assume that no heat is lost to the surroundings during the process, and that the heat capacity and density of coffee is that same as that of water (I’m sure it wasn’t very good coffee!). (note: you will need to look up the heat capacities in your text for the species in this problem!)

Explanation / Answer

specific heat capacity of iron= 0.451 J/gºC

specific heat capacity of water= 4.184 J/gºC

The heat gained by the coffe is equal to the heat lost by the iron.

0.5L= 0.5kg of coffe= 5x102g

heat coffe= heat Fe

5x102g x 4.184 J/gºC x (Tf - 20.1)ºC = 5x102g x 0.451 J/gºC x (402.3 - Tf)

Tf= 57,3ºC

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