1.5kg iron horse shoe initially at 600°c, it dropped into a bucket containing 20kg of water at 25°c. what is the final temperature. (ignore heat capacity of the container) and assumed that a negligible amount of water boils always. (SHC of water 4186jkg°c, SHC of iron is 448jkg°c

Question

Rosy

Physics

29 December, 11:18

1.5kg iron horse shoe initially at 600°c, it dropped into a bucket containing 20kg of water at 25°c. what is the final temperature. (ignore heat capacity of the container) and assumed that a negligible amount of water boils always. (SHC of water 4186jkg°c, SHC of iron is 448jkg°c

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Skyler Huffman · Answer 1

Let final temperature be θ

You have not given values for specific heat capacities, but any text-book will give the figures as

Iron = 460 J/kgK

Water = 4187 J/KgK

Heat lost by horse shoe = heat gained by water (mC δt)

1.5 x 460 x (600 - θ) = 20 x 4187 x (θ - 25)

690 (600 - θ) = 83740 (θ - 25)

414000 - 690 θ = 83740 θ - 2093500

2507500 = 84430 θ

θ = 29.7 C

Final temperature of horse shoe and water is 29.7 C