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A blacksmith heats a 1,540 g iron horseshoe to a temperature of 1445°C before dropping it into 4,280 g of water at 23.1°C. If the specific heat of iron is 0.4494 J / g °C, and the water absorbs 947,000
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A blacksmith heats a 1,540 g iron horseshoe to a temperature of 1445°C before dropping it into 4,280 g of water at 23.1°C. If the specific heat of iron is 0.4494 J / g °C, and the water absorbs 947,000 J of energy from the horseshoe, what is the final temperature of the horseshoe-water system after mixing?

A. 734°C
B. 298°C
C. 76.7°C
D. 29.8°C

User Nagelfar
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1 Answer

3 votes
The answer is c
76.7 C
User Ratnesh
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