If a 62.1 gram piece of copper is heated to 100.0oC and then put into a vessel containing 250.0 mL of water at 1.5oC, what will be the final temperature of the water (in oC)?  Take the molar heat capacity of copper to be 24.4 J/(mol oC) and that of H2O(l) to be 75.3 J/(mol oC).  Assume the density of water is 1.00 g/mL.Your answer should have 3 significant figures.

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Asked Oct 14, 2019
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If a 62.1 gram piece of copper is heated to 100.0oC and then put into a vessel containing 250.0 mL of water at 1.5oC, what will be the final temperature of the water (in oC)?  Take the molar heat capacity of copper to be 24.4 J/(mol oC) and that of H2O(l) to be 75.3 J/(mol oC).  Assume the density of water is 1.00 g/mL.

Your answer should have 3 significant figures.

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The moles of copper and water...

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Given, Copper 62.1g water 50.0mL massof water=volumex Density 250.0mLx 250.0g mL mass molesof water=. molarmass 250.0g 18.015 g/mol _mass of Copper -13.8771 mol molesof Copper molar mass 62.1g 63.546 g/mol .=0.9772 mol

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