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Thermal equilibrium

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10.0g of Fe(s) at 98.0 degrees Celsius is placed in 50.0mL of H2O(l) at 20 degrees Celsius. Assuming no energy is lost to the surroundings what is the final temperature of Fe(s) and H2O(l) at thermal equilibrium?

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Let t be the final temperature of iron+water
Specific heat of iron = 0.11 ...

Solution Summary

The thermal equilibrium are analyzed.

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Suppose you add 113.1 grams of ice to 200.1 grams of water in an insulated cup, where the water is initially at 34.9 oC. How many grams of ice remain after the system reaches thermal equilibrium?

The heat capacity of water is 4.184 J/goC and the enthalpy of melting ice is 334 J/g. If all the ice is melted, just enter 0.00

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