A 5.0 g sample of a certain metal is heated to 100.0 degree Celsius and is quick

Question

A 5.0 g sample of a certain metal is heated to 100.0 degree Celsius and is quickly immersed in a calorimeter that contains 10.0 g of water at 20.0 degree Celsius. The metal, water, and calorimeter (heat capacity= 10.0 J/degree Celsius) reach equilibrium temperature at 25.0 degree Celsius. The molar mass of the metal is 60. Determine the metal's molar heat capacity. I Know the equation is specific heat times mass times change in temperature but I can not figure out exactly what is molar heat capacity. I believe in the zumdahl 7th edition refers to my question.

Explanation / Answer

Molar heat capacity is the specific heat capacity per mole ofsubstance. . Heat given out by the metal = moles * molar heat capacity *temperature difference                                           =(mass /molar mass) * molar heat capacity * temperaturedifference                                           =(5.0 g / 60 g/mol) * mhc * (100-25)                                           =6.25 mhc . Heat absorbed by the water = 10.0 g * 4.184 J/ (g.C) * (25-20) C                                           = 209.2 J . Heat absorbed by the calorimeter = Heat capacity * temperaturedifference                                                    = 10.0 J/C * (25-20)C                                                    = 50.0 J . Heat given out by the metal is equal to the heat absorbed bythe water and calorimeter    So we get 6.25 mhc = 209.2 J + 50.0 J       So molar heat capacity ofthe metal = 41.742 J/ (mol.C)

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