One way to cool a cup of coffee is to plunge an ice-cold piece of aluminum into it. Suppose a 20.0g piece of aluminum is stored in the refrigerator at 32 degrees F(0.0 degrees C) and then put into a cup of coffee. The cofee’s temperature drops from 90.0 degrees C to 75.0 degrees C. How much energy (in kilojoules) did the coffee transfer to the piece of aluminum? Assume coffee and aluminum reach thermal equilibrium meaning same final temperature. The specific heat capacity of water and aluminum is 2.06 and 0.902 J g^-1degreesC^-1
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1 response so far ↓
1 esstee2001 // Oct 29, 2008
Heat lost by coffee = heat gained by aluminium
Heat gained by Al = mc x delta T = 20g x 0.902 J/g-degC x (75 - 0)degC = 1353 J = 1.353kJ