Question

Example - How many joules of energy must a cup of coffee lose for its temperature to drop from 60.0°C to the temperature of your body (37.0°C)? Assume that the cup holds 250. mL of coffee (with a density of 1.00 g/mL) and that the specific heat of coffee is the same as water (4.18 J/g°C).

Answer 1

Density ot coffee 19/mL mass of coffee = coffee 9(mL X 250 mL 250 9 coffee Specific heat of toffee = 4.18 3/gc Hences will absorb heat 4.18 Jto imerease its 9 Coffee temperatwe by we can say that, 4. 18Jheat if it lower its coffee will Yelease 14 temperature by 1c heat 1045 J (4.18 X 250) coffee will release 250 9 heat when it Lower its temperature by c total lowering of temperature (60°c 37) Here 23°c Now 1045 Jheat when 1t lower its 250 9coffee releases temperature by C when tempehature will be lowehed by 23 9 energy releas ed will be (1045x 23)J 24035 7 be Henceg energy will Losed by the coffee. 24035 J