To treat a burn on your hand, you decide to place an ice cube on the burned skin

Question

To treat a burn on your hand, you decide to place an ice cube on the burned skin. The mass of the ice cube is 11.3 g, and its initial temperature is -14.4 °C. The water resulting from the melted ice reaches the temperature of your skin, 32.0 °C. How much heat is absorbed by the ice cube and resulting water? Assume that all the water remains in your hand. _________ J

Constants may be found here:

Quantity per gram per mole Enthalpy of fusion 333.6 J/g 6010. J/mol Enthalpy of vaporization 2257 J/g 40660 J/mol Specific heat of solid H2O (ice) 2.087 J/(g·°C) * 37.60 J/(mol·°C) * Specific heat of liquid H2O (water) 4.184 J/(g·°C) * 75.37 J/(mol·°C) * Specific heat of gaseous H2O (steam) 2.000 J/(g·°C) * 36.03 J/(mol·°C) *

Explanation / Answer

heat absorbed = mass * specific heat of ice * change in temperature + enthalpy of fusion * mass

heat absorbed = 11.3 * 2.087 * (32 - (-14.4)) + 11.3 * 333.6

heat absorbed = 4863.93584 J

Related Questions

Navigate

• Browse (All)
• Browse T
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.