A 2.0-kg mass of iron (specific heat = 0.12 kcal/kg · Cº)at a temperature of 430ºC is dropped into 48 kg of water.The water is initially at a temperature of 10ºC.With no heat losses to the surroundings,the equilibrium temperature of the iron and water is approximately

Question

Quizplus · Accepted Answer

The equilibrium temperature can be found using the principle of conservation of energy, where the heat lost by the iron is equal to the heat gained by the water. The formula for heat (Q) is Q = mcΔT, where m is mass, c is specific heat, and ΔT is the change in temperature. For iron, Q_iron = m_iron * c_iron * (T_final - T_initial_iron), and for water, Q_water = m_water * c_water * (T_final - T_initial_water). Since Q_iron = -Q_water (heat lost by iron is gained by water), we can set their magnitudes equal and solve for T_final. Given the specific heat of water is approximately 1 kcal/kg·ºC, and using the given values, solving the equation yields a final temperature close to 12ºC, indicating that option A is correct.

A 20-Kg Mass of Iron (Specific Heat = 0