Answer:
The temperature of the system when it reaches equilibrium is 0°C.
Step-by-step explanation:
Heat gained by ice at 0 °C to convert into 0 °C water is:
Mass of ice at 0 °C = 200g
Enthalpy of fusion is defined as the the heat gain when 1 g of the substance at its freezing point melts to liquid under standard pressure.
Thus heat gained by water = 80 calg⁻¹×200 g = 16000 kcal
Heat lost by water at 20 °C to convert to 0 °C:
The relation between heat released/gained in a system and the temperature is:
where,
Q=mcΔT
Q is the amount of heat absorbed or released
m is the mass
ΔT is the change in temperature
c is called the specific heat.
Specific heat is defined as heat gained by 1 unit mass of any sample to raise the temperature by 1 °Celsius.
Thus, from the question:
Mass of water =350 g
ΔT = (20 -0)°C = 20°C
Specific heat of water = 1 cal/g°C
Thus, Heat lost by water :
Q = 350 g×1 cal/g°C×20°C = 7000 cal
Thus, Heat lost < Heat gained, the system is yet at equilibrium. Not all the ice melt in the system.
Thus, The temperature of the system when it reaches equilibrium is 0°C.