200 g of ice at 0°c is dropped into a calorimeter of negligible heat capacity containing 350 g of water at 20°c. what is the temperature of the system when it reaches equilibrium? the latent heat of fusion of water is 80 cal/g.

The temperature of the system when it reaches equilibrium is 0°C.

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.

answers: to make sure that all of the broken pieces of tablet were added to the water, to allow for fair comparison of all three trials, with different particle sizes to avoid experimental error