Question

Suppose that 100.0 g of ice at 0 degrees Celsius are added to 300.0 g of water at 25.00 degrees Celsius. Is this sufficient ice to lower the temperature of the water to 5.00 degrees Celsius and still have ice remaining? Calculate the energy (heat), which must be removed from water to achieve the desired temperature change, and then prove that there is (is not) sufficient ice to cool the water. Use the specific heat capacity of water (4.184 J/g-*C) and heat of fusion of ice (335 J/g).

Answer 1

Amount of heat that must be removed from 300.0 g of water to decrease temperature from 25.00 deg ree celsius to 5.00 degree celsius is mass specific heat capacity temperature change. It is .....(1)
Amound of heat required to melt 100.0 g of ice at 0 degree celsius is the product of mass and heat of fusion of ice. It is ....(2)
As (2) > (1), ice is sufficient to lower the temperature of the water to 5.00 degree celsius and still have ice remaining. Also when ice is melted to form water at 0 degree celsius, some heat will be required to increase its temperature from 0 degree celsius to 5 degree celsius.