Calculate the thermal capacity of 200 gm Aluminium. Specific heat capacity of Aluminium `0.21` calorie `gm^-1` `@C^-1`.

What is the thermal capacity of 40 gm of aluminium? Specific heat of aluminium is 0.2 cal g^-1^@C^-1 .

5 gm of ice at -10^@C are mixed with 20 gm of water at 39^@C . Will whole of the ice melt? If so, what is the final temperature of the mixture? Specific heat capacity of ice = 0.5 cal gm^-1 "^@C^-1 and latent heat of fusion of ice = 80 cal gm^-1 , specific heat capacity of water = 1cal gm^-1 "^@C^-1 .

Calculate the number of moles in 1.5 gm of amonia.

Calculate the increase in energy (in joule) per atom of a piece of aluminium when its temperature is raised by 1^(@)C . Given 27 g of aluminium contains 6xx10^(23) atoms, and specific heat capacity of aluminium ="0.2 cal .g"^(-1).^(@)C^(-1) .

How much heat is required to rise temperature from -8^@C to 50^@C of 10gm ice. Specific heat of ice 0.5 calorie gm ^-1^@C^ - 1 .

Calculate the number of kJ of heat necessary to raise the temperature of 60.0 g of aluminium from 35^@C to 55^@C . Molar heat capacity of Al is 24 J mol^-1 K^-1 . Molar mass of Al =27g mol^-1 .

A sample of 100 gm of water is slowly heated from 27^(@)C to 87^(@)C . Calculate the change in the entropy of water. Specific heat capacity of water = 4200 J cdot kg^(-1) cdot K^(-1)

A piece of iron of mass 100 gm is kept inside a furnace for a long time and then put in a calorimeter of water equivalent 10 gm containing 240 gm of water at 20°C. The mixture attains an equilibrium temp. of 60^@C . Find the temperature of the furnace. Specific heat capacity of iron = 470 J kg^-1"^@C^-1 .

A piece of platinum of mass 200 g, is heated for a sufficiently long time in a furnace and dropped quickly in 650 g of water at 10^(@)C , kept in a container of water equivalent 50g. Final temperature of the mixture becomes 25^(@)C . If the specific heat capacity of platinum is "0.03 cal.g"^(-1).^(@)C^(-1) , find the temperature of the furnace.