A 50 g ice at `0^(@)C` is added to 200 g water at `70^(@)C` taken in a flask. When the ice has melted completely, the temperature of the flask and the contents is reduced to `40^(@)C`. Now to bring down the temperature of the contents to `20^(@)C`, find a further amount of ice that is to be added.

10 g ice at 0^(@)C is mixed with 20 g of water at 20^(@)C . What is the temperature of mixture?

One gram of ice at 0^(@)C is added to 5 gram of water at 10^(@)C . If the latent heat of ice be 80 cal/g, then the final temperature of the mixture is -

Ice at 0^@C is added to 200 g of water initially at 70^@C in a vacuum flask. When 50 g of ice has been added and has all melted the temperature of the flask and contents is 40^@C . When a further 80 g of ice has been added and has all melted the temperature of the whole becomes 10^@C . Find the latent heat of fusion of ice.

Ice at 0^@C is added to 200 g of water initially at 70^@C in a vacuum flask. When 50 g of ice has been added and has all melted the temperature of the flask and contents is 40^@C . When a further 80 g of ice has been added and has all melted the temperature of the whole becomes 10^@C . Find the latent heat of fusion of ice.

300 g of water at 25^(@)C is added to 100 g of ice at 0^(@)C . The final temperature of the mixture is

50g of ice at 0^(@)C is mixed with 200g of water at 0^(@)C.6 kcal heat is given to system [Ice +water]. Find the temperature (in .^(@)C ) of the system.