`0.3 Kg` of hot coffee, which is at `70^(@)C`, is poured into a cup of mass 0.12 kg . Find the final equilibrium temperature. Take room temperature at `20^(@)C` .
(`s_(coffee) = 4080 J/kg-K and s_(cup) = 1020 J/kg-K`.)

0.3 kg of hot coffee , which is at 70^@C is poured into a cap of mass 0.12 kg. Find the final equilibrium temperature . Take room temperature as 20^(@)C , S_("coffee") = 4080J//kg - K and S_("cup")=1020J//kg - K

1kg ice at -10^(@) is mixed with 1kg water at 50^(@)C . The final equilibrium temperature and mixture content.

1kg ice at -10^(@) is mixed with 1kg water at 50^(@)C . The final equilibrium temperature and mixture content.

2 kg ice at 0^@C is mixed with 8 kg of water at 20^@C . The final temperature is

10 litres of hot water at 70^@C is mixed with an equal volume of cold water at 20^@ C . Find the resultant temperature of the water. (Specific heat of water = 4200 J//kg -K ).

2 kg water at 80^@C is mixed with 3 kg water at 20^@C . Assuming no heat losses, find the final temperature of the mixture

In a mixture of 35 g of ice and 35 g of water in equilibrium, 4 gm steam is passed. The whole mixture is in a copper calorimeter of mass 50 g . Find the equilibrium temperature of the mixture. Given that specific heat of water is 4200 J/kg K and that of copper is 420 J/Kg K and latent heat of fusion of ice is 3.36xx10^(5) J/kg and latent heat of vaporization of water is 2.25xx10^(6) J/kg.

10 litres of hot water at 70^(@) C is mixed with an equal volume of cold water at 20^(@) C. Find the resultant temperature of the water. (Specific heat of water = 4200 j/kg K )