A piece of copper of mass `m = 90 g` at a temperature `t_1 = 90 ^@C` was placed in a calorimeter in which ice of mass `50 g` was at a temperature `-3 ^@C`. Find the entropy increment of the piece of copper by the moment the thermal equilibrium is reached.

A piece of copper of mass m_1 = 300 g with initial temperature t_1 = 97 ^@C is placed into a calorimeter in which the water of mass m_2 = 100 g is at a temperature t_2 = 7 ^@ C . Find the entropy increment of the system by the moment the temperature t_2 = 7 ^@ C . FInd the entropy increment of the system by the moment the temperatures equalize. The heat capacity of the calorimeter itself is negligibly small.

Water of mass m = 1.00 kg is heated from the temperature t_1 = 10^@C up to t_2 = 100 ^@C at which it evaporated completely. Find the entropy increment of the system.

The ice with the initial temperature t_1 = 0 ^@C was first melted, then heated to the temperature t_2 = 100^@C and evaporated. Find the increment of the system's specific entropy.

A piece of metal of mass 112 g is heated to 100^@ C and dropped into a copper calorimeter of mass 40 g containing 200 g of water at 16^@ C . Neglecting heat loss, the specific heat of the metal is nearly, if the equilibrium temperature reached is 24^@ C . (S_(cu) = 0.1 cal//g-.^(@) C) .

50 g ice at 0^(@)C is dropped into a calorimeter containing 100 g water at 30^(@)C . If thermal . capacity of calorimeter is zero then amount of ice left in the mixture at equilibrium is

50 g ice at 0^(@)C is dropped into a calorimeter containing 100 g water at 30^(@)C . If thermal . capacity of calorimeter is zero then amount of ice left in the mixture at equilibrium is