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.

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.

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.

Find the entropy increment of an aluminium bar of mass m = 3.0 kg on its heating from the temperature T_1 = 300 K up to T_2 = 600 K if in this temperature interval the specific heat capacity of aluminimum varies as c = a + bT , where a = 0.77 J//(g.K), b = 0.46 mJ//(g. k^2) .

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.

One mole of water being in equilibrium with a negligible amount of its saturated vapour at a temperature T_1 was completely converted into saturated vapour at a temperature T_2 . Find the entropy increment of the system. The vapour is assumed to be an ideal gas, the specific volume of the liquid is negligible on comparsion with that of the vapour.

One mole of a Van der Waals gas which had initially the volume V_1 and the temperature T_1 was transferred to the state with the volume V_2 and the temperature T_2 . Find the corresponding entropy increment of the gas, assuming its molar heat capacity C_V to be known.

Water of mass m_(2) = 1 kg is contained in a copper calorimeter of mass m_(1) = 1 kg . Their common temperature t = 10^(@)C . Now a piece of ice of mass m_(2) = 2 kg and temperature is -11^(@)C dropped into the calorimeter. Neglecting any heat loss, the final temperature of system is. [specific heat of copper =0.1 Kcal//kg^(@)C , specific heat of water = 1 Kcal//kg^(@)C , specific heat of ice = 0.5 Kcal//kg^(@)C , latent heat of fusion of ice = 78.7 Kcal//kg ]

Water of mass m_(2) = 1 kg is contained in a copper calorimeter of mass m_(1) = 1 kg . Their common temperature t = 10^(@)C . Now a piece of ice of mass m_(2) = 2 kg and temperature is -11^(@)C dropped into the calorimeter. Neglecting any heat loss, the final temperature of system is. [specific heat of copper =0.1 Kcal//kg^(@)C , specific heat of water = 1 Kcal//kg^(@)C , specific heat of ice = 0.5 Kcal//kg^(@)C , latent heat of fusion of ice = 78.7 Kcal//kg ]