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Social ScienceHow much heat is required to convert solid ice with a mass of 930 g at a temperature of -10.0 °C to liquid water at a temperature of 59.0 °C? The specific heat of ice is cice = 2100 J/kgK, the specific heat of water is cwater = 4186.8 J/kgK, and the heat of fusion for water is Lf = 334 kJ/kg.
How much heat is required to convert solid ice with a mass of 930 g at a temperature of -10.0 °C to liquid water at a temperature of 59.0 °C? The specific heat of ice is cice = 2100 J/kgK, the specific heat of water is cwater = 4186.8 J/kgK, and the heat of fusion for water is Lf = 334 kJ/kg.
Expert Answer
The specific heat capacity for a given chemical substance or a solution refers to the amount of the heat that is required to increase the temperature of a given substance or system per unit of its mass. The mathematical relationship between specific heat capacity, mass, change in temperature and the heat of the solution is given by the following equation:
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q=mxcxAT q is the amount of heat or energy released or absorbed during the reaction m is the mass of the given substance c is the specific heat capacity AT is the change in the temperature of the system
The initial temperature is given to be -10.0 oC = -283.15 K.
The final temperature is given to be 59 oC =332.15 K.
The specific heat capacity of water is given to 4186.8 J kg-1 K-1.
The specific heat capacity of ice is given to 2100 J kg-1 K-1.
The mass of ice is given to be 930 g=0.93 kg.
This conversion takes place by three steps. In first step, the temperature of the ice raises from -10oC to 0.0oC.
In the first step the heat absorbed during the reaction can be calculated as follows:
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mxcxAT ice q=0.93 kgx2100 J/kg Kx(273.15 K-263.15 K) = 19530 J 19.53 kJ
The heat which is absorbed during the melting...
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92mxL q20.93 kgx334 kJ/kg 310.62 kJ
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