It took 722kJ of heat to melt a piece of ice taken at a temperature of -10 degrees Celsius. Determine the mass of ice.

Given:

T0 = ​​-10 degrees Celsius – initial ice temperature;

T1 = 0 degrees Celsius – ice melting temperature;

c = 2050 J / (kg * C) – specific heat capacity of ice;

q = 330 kJ / kg = 330,000 J / kg is the specific heat of melting of ice;

Q = 722 kJ = 722000 Joule – the amount of energy expended to melt ice.

It is required to determine m (kilogram) – the mass of ice.

The total amount of energy is equal to the sum of the energy required to heat ice to the melting temperature and the energy to melt:

Q = Qheating + Qmelting;

Q = c * m * (T1 – T0) + q * m;

Q = m * (c * (T1 – T0) + q);

m = Q / ((c * (T1 – T0) + q)) = 722000 / (2050 * (0 + 10) + 330000) =

= 722000 / (20500 + 330000) = 722000/350500 = 2.06 kilograms.

Answer: The mass of ice is 2.06 kilograms.