What amount of heat is required to melt 500 g of ice at a temperature of -10 degrees?

Initially, the ice needs to be heated from – 10 ° C to 0 ° C – to the temperature of its melting. And then melt it. The total amount of required heat will consist of two parts – the heat of heating and the heat of fusion.

The amount of heat that needs to be reported to the ice will be determined by the formula – Q load = c * m * (t load – t start), where Q load is the amount of heat required to heat the body, c is the specific heat capacity of the substance (in our case, ice) , m is the body weight, t heat is the temperature to which the body was heated, t start is the initial temperature at which the bodies began to be heated.

(t load – t start) – the temperature difference in our case is 10 ° С.

The specific heat capacity of ice is 2050 J / kg ° C.

500 g of ice means a mass of 0.5 kg.

Substituting the values ​​into the above formula, we get – Q load = (2050 J / kg ° C) * (0.5 kg) * (10 ° C) = 10250 J or 10.25 kJ.

In order to melt ice at the melting temperature, it will be necessary to report the amount of heat, which is determined by the formula – Q melt = λm, where Q melt is the amount of heat required to melt ice, λ is the specific heat of crystallization (melting), m is the mass – Q melt = 330 kJ / kg * 0.5 kg = 165 kJ.

The final answer: the total amount of thermal energy required to melt ice under the given conditions will be – Q = Q load + Q melt – 10.25 kJ + 165 kJ = 175.25 kJ.