They took 4 kg of ice at a temperature of -20 ° C and turned it into water

They took 4 kg of ice at a temperature of -20 ° C and turned it into water with a temperature of 0 ° C. How much heat was absorbed in this case?

Given:

m = 4 kilograms – ice mass;

T0 = ​​-20 degrees Celsius – initial ice temperature;

c = 2100 J / (kg * C) – specific heat capacity of ice;

T = 0 degrees Celsius – ice melting point;

q = 330000 Joule / kilogram – specific heat of ice melting.

It is required to determine Q (Joule) – the amount of heat required to transform ice into water.

Let us find the amount of heat required to heat the ice to the melting point:

Q1 = c * m * (T – T0) = 2100 * 4 * (0 + 20) = 8400 * 20 = 168000 Joules.

Let’s find the amount of heat needed to melt the ice:

Q2 = q * m = 330,000 * 4 = 1,320,000 Joules.

Total heat needed:

Q = Q1 + Q2 = 168000 + 1320000 = 1488000 Joules = 1.488 MJ.

Answer: heat will be consumed, equal to 1.488 MJ.