A 152g sample of ice at -37 degrees Celsius is heated until it turns into liquid water at 0 degrees Celsius. Find the change in heat content of the system.

I'm really confused on how to solve this question knowing the fact that the state of the system is changing from ice to liquid.

heat the ice to 0ºC

... specific heat of ice?

melt the ice to water at 0ºC
... heat of fusion of ice?

how do I calculate the heat of fusion of ice??

it is a constant ... like specific heat ... look it up

To solve this question, we need to consider the specific heat capacity of ice, the specific heat capacity of water, and the heat of fusion.

First, let's calculate the heat required to raise the temperature of the ice from -37°C to its melting point of 0°C:

Q1 = mass × specific heat capacity (ice) × change in temperature

Given:
mass of ice = 152g
specific heat capacity of ice = 2.09 J/g°C
change in temperature = 0°C - (-37°C) = 37°C

Q1 = 152g × 2.09 J/g°C × 37°C = 11393.84 J

Next, we need to calculate the heat required to melt the ice into water at 0°C. This heat is called the heat of fusion, denoted by the symbol ∆Hf:

Q2 = mass × heat of fusion

Given:
mass of ice = 152g
heat of fusion of water = 334 J/g

Q2 = 152g × 334 J/g = 50848 J

Now, we can calculate the total change in heat content (∆H) of the system by adding the heat required for raising the temperature of ice and the heat required for the phase change:

∆H = Q1 + Q2 = 11393.84 J + 50848 J = 62241.84 J

Therefore, the change in heat content of the system is 62241.84 J.