How much heat is required to turn 500 grams of ice at a temperature of 4 degrees

How much heat is required to turn 500 grams of ice at a temperature of 4 degrees into water with a temperature of 0 degrees?

1). Before the ice begins to melt, it must be heated to the melting point of the ice, that is, to 0 degrees Celsius. In order to calculate how much heat the ice should receive when heated from a temperature of – 4 degrees to a temperature of 0 degrees, we will use the formula: Q = m • c • Δt. Ice mass m = 500 g = 0.5 kg. Specific heat capacity of ice c = 2100 J / (kg • deg), temperature change Δt = 0 – (- 4); Δt = 4 degrees. We get Q = 0.5 kg • 2100 J / (kg • deg) • 4 deg, Q = 4200 J.
2). To calculate how much heat the ice must receive in order to turn into a liquid state, we will use the formula Q = λ • m, where the specific heat of melting of ice λ = 0.34 MJ / kg. We substitute the values ​​of physical quantities: Q = 0.5 kg • 340,000 J / kg = 170,000 J.
3). Let’s find how much energy is required for both processes. Q = 4200 J + 170,000 J = 174200 J.
Answer: 174200 Joules of energy is needed to turn this ice into a liquid state.