How much heat is needed to melt 14.3kg of silver that is initially at 44°C?
Google the specific heat of silver:
0.2386476 J/gC
Convert kg to g:
14.3 kg = 14300 g
Google the melting point of silver:
961.8 C
Thus the required temperature change is 961.8 - 44 = 921.8 C
0.2386476 J/gC x 14300 g x 921.8 C
= _______ J of heat
To determine how much heat is needed to melt 14.3 kg of silver initially at 44°C, we need to consider the specific heat capacity of silver and the heat of fusion.
1. Find the specific heat capacity of silver:
The specific heat capacity (C) is the amount of heat energy required to raise the temperature of a substance by 1 degree Celsius per unit mass. The specific heat capacity of silver is 0.235 J/g°C.
2. Calculate the temperature change:
Since we want to melt the silver, we need to raise its temperature from 44°C to its melting point. The melting point of silver is 961.8°C. Therefore, the temperature change (∆T) is 961.8°C - 44°C = 917.8°C.
3. Calculate the heat required to raise the temperature:
The formula to calculate the heat energy (Q) required to raise the temperature of a substance is Q = m * C * ∆T, where:
- Q is the heat energy in joules
- m is the mass of the substance in kilograms
- C is the specific heat capacity of the substance in J/g°C
- ∆T is the temperature change in degrees Celsius
Converting 14.3 kg to grams, we have m = 14,300 g.
Plugging the values into the formula:
Q = (14,300 g) * (0.235 J/g°C) * (917.8°C)
Q = 3,034,629 Joules
Therefore, approximately 3,034,629 Joules of heat energy is needed to melt 14.3 kg of silver initially at 44°C.