What are the joules needed to melt 50.0g of ice at 0 degree C and to warm the liquid to 65.0 degree C?
Thank YOu
To find the total amount of energy (in joules) needed to melt the ice and warm the liquid, we need to consider two processes: melting the ice and then heating the resulting liquid.
First, let's calculate the energy required to melt the ice. The heat energy required to melt a substance can be calculated using the formula:
Q = m * ΔHf
Where:
Q is the heat energy in joules,
m is the mass of the substance in grams, and
ΔHf is the heat of fusion for the substance.
The heat of fusion for ice is 334 J/g.
Substituting the given values:
m = 50.0 g
ΔHf = 334 J/g
Q(melt) = m * ΔHf
Q(melt) = 50.0 g * 334 J/g
Now, let's calculate the energy required to heat the liquid. The heat energy required to heat a substance can be calculated using the formula:
Q = m * c * ΔT
Where:
Q is the heat energy in joules,
m is the mass of the substance in grams,
c is the specific heat capacity of the substance,
ΔT is the change in temperature.
The specific heat capacity of water is approximately 4.18 J/g°C.
Substituting the given values:
m = 50.0 g
c = 4.18 J/g°C
ΔT = 65.0°C - 0°C = 65.0°C
Q(heat) = m * c * ΔT
Q(heat) = 50.0 g * 4.18 J/g°C * 65.0°C
To get the total energy, we can add the energy required for melting and the energy required for heating:
Total energy = Q(melt) + Q(heat)
Now, you can calculate the final value by substituting the calculated values into the above equation.