Does anyone know how much heat do I need to convert 95g. of ice at -25 C. to water at 30 C. the heat capacity of H2O(s) is 2.1 J/g*C.
q1 = heat to move ice at -25C to zero C.
q1 = mass ice x specific heat ice x (25)
q2 = heat to melt ice at zero C to liquid water at zero C.
q2 = mass ice x heat fusion.
q3 = heat to move liquid water at zero C to 30C.
q3 = mass water x specific heat water x (Tfinal-Tinitial)
Total heat = q1 + q2 + q3.
To calculate the amount of heat required to convert ice at -25°C to water at 30°C, we need to consider the different steps involved in the process.
Step 1: Determine the heat required to raise the temperature of the ice from -25°C to 0°C.
The heat required can be calculated using the formula:
q = m * c * ΔT
where:
q is the heat (in Joules),
m is the mass of the substance (in grams),
c is the specific heat capacity (in J/g°C), and
ΔT is the change in temperature (in °C).
In this case, the mass (m) is 95g, the specific heat capacity (c) is 2.1 J/g°C, and the change in temperature (ΔT) is (0°C - (-25°C)) = 25°C.
Plugging in these values into the formula, we get:
q1 = 95g * 2.1 J/g°C * 25°C
Step 2: Determine the heat required to convert the ice at 0°C into water at 0°C.
The heat required for this phase change is calculated using the formula:
q2 = m * Lf
where:
q2 is the heat (in Joules),
m is the mass of the substance (in grams), and
Lf is the heat of fusion for water (in J/g).
The heat of fusion for water is 334 J/g.
Plugging in the values, we get:
q2 = 95g * 334 J/g
Step 3: Determine the heat required to raise the temperature of the water from 0°C to 30°C.
Using the first formula again with a change in temperature of (30°C - 0°C) = 30°C, we get:
q3 = 95g * 4.18 J/g°C * 30°C
Step 4: Calculate the total heat required.
To get the total heat required, we need to add up the heat required for each step:
Total heat = q1 + q2 + q3
Now, you can plug the values into the equations and calculate the total heat.