find the heat of fusion of ice
M copper calorimeter= 50 g
M h20 200 g at 30 C
M ice=20.45 at 0 C
t2= 20C
To find the heat of fusion of ice, you can use 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 (in J/g°C), and
ΔT is the change in temperature (in °C).
In this case, we'll need to consider three steps: heating the ice from 0°C to 0°C, melting the ice at 0°C, and heating the resulting water from 0°C to 20°C. Let's look at each step separately:
1. Heating the ice from 0°C to 0°C:
Since there is no change in temperature, ΔT will be 0. Therefore, the heat energy required for this step will be 0.
2. Melting the ice at 0°C:
To calculate the heat energy required for this step, we need to use the formula:
Q = m × ΔHf
Where:
Q is the heat energy (in joules),
m is the mass of the ice (in grams), and
ΔHf is the heat of fusion of ice (in J/g).
We are given that the mass of the ice (m) is 20.45 g. However, we don't have the value for the heat of fusion (ΔHf) of ice. The heat of fusion of ice is approximately 334 J/g. You can find this value from reference materials or textbooks.
3. Heating the resulting water from 0°C to 20°C:
We can now calculate the heat energy required for this step using the formula mentioned earlier:
Q = m × C × ΔT
Given:
m = mass of water = 200 g
C = specific heat capacity of water = 4.18 J/g°C (approximately; this is a commonly used value for the specific heat of water)
ΔT = change in temperature = final temperature (t2) - initial temperature (0°C)
ΔT = 20°C - 0°C = 20°C
Now, calculate the heat energy for this step.
Finally, to find the total heat energy required, sum the heat energies from each step:
Total Q = Q (heating ice from 0°C to 0°C) + Q (melting ice at 0°C) + Q (heating water from 0°C to 20°C)
Note: Please make sure to check the correctness of the values and units provided in the question and use appropriate formulas accordingly.