Consider a 27.5g piece of ice at 0.00C.
a) how much heat is required to convert the ice to water that is also 0.00 C?
b) how much heat would be required to warm this water from 0.00 C to 17.50 C?
I don't understand the process of how to go about solving this problem.
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To solve these problems, we will need to apply the principles of heat transfer and phase changes. The specific heat capacity and latent heat of fusion of ice will be used.
a) To calculate the heat required to convert the ice to water at 0.00°C, we need to consider the phase change of ice to water. The heat required for a phase change is given by the equation:
Q = m * ΔH
Where:
Q = heat energy required
m = mass of the substance
ΔH = latent heat of fusion
For ice, the latent heat of fusion is 334 J/g. Therefore, to convert the ice to water at 0.00°C, we can calculate the heat required as follows:
Q = 27.5g * 334 J/g = 9215 J
So, the amount of heat required to convert the ice to water at 0.00°C is 9215 J.
b) To calculate the heat required to warm the water from 0.00°C to 17.50°C, we need to use the equation:
Q = m * c * ΔT
Where:
Q = heat energy required
m = mass of the substance
c = specific heat capacity of the substance
ΔT = change in temperature
For water, the specific heat capacity is approximately 4.18 J/g°C. Therefore, we can calculate the heat required as follows:
Q = 27.5g * 4.18 J/g°C * (17.50°C - 0.00°C) = 1676.575 J
So, the amount of heat required to warm the water from 0.00°C to 17.50°C is approximately 1676.575 J.
To solve these problems, you need to know the latent heat of fusion and specific heat capacity of the substances involved. You can find these values in a physics or chemistry reference book or use online resources.