To find the total amount of heat required for this process, we will break the process into three parts: heating the ice from -15°C to 0°C, melting the ice at 0°C, and heating the resulting water from 0°C to 115°C.
1. Heating the ice from -15°C to 0°C:
To calculate the heat required for this process, we'll use the formula Q = mcΔT, where Q is the heat, m is the mass of the ice, c is the specific heat of the ice, and ΔT is the change in temperature. The specific heat of ice is 2100 J/(kg·°C).
Q1 = (0.200 kg) * (2100 J/(kg·°C)) * (0 - -15°C)
Q1 = 0.200 * 2100 * 15
Q1 = 6300 J
2. Melting the ice at 0°C:
To melt the ice, we'll use the formula Q = mL, where L is the latent heat of fusion for ice. The latent heat of fusion for ice is 334,000 J/kg.
Q2 = (0.200 kg) * (334,000 J/kg)
Q2 = 66800 J
3. Heating the resulting water from 0°C to 115°C:
Now that the ice is melted, we'll use the equation Q = mcΔT once again, but this time using the specific heat of water, which is 4186 J/(kg·°C).
Q3 = (0.200 kg) * (4186 J/(kg·°C)) * (115 - 0°C)
Q3 = 0.200 * 4186 * 115
Q3 = 96394 J
Finally, to find the total amount of heat required, we add the heat from each step:
Total = Q1 + Q2 + Q3
Total = 6300 J + 66800 J + 96394 J
Total = 169494 J
The total amount of heat required for this process is 169,494 J.
A 0.200 kg block of ice at -15 degrees Celsius is placed into a pan on a stove, heated to a liquid, and then to vapour with a final temperature of 115 degrees Celsius. Calculate the total amount of heat required for this process.
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