Find the amount of heat required to convert 10g of ice to steam at 110 degree Celsius.
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To find the amount of heat required to convert a substance from one phase to another, you need to consider the heat absorbed or released during each phase change and the heat required to raise the temperature within the phase.
In this case, we have three phases: ice, water, and steam.
1. First, calculate the heat required to raise the temperature of the ice from its initial temperature, which is below 0°C, to 0°C. The specific heat capacity of ice is 2.09 J/g°C. Since we have 10g of ice, the heat required can be calculated as follows:
Heat = mass * specific heat capacity * temperature difference
Heat = 10g * 2.09 J/g°C * (0°C - (-10°C)) = 209 J
2. Next, calculate the heat required to melt the ice at 0°C into water at 0°C. The heat of fusion for ice is 334 J/g. The formula to calculate the heat required is:
Heat = mass * heat of fusion
Heat = 10g * 334 J/g = 3340 J
3. Now, calculate the heat required to raise the temperature of the water from 0°C to the boiling point of water, which is 100°C. Water has a specific heat capacity of 4.18 J/g°C. The formula to calculate the heat required is:
Heat = mass * specific heat capacity * temperature difference
Heat = 10g * 4.18 J/g°C * (100°C - 0°C) = 4180 J
4. Lastly, calculate the heat required to vaporize the water at 100°C into steam at 110°C. The heat of vaporization for water is 2260 J/g. The formula to calculate the heat required is:
Heat = mass * heat of vaporization
Heat = 10g * 2260 J/g = 22600 J
Now, we add up all the heats from the different steps to get the total heat required:
Total heat = Heat (raising temperature of ice) + Heat (melting ice) + Heat (raising temperature of water) + Heat (vaporizing water)
Total heat = 209 J + 3340 J + 4180 J + 22600 J = 30429 J
Therefore, the amount of heat required to convert 10g of ice to steam at 110°C is 30429 J.