How much heat is added to a 10.0 g of ice at -20.0 degrees Celsius to convert it to steam at 120.0 degrees Celsius?
compute and add the following heats:
heat to heat ice from -20C to 0C
heat to melt ice at 0C
Heat to heat water from 0 to 100C
heat to convert water to steam at 100C
heat to heat steam from 100 to 120C
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How much heat is added to 10.0 g of ice at negative 20 degrees Celsius to convert it to steam at 120 degrees celsius
A metal block absorbs 4500 cal of heat when heated from 30degree C to 80 degree C .its thermal capacity is
To calculate the total heat added, you need to calculate and sum the individual heats for each step of the process:
1. Heat to heat ice from -20°C to 0°C:
The specific heat capacity of ice is 2.09 J/g°C. Therefore, you can calculate the heat using the formula Q = m * c * ΔT, where Q is the heat, m is the mass, c is the specific heat capacity, and ΔT is the change in temperature. In this case, the mass (m) is 10.0 g, the specific heat capacity (c) is 2.09 J/g°C, and the change in temperature (ΔT) is (0 - (-20)) = 20°C.
Therefore, the heat for this step is Q1 = 10.0 g * 2.09 J/g°C * 20°C.
2. Heat to melt ice at 0°C:
The heat required to melt ice is called the heat of fusion. For water, the heat of fusion is 334 J/g.
The heat (Q2) required to melt the ice is Q2 = 10.0 g * 334 J/g.
3. Heat to heat water from 0°C to 100°C:
The specific heat capacity of liquid water is 4.18 J/g°C. To calculate the heat required, use the same formula as before: Q = m * c * ΔT. The mass (m) remains 10.0 g, the specific heat capacity (c) is 4.18 J/g°C, and the change in temperature (ΔT) is 100°C.
Therefore, the heat (Q3) for this step is Q3 = 10.0 g * 4.18 J/g°C * 100°C.
4. Heat to convert water to steam at 100°C:
The heat required to convert water to steam is called the heat of vaporization. For water, the heat of vaporization is 2260 J/g.
The heat (Q4) required to convert the water to steam is Q4 = 10.0 g * 2260 J/g.
5. Heat to heat steam from 100°C to 120°C:
The specific heat capacity of steam is 2.03 J/g°C. To calculate the heat required, use the same formula: Q = m * c * ΔT. The mass (m) remains 10.0 g, the specific heat capacity (c) is 2.03 J/g°C, and the change in temperature (ΔT) is (120 - 100) = 20°C.
Therefore, the heat (Q5) for this step is Q5 = 10.0 g * 2.03 J/g°C * 20°C.
Finally, to find the total heat added, add up all the heat values calculated from the previous steps:
Total heat added = Q1 + Q2 + Q3 + Q4 + Q5.
Simply substitute the previously calculated values into the equation to find the answer.