given the following info for water specfic heat capacity of ice 2.06j/gdegrees calculate the total quanity of heat evolved when 10.0g of steam is condensed,cooled,and frozen to ice at -50 degrees
See your other post above.
To calculate the total quantity of heat evolved when 10.0g of steam is condensed, cooled, and frozen to ice at -50 degrees, we need to consider the different stages involved in the process and the specific heat capacities of each substance.
Here's how you can calculate it:
1. First, calculate the heat required to condense steam to water:
The heat of condensation for steam is approximately 2260 J/g.
Therefore, the heat required to condense 10.0g of steam is: 10.0g x 2260 J/g = 22600 J.
2. Next, calculate the heat required to cool the water from its boiling point to 0 degrees Celsius:
The specific heat capacity of water is approximately 4.18 J/g°C.
The temperature change is 100 degrees Celsius (from 100°C boiling point to 0°C).
Therefore, the heat required to cool 10.0g of water is: 10.0g x 4.18 J/g°C x 100°C = 4180 J.
3. Finally, calculate the heat required to freeze the water to ice at -50 degrees Celsius:
The specific heat capacity of ice is given as 2.06 J/g°C.
The temperature change is 50 degrees Celsius (from 0°C to -50°C).
Therefore, the heat required to freeze 10.0g of water is: 10.0g x 2.06 J/g°C x 50°C = 1030 J.
To find the total quantity of heat evolved, add up the values from each step:
Total heat evolved = Heat required to condense + Heat required to cool + Heat required to freeze
Total heat evolved = 22600 J + 4180 J + 1030 J = 27810 J
So, the total quantity of heat evolved when 10.0g of steam is condensed, cooled, and frozen to ice at -50 degrees is 27810 J.