if 180 grams of ice at -123 degrees celsius is heated to steam at 125 degrees celsius, how much energy would it take?
So this in stages.
q1 = heat to raise T of solid ice from -123 to solid ice at zero C.
q1 = mass ice x specific heat ice x (Tfinal-Tinitial)
where Tfinal = 0 and Tinitial = -123.
q2 = heat to melt ice.
q2 = mass ice x heat fusion.
q3. heat to raise T of liquid water from zero C to 100 C.
[mass water x specific heat water x (Tfinal-Tinitial)
q4 = heat to convert liquid water at 100 C to steam at 100 C.
q4 = [mass water x heat vaporization)
q5 = heat to raise T of steam at 100 to steam at 125 C.
q5 = [mass steam x specific heat steam x (Tfinal-Tinitial)]
Total Q = sum individual q values.
q2 =
To calculate the amount of energy required to heat the ice to steam, we need to consider two main steps: heating the ice from its initial temperature to its melting point, and then heating the resulting water to its boiling point and transforming it into steam.
Step 1: Heating the ice
To calculate the energy required to heat the ice from -123 degrees Celsius to its melting point (0 degrees Celsius), we can use the equation:
Q = m * c * ΔT
Where:
Q is the energy in joules,
m is the mass of the ice in grams,
c is the specific heat capacity of ice (2.09 J/g°C), and
ΔT is the change in temperature in degrees Celsius.
Using the equation, the energy required to heat the ice can be calculated as follows:
Q1 = m * c * ΔT
Q1 = 180 g * 2.09 J/g°C * (0 - (-123))°C
Step 2: Melting the ice and heating the water and steam
To calculate the energy required to melt the ice and heat the resulting water and steam, we need to consider the heat of fusion and the specific heat capacity of water and steam.
The heat of fusion (also called the heat of melting) for water is 334 J/g. This represents the amount of energy required to change a substance from a solid to a liquid at the same temperature.
The specific heat capacity of water is 4.18 J/g°C, which represents the amount of energy required to raise the temperature of water by 1 degree Celsius.
The specific heat capacity of steam is 1.99 J/g°C, which represents the amount of energy required to raise the temperature of steam by 1 degree Celsius.
To calculate the energy required to melt the ice and heat the resulting water and steam, we'll consider three separate steps:
1. Heating the ice from its melting point to its boiling point (0°C to 100°C),
2. Melting the ice at its melting point (0°C),
3. Heating the resulting water from its boiling point to the final temperature (100°C to 125°C).
The energy needed for each step can be calculated as follows:
1. Heating the ice:
Q2 = m * c * ΔT
Q2 = 180 g * 4.18 J/g°C * (100 - 0)°C
2. Melting the ice:
Q3 = m * heat of fusion
Q3 = 180 g * 334 J/g
3. Heating the resulting water:
Q4 = m * c * ΔT
Q4 = 180 g * 4.18 J/g°C * (125 - 100)°C
To find the total energy required, sum up the energies from each step:
Total energy = Q1 + Q2 + Q3 + Q4
Now, you can substitute the values into the equations and calculate the total energy required to heat the ice to steam.