calculate the amount of energy required to convert 55.0g of ice at -10.0°c into steam at 125°c?
Two formulas you need.
Within a phase:
mass x specific heat x (Tfinal-Tinitial). For example: water from zero C to 100 C as a liquid it will be
grams H2O x 4.184 x (100-0) = q
At a phase change:
melting point phase change is
q = mass ice x heat fusion.
boiling point phase change is
q = mass water x heat vaporization.
Then all all of the qs together.
169713.5 joules or 40562.5 calories
169,713.5 joules or 40562.5 calories
To calculate the amount of energy required to convert ice at -10.0°C into steam at 125°C, we need to consider several steps in the process of phase change.
First, we need to calculate the energy required to raise the temperature of the ice from -10.0°C to its melting point, which is 0°C. We use the formula:
q1 = mass × specific heat capacity × temperature change
The specific heat capacity of ice is 2.09 J/g°C. So, the energy required to heat the ice is:
q1 = 55.0g × 2.09 J/g°C × (0.0 - (-10.0))°C
Next, we need to calculate the energy required to melt the ice at 0°C into water at 0°C. The energy required for this phase change is given by:
q2 = heat of fusion × mass
The heat of fusion for ice is 334 J/g. Therefore, the energy required to melt the ice is:
q2 = 334 J/g × 55.0 g
Once the ice is completely melted, we need to calculate the energy required to raise the temperature of water from 0°C to its boiling point, which is 100°C. The specific heat capacity of water is 4.18 J/g°C. Thus, the energy required to heat the water is:
q3 = 55.0g × 4.18 J/g°C × (100.0 - 0.0)°C
Finally, we need to calculate the energy required for the phase change from water at 100°C to steam at 125°C. The heat of vaporization for water is 2260 J/g. Hence, the energy required for this phase change is:
q4 = heat of vaporization × mass
q4 = 2260 J/g × 55.0 g
To find the total energy required for the entire process, we sum up all the heat values:
Total energy required = q1 + q2 + q3 + q4
Calculate each of the above expressions and add them up to find the total energy required to convert 55.0g of ice at -10.0°C into steam at 125°C.