A 100.0 g sample of ice at -15°C is heated until it is converted to water vapour at 120.0°C.
Calculate the total energy change.
Sum of the all steps it will show the total number of calories
To calculate the total energy change, we need to consider the three stages of energy transfer that occur during this process:
1. Heating the ice from -15°C to 0°C: To determine this energy change, we'll use the formula Q = mcΔT, where Q is the heat energy, m is the mass, c is the specific heat capacity, and ΔT is the change in temperature. The specific heat capacity of ice is 2.09 J/g°C.
So, the energy change for this stage is Q1 = (mass of ice)(specific heat capacity of ice)(change in temperature).
Q1 = (100.0 g)(2.09 J/g°C)(0 - (-15)°C).
2. Melting the ice at 0°C: The energy required to change a substance from a solid to a liquid, at its melting point, is given by the formula Q = mL, where Q is the heat energy, m is the mass, and L is the latent heat of fusion. The latent heat of fusion for ice is 334 J/g.
So, the energy change for this stage is Q2 = (mass of ice)(latent heat of fusion of ice).
Q2 = (100.0 g)(334 J/g).
3. Heating the water from 0°C to 100°C: For this stage, we'll use the same formula as in stage 1, but now we'll use the specific heat capacity of water, which is 4.18 J/g°C.
So, the energy change for this stage is Q3 = (mass of water)(specific heat capacity of water)(change in temperature).
Q3 = (mass of water)(4.18 J/g°C)(100 - 0)°C.
Note: At 100°C, the water changes its state to steam (water vapor). We assume that all the water is vaporized at 100°C.
4. Heating the water vapor from 100°C to 120.0°C: Again, we'll use the formula from stage 1, but now we'll use the specific heat capacity of steam, which is 2.03 J/g°C.
So, the energy change for this stage is Q4 = (mass of water vapor)(specific heat capacity of steam)(change in temperature).
Q4 = (mass of water vapor)(2.03 J/g°C)(120 - 100)°C.
Finally, we can calculate the total energy change by summing up the energy changes from each stage:
Total energy change = Q1 + Q2 + Q3 + Q4
Now, you can substitute the respective values into the formulas and calculate the total energy change.
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I honestly have no idea how to do this. Could you show me the first part step by step
You do this in steps.
q1 = heat to raise T of solid ice at -15 C to zero C.
q2 = heat to melt ice
q3 = heat to raise T of liquid H2O from zero C to 100 C
q4 = heat to vaporize liquid H2O at 100 C to steam at 100 c.
q5 = heat to raise T of steam from 100 c to 120 C.
Total is sum of each step.
Do what you know to do and post your work if you have question. Explain what trouble your are having.