To calculate the energy required to change a 20-g ice cube from ice at 0°C to steam at 140°C, you need to consider the phases and their specific heat capacities. Calculate the energy required to heat the ice, melt the ice, heat the water, vaporize the water, and heat the steam. Add up all the energies to get the total energy required.
Step-by-step explanation:
To calculate the energy required to change a 20-g ice cube from ice at 0°C to steam at 140°C, we need to consider the different phases and their specific heat capacities. The energy can be calculated using the following steps:
Energy required to heat the ice from -20°C to 0°C: Q = mcΔT, where m = mass of ice, c = specific heat capacity of ice, and ΔT = change in temperature. Assume the specific heat capacity of ice to be 2.06 J/g°C.
Energy required to melt the ice at 0°C: Q = mLf, where m = mass of ice and Lf = latent heat of fusion. The latent heat of fusion for ice is 334 J/g.
Energy required to heat the water from 0°C to 100°C: Q = mcΔT, where m = mass of water, c = specific heat capacity of water, and ΔT = change in temperature. Assume the specific heat capacity of water to be 4.18 J/g°C.
Energy required to vaporize the water at 100°C: Q = mLv, where m = mass of water and Lv = latent heat of vaporization. The latent heat of vaporization for water is 2260 J/g.
Energy required to heat the steam from 100°C to 140°C: Q = mcΔT, where m = mass of steam, c = specific heat capacity of steam, and ΔT = change in temperature. Assume the specific heat capacity of steam to be 2.03 J/g°C.
Now, plug in the values and calculate the energy required for each step. Add up all the energies to get the total energy required.