Suppose 4 grams of ethyl alcohol evaporates through an isobaric process at atmospheric pressure (P=1.013e2 kPa). It's volume in the liquid state is 5mL and it's volume in the gaseous state is 2L. The process' initial state is when evaporation begins. The process' final state is when evaporation is complete. Ignore complexities in this process (such as mixing of the alcohol vapor with the air) and use only what you've learned in class. Remember the SI unit for volume is m? Substance Water Ethyl Alcohol Oxygen Sulfur Specific Heat Ji(kg) 4186 2400 920 732 Temp of Latent Heat of vaporization (K0 Vaporization (J/kg) 373.15 2.26E+06 351.15 8.54E+05 90.18 2.13E+05 717.75 3.26E+05 Temp of fusion (K) 273.15 159.15 54.36 392.15 Latent Heat of Fusion (Jika) 3.33E+05 1.04E+05 1.38E+04 3.81E+04 (1) A thermodynamic state is fully defined by two state variables. What is the volume and the temperature at the initial state? (ii) What is the volume and temperature at the final state? (iii) Calculate the work done on the system in Joules as the ethyl alcohol evaporates isobarically *Note: in our convention positive work or heat will imply that energy was given to the system by its surroundings: negative work or heat implies that the system gave energy to its surroundings. (iv) Calculate the energy by heat transferred into the system in Joules during vaporization. (V) Use the 1st law of thermodynamics to calculate the change in internal energy of the system during this process in Joules