Final Answer:
PV work done = 49.81 kJ (as work done is negative, indicating energy released in the reaction). PV work done = -49.81 kJ
Step-by-step explanation:
The PV work done during a chemical reaction can be calculated using the equation W = -PΔV, where P is the pressure and ΔV is the change in volume. Given that the volume change is -70.7 L and the reaction occurs at atmospheric pressure (approximately 1 atm), we can use the formula to find the work done.
W = -PΔV = -(1 atm) × (-70.7 L) = 70.7 L atm. Now, to convert L atm to kilojoules (kJ), we use the conversion factor 1 L atm = 101.3 J, which is equivalent to 0.1013 kJ. Therefore, W = 70.7 L atm × 0.1013 kJ/L atm = -49.81 kJ.
In this reaction, ethylene (C₂H₄) reacts with hydrogen chloride (HCl) to form chloroethane (C₂H₅Cl). Since the question doesn't provide specific details about the reaction, the PV work done is solely determined by the change in volume and the pressure at which the reaction occurs, assuming it's an ideal gas reaction. The negative sign indicates work done on the system, as the volume decreases during the reaction (negative ΔV) at constant pressure.
Understanding the pressure and volume changes in a reaction helps in calculating the work done, which is crucial in understanding the energy changes associated with chemical reactions.
This calculation of PV work helps in assessing the energy changes occurring in a chemical reaction concerning volume alteration, an essential aspect in studying the thermodynamics of chemical processes.