As shown here, one type of computer keyboard cleaner contains liquefied 1,1-difluoroethane (C2H4F2), which is a gas at atmospheric pressure. When the nozzle is squeezed, the 1,1-difluoroethane vaporizes out of the nozzle at high pressure, blowing dust out of objects. (d) Given your answers to (a), (b), and (c), do you think the operation of this product depends more on enthalpy or entropy? (a) Based on your experience, is the vaporization a spontaneous process at room temperature?

Verified step by step guidance

1. Step 1: Understand the process of vaporization. Vaporization is the phase transition from liquid to gas. For a process to be spontaneous, the change in Gibbs free energy (\( \Delta G \)) must be negative. The equation \( \Delta G = \Delta H - T\Delta S \) relates Gibbs free energy to enthalpy (\( \Delta H \)) and entropy (\( \Delta S \)).
2. Step 2: Consider the spontaneity of vaporization at room temperature. At room temperature, vaporization is generally spontaneous for many substances, including 1,1-difluoroethane, because the increase in entropy (\( \Delta S \)) when a liquid becomes a gas often outweighs the enthalpy change (\( \Delta H \)).
3. Step 3: Analyze the role of enthalpy (\( \Delta H \)) in the process. Enthalpy change during vaporization is typically positive because energy is required to overcome intermolecular forces in the liquid state. However, this energy input is often offset by the entropy increase.
4. Step 4: Analyze the role of entropy (\( \Delta S \)) in the process. The transition from a more ordered liquid state to a less ordered gaseous state results in a significant increase in entropy, which is a key driver for the spontaneity of vaporization.
5. Step 5: Conclude whether the operation depends more on enthalpy or entropy. Given the significant increase in entropy during vaporization, the process likely depends more on entropy than enthalpy, as the disorder introduced by the gas phase is a major factor in the spontaneity of the process.