Answer :
Final answer:
The energy needed to condense 0.885 mol of ethanol is approximately 34.17 kJ.multiplying the number of moles (0.885) by the enthalpy of vaporization, we arrive at the total energy required for this process, which amounts to approximately 34.17 kJ.
Explanation:
To find the energy needed to condense ethanol, multiply the number of moles by the enthalpy of vaporization.
The enthalpy of vaporization of ethanol is 38.6 kJ/mol, so for 0.885 mol: 38.6 kJ/mol * 0.885 mol = 34.17 kJ.
The energy required to condense 0.885 mol of ethanol, given an enthalpy of vaporization of 38.6 kJ/mol, can be calculated straightforwardly. Each mole of ethanol requires 38.6 kJ to transition from a gaseous state to a liquid state.
Therefore, by multiplying the number of moles (0.885) by the enthalpy of vaporization, we arrive at the total energy required for this process, which amounts to approximately 34.17 kJ. This energy is essential to facilitate the phase transition from gas to liquid, indicative of the energy transfer associated with the process.
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