Calculate the change in entropy that occurs in the system when 1.00 mole of diethyl ether (C₄H₁₀O) condenses from a gas to a liquid at its normal boiling point (34.6 °C). See Table 11.7 for heats of vaporization.

검증된 단계별 안내

Identify the process: The problem involves the condensation of diethyl ether from gas to liquid at its boiling point.

Recall that the change in entropy (\( \Delta S \)) for a phase change can be calculated using the formula \( \Delta S = \frac{\Delta H_{\text{vap}}}{T} \), where \( \Delta H_{\text{vap}} \) is the heat of vaporization and \( T \) is the temperature in Kelvin.

Convert the given temperature from Celsius to Kelvin by adding 273.15 to the Celsius temperature: \( T = 34.6 + 273.15 \).

Look up the heat of vaporization (\( \Delta H_{\text{vap}} \)) for diethyl ether from Table 11.7. Ensure the units are consistent, typically in Joules per mole (J/mol).

Substitute the values of \( \Delta H_{\text{vap}} \) and \( T \) into the formula \( \Delta S = \frac{\Delta H_{\text{vap}}}{T} \) to find the change in entropy.

비슷한 문제에 대한 검증된 영상 답변:

이 영상 해법은 위 문제에 도움이 된다고 튜터들이 추천한 것입니다.

영상 길이:

주요 개념

질문에 올바르게 답하기 위해 반드시 이해해야 하는 핵심 개념들은 다음과 같습니다.

Entropy

Entropy is a measure of the disorder or randomness in a system. In thermodynamics, it quantifies the amount of energy in a physical system that is not available to do work. When a substance transitions from gas to liquid, such as diethyl ether condensing, the entropy typically decreases because the molecules become more ordered in the liquid state.

Heat of Vaporization

The heat of vaporization is the amount of energy required to convert a unit mass of a substance from liquid to gas at its boiling point. This value is crucial for calculating changes in entropy during phase transitions. For diethyl ether, the heat of vaporization will provide the necessary energy value to determine the entropy change when it condenses.

Phase Change and Temperature

Phase changes, such as condensation, occur at specific temperatures known as boiling or melting points. The normal boiling point of diethyl ether is 34.6 °C, which is the temperature at which it transitions from gas to liquid under standard atmospheric pressure. Understanding the relationship between temperature and phase changes is essential for calculating thermodynamic properties like entropy.

Calculate the change in entropy that occurs in the system when 1.00 mole of diethyl ether (C4H10O) condenses from a gas to a liquid at its normal boiling point (34.6 °C). See Table 11.7 for heats of vaporization.