**Question:**How much energy must be transferred as heat for a reversible isothermal expansion of an ideal gas at 132°C if the entropy of the gas increases by 46.0 J/K?**Explanation:**In an isothermal process, the temperature remains constant. To find the energy transferred as heat (Q), when the entropy (ΔS) increases, we use the relationship for reversible processes:\[ Q = T \times \Delta S \]Where:- \( T \) is the absolute temperature in Kelvin (K).- \( \Delta S \) is the change in entropy.Convert the temperature from °C to K:\[ T(K) = 132 + 273.15 = 405.15 \, K \]Given:- \( \Delta S = 46.0 \, J/K \)Substituting the values:\[ Q = 405.15 \, K \times 46.0 \, J/K \]Calculate to find the energy transferred as heat.

Temperature (T) = 132oC Process = Isothermal Change in entropy = +46 JK

Answered: How much energy must be transferred as…

College Physics

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How much energy must be transferred as heat for a reversible isothermal expansion J. of an ideal gas at 132°C if the entropy of the gas increases by 46.0 K