Asked by reed
Clapeyron equation: dp/dT = ΔS / ΔV
My textbook says, for fusion/melting reactions: dp/dT = ΔH / (T ΔV)
this implies that T * ΔS = ΔH.
I know T * ΔS = q and at constant pressure, that equals H, but the dp/dT reaction is not at constant pressure. Please explain. Thanks!
My textbook says, for fusion/melting reactions: dp/dT = ΔH / (T ΔV)
this implies that T * ΔS = ΔH.
I know T * ΔS = q and at constant pressure, that equals H, but the dp/dT reaction is not at constant pressure. Please explain. Thanks!