Statement I: Along an adiabatic path with nonzero temperature change, ( m d T ) δ Q = 0 . Statement II: Negative process-specific heat necessarily means negative equilibrium heat capacity at constant volume.

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Statement I: Along an adiabatic path with nonzero temperature change, $\frac{δ Q}{( m d T )} = 0$ . Statement II: Negative process-specific heat necessarily means negative equilibrium heat capacity at constant volume.

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Answer:

Solution:

I true: heat transfer is zero. II false: work can make heat and temperature changes have opposite signs without negative equilibrium Cv. B.

Subject:PhysicsTopic:Heat & ThermoSubtopic:Thermal Expansion

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