Which of the following is/are true in the case of an adiabatic process
`q=W`
`Delta U=q`
`q=0`
`Delta U=W`

In which of the following Delta H = Delta U ?

For which of the following change Delta H!=Delta U ?

Which of the following processes must violate the first law of thermodynamics (Q=W+DeltaE_(int) )?

In a reversible adiabatic change Delta Q is

Which of the following are path functions (A) W (B) Q (C) Q+W (D) H-TS

Which of the following are path functions (A) W (B) Q (C) Q+W (D) H-TS

An ideal gas is undergoing a cyclic thermodynamic process in different ways as shown in the corresponding P-V diagrams in column 3 of the table. Consider only the path from state 1 to state 2. W denotes the corresponding work done on the system. The equations and plots in the table have standard notations as used in thermodynamic process. Here is the ratio of heat capacities at constant pressure and constant volume. The number of moles in the gas in n. Which of the following options is the only correct representation of a process in which Delta U = Delta Q - P Delta V ?

Which of the following are not state functions? (I) q+w (II) q (III) w (IV) H-TS

Which of the following are not state functions? (I) q+w (II) q (III) w (IV) H-TS