Which of the following processes must violate the first law of thermodynamic? (There may be more then one ansewer!)

(A) W > 0, Q_int = 0 (B) W > 0, Q _int > 0 (C) W > 0, Q _int ), and ∆E_int

(E) W > 0, Q > 0, and ∆E_int

The correct option is (E).
In accordance to first law of thermodynamics, for a thermodynamic system, in which internal energy is the only type of energy the system may have, the law of conservation of energy may be expressed as
Q + W = ΔE_int
Here Q is the energy transferred (as heat) between the system and environment, W is the work done on (or by) the system and ΔE_int is the change in the internal energy of the system.
By convention we have chosen Q to be positive when heat is transferred into the system and W to be positive when work is done on the system.
In the option (E), W > 0 and Q > 0. If we put this condition in the left hand side of the equation Q + W = ΔE_int, then the right hand side of the equation must be greater than zero (ΔE_int > 0). Thus W > 0, Q > 0, and ΔE_int < 0 must violate the first law of thermodynamics. Therefore option (E) is correct.