Which of the statements A–D is false?

Question

A. Internal energy is a state function, while heat and work are not state functions.
B. If we write “?H = MCP?T”, we are assuming that the heat capacity is constant.
C. If we write “dH = MCPdT”, we are assuming either that the pressure of the system is constant or that enthalpy is independent of pressure.
D. When Q or W is positive, this means that either heat is added to the system (Q> 0 ) or work is done on the system (W> 0), according to the sign convention in this book.
E. None of these are false.

Answer 1

A. Incorrect. This statement is true: Internal energy is a state function, and heat and work are dependent upon the path of the process.
B. Incorrect. This statement is true: dH = MCPdT only integrates to ?H = MCP?T if M and CP are both constant with respect to T.
C. Incorrect. This statement is true: Enthalpy is in general dependent upon both temperature and pressure. If pressure is constant, or if pressure doesn’t influence enthalpy for a specific case (e.g. ideal gases), then the equation for enthalpy simplifies to dH = MCPdT.
D. Incorrect. This statement is true: It is a correct description of the sign convention that was established in Section 1.4.3 of the book.
E. Correct.