Question

Which one of the following statements is true?
a. The enthalpy change for a reaction is independent of the state of the reactants and products.
b. Enthalpy is an intensive property.
c. Enthalpy is a state function.
d. H is the value of q measured under conditions of constant volume.
e. The enthalpy change of a reaction is the reciprocal of the ΔH of the reverse reaction.

Answer 1

Answer: Option (c) is the correct answer.

Explanation:

A state function is defined as the function of a system which relates to several state variables that depend only on the current equilibrium state of the system.

A state function does not depend on the path followed by the system to reach at its present state.

Enthalpy change is represented by $\Delta H$ and its value depends on state functions like U, P and V. Therefore, change in enthalpy is also a state function.

Value of these functions does not depend on the path taken to reach their values.

Therefore, we can conclude that the statement enthalpy is a state function, is true.

Answer 2

The statement about enthalpy which is considered to be true is: C. Enthalpy is a state function.

An enthalpy can be defined as a thermodynamic quantity that gives the total heat content of a system.

Basically, enthalpy is the total sum of the internal energy of a system and the product of its volume and pressure.

Mathematically, enthalpy is given by the formula:

$H = U + PV$

Where:

• H is the enthalpy.

• U is the internal energy.

• P is the pressure.

• V is the volume.

The above parameters are all state functions because their value is highly dependent on the state of a system.

This ultimately implies that, enthalpy is a state function because its parameters (U, P and V) are all determined by the state of a system.

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