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Chapter 6: Problem 12

Explain what is meant by a state function. Give two examples of quantities that are state functions and two that are not.

Short Answer

Expert verified
A State Function is a property of a system that depends only on the system's current state. Examples include Energy, Enthalpy, and Entropy. Non-State Functions, such as Work and Heat, depend on the path taken by the system to go from the initial to the final state.

Step by step solution

01

Define State Function

A State Function is a property of a system that only depends on the current state of the system, not on the way in which the system acquired that state. In other words, it is path independent and it only depends on the initial and final states of the system.
02

Examples of State Functions

Common examples of state functions in thermodynamics include Energy, Enthalpy, and Entropy. They all depend on the state of the system and don't dwindle with the path taken by the system to reach that state.
03

Non-State Function Definition

Non-State Function, also known as Path Function, depends not only on the initial and final states of the system but also on the path taken by the system to get from the initial state to the final state.
04

Examples of Non-State Functions

Work and Heat are common examples of Non-State Function. They are path-dependent and change based on the course taken by the system to reach from initial to final state.

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Most popular questions from this chapter

A 0.1375-g sample of solid magnesium is burned in a constant-volume bomb calorimeter that has a heat capacity of \(3024 \mathrm{~J} /{ }^{\circ} \mathrm{C}\). The temperature increases by \(1.126^{\circ} \mathrm{C} .\) Calculate the heat given off by the burning \(\mathrm{Mg},\) in \(\mathrm{kJ} / \mathrm{g}\) and in \(\mathrm{kJ} / \mathrm{mol} .\)

A quantity of \(2.00 \times 10^{2} \mathrm{~mL}\) of \(0.862 \mathrm{MHCl}\) is mixed with an equal volume of \(0.431 M \mathrm{Ba}(\mathrm{OH})_{2}\) in a constant-pressure calorimeter of negligible heat capacity. The initial temperature of the \(\mathrm{HCl}\) and \(\mathrm{Ba}(\mathrm{OH})_{2}\) solutions is the same at \(20.48^{\circ} \mathrm{C}\), For the process $$\mathrm{H}^{+}(a q)+\mathrm{OH}^{-}(a q) \longrightarrow \mathrm{H}_{2} \mathrm{O}(l)$$ the heat of neutralization is \(-56.2 \mathrm{~kJ} / \mathrm{mol}\). What is the final temperature of the mixed solution?

Consider the dissolution of an ionic compound such as potassium fluoride in water. Break the process into the following steps: separation of the cations and anions in the vapor phase and the hydration of the ions in the aqueous medium. Discuss the energy changes associated with each step. How does the heat of solution of \(\mathrm{KF}\) depend on the relative magnitudes of these two quantities? On what law is the relationship based?

Which of the following does not have \(\Delta H_{\mathrm{f}}^{\circ}=0\) at \(25^{\circ} \mathrm{C} ?\) \(\begin{array}{lllll}\text { He }(g) & \text { Fe }(s) & \text { Cl }(g) & \text { S }_{8}(s) & \text { O }_{2}(g) & \text { Br }_{2}(l)\end{array}\)

Calculate the standard enthalpy change for the reaction $$2 \mathrm{Al}(s)+\mathrm{Fe}_{2} \mathrm{O}_{3}(s) \longrightarrow 2 \mathrm{Fe}(s)+\mathrm{Al}_{2}\mathrm{O}_{3}(s)$$ given that$$\begin{array}{l}2 \mathrm{Al}(s)+\frac{3}{2} \mathrm{O}_{2}(g) \longrightarrow \mathrm{Al}_{2}\mathrm{O}_{3}(s) \\\\\Delta H_{\mathrm{rxn}}^{\circ}=-1669.8 \mathrm{~kJ} / \mathrm{mol} \\ 2 \mathrm{Fe}(s)+\frac{3}{2} \mathrm{O}_{2}(g) \longrightarrow \mathrm{Fe}_{2} \mathrm{O}_{3}(s) \\\\\Delta H_{\mathrm{rxn}}^{\circ}=-822.2 \mathrm{~kJ} / \mathrm{mol}\end{array}$$
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