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Chapter 7: Problem 18

The enthalpy change for a reaction is a state function and it is an extensive property. Explain.

Short Answer

Expert verified
The enthalpy change for a reaction, denoted by 螖H, is classified as a state function because it depends solely on the initial and final states of a system, and not how the system transitioned from one state to another. This means, irrespective of the path taken during the reaction, the enthalpy change will remain the same as long as the initial and final states are the same. The enthalpy change is also considered an extensive property, as its value is proportional to the quantity of substances involved in the reaction. In other words, if the amount of reactants increases or decreases, the enthalpy change will correspondingly increase or decrease. Thus, enthalpy change exhibits behavior of both a state function and an extensive property.

Step by step solution

01

Definition of a State Function

A state function is a property that depends only on the current state of a system and not on the path taken to reach that state. This means that any changes in its value depend solely on the initial and final states of the system, regardless of how the process occurred.
02

Definition of an Extensive Property

An extensive property is a property that depends on the quantity or size of a substance within the system. Its value is proportional to the amount of substance in the system, which means if we change the amount of substance, the value of the property also changes linearly.
03

Enthalpy Change as a State Function

The enthalpy change for a reaction, denoted by 螖H, is the difference in enthalpy between the products and reactants of a chemical reaction, calculated at constant pressure. Since enthalpy is a state function, its change depends only on the initial and final enthalpy values of the system. This means that 螖H is also a state function, as it merely demonstrates the difference in enthalpy between two states, without depending on the process or pathway by which the reaction took place.
04

Enthalpy Change as an Extensive Property

As mentioned earlier, extensive properties depend on the quantity or size of the substance present in the system. Enthalpy change exhibits this behavior because it is proportional to the amount of reactants involved in the reaction. If we increase the amount of reactants, the enthalpy change will also increase proportionally. This linear relationship shows that enthalpy change is an extensive property. In conclusion, the enthalpy change for a reaction is considered a state function because it depends only on the initial and final states of a system, and not the path between them. It is also an extensive property since its value is proportional to the size or quantity of the substances involved in the reaction.

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Most popular questions from this chapter

The heat capacity of a bomb calorimeter was determined by burning 6.79 g methane (energy of combustion \(=-802 \mathrm{kJ} / \mathrm{mol}\) \(\mathrm{CH}_{4}\)) in the bomb. The temperature changed by \(10.8^{\circ} \mathrm{C}\). a. What is the heat capacity of the bomb? b. \(A 12.6-g\) sample of acetylene, \(C_{2} H_{2},\) produced a temperature increase of \(16.9^{\circ} \mathrm{C}\) in the same calorimeter. What is the energy of combustion of acetylene (in \(\mathrm{kJ} / \mathrm{mol}\) )?

A balloon filled with \(39.1 \mathrm{moles}\) of helium has a volume of \(876 \mathrm{L}\) at \(0.0^{\circ} \mathrm{C}\) and \(1.00 \mathrm{atm}\) pressure. The temperature of the balloon is increased to \(38.0^{\circ} \mathrm{C}\) as it expands to a volume of \(998 \mathrm{L}\), the pressure remaining constant. Calculate \(q, w,\) and \(\Delta E\) for the helium in the balloon. (The molar heat capacity for helium gas is \(20.8 \mathrm{J} /^{\circ} \mathrm{C} \cdot \mathrm{mol}.\))

The enthalpy of combustion of solid carbon to form carbon dioxide is \(-393.7 \mathrm{kJ} / \mathrm{mol}\) carbon, and the enthalpy of combustion of carbon monoxide to form carbon dioxide is \(-283.3 \mathrm{kJ} / \mathrm{mol}\) CO. Use these data to calculate \(\Delta H\) for the reaction $$2 \mathrm{C}(s)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{CO}(g)$$

The bomb calorimeter in Exercise 102 is filled with 987 g water. The initial temperature of the calorimeter contents is \(23.32^{\circ} \mathrm{C} . \mathrm{A}\) \(1.056-\mathrm{g}\) sample of benzoic acid \(\left(\Delta E_{\text {comb }}=-26.42 \mathrm{kJ} / \mathrm{g}\right)\) is combusted in the calorimeter. What is the final temperature of the calorimeter contents?

If the internal energy of a thermodynamic system is increased by \(300 .\) \(\mathrm{J}\) while \(75 \mathrm{J}\) of expansion work is done, how much heat was transferred and in which direction, to or from the system?
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