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Chapter 9: Problem 31

What is meant by an entbalpy change?

Short Answer

Expert verified
Answer: Enthalpy change is the difference in the total energy of a system before and after a thermodynamic process. It is significant in chemistry because it helps in determining whether a chemical reaction is exothermic (releases energy) or endothermic (absorbs energy). This information is crucial in understanding the behavior of chemical reactions.

Step by step solution

01

Define enthalpy change

Enthalpy (H) is a thermodynamic property that represents the total energy of a system, including its internal energy and work done by the system against external pressure. Enthalpy change (鈭咹) is the difference in enthalpy between the final state and the initial state of a system for any given thermodynamic process.
02

Understand the significance of enthalpy change in chemistry

Enthalpy change is an essential concept in chemistry, particularly in the study of chemical reactions. It helps us to determine whether a reaction is exothermic (releases energy) or endothermic (absorbs energy). In an exothermic reaction, the enthalpy change is negative (鈭咹 < 0), and heat is released to the surroundings. Meanwhile, in an endothermic reaction the enthalpy change is positive (鈭咹 > 0), and heat is absorbed from the surroundings.
03

Derive the equation for enthalpy change

The equation for enthalpy change (鈭咹) can be derived from the definition of enthalpy. Suppose we have a system with initial enthalpy (H1) and it undergoes a thermodynamic process until it reaches its final state with enthalpy (H2). The enthalpy change is given by: 鈭咹 = H2 - H1 Where 鈭咹 represents the enthalpy change, H2 is the final enthalpy, and H1 is the initial enthalpy of the system. In conclusion, enthalpy change is the difference in the total energy of a system before and after a thermodynamic process, which is crucial in understanding the behavior of chemical reactions and determining whether they are exothermic or endothermic.

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Most popular questions from this chapter

Explain the difference between potential energy and kinetic energy in molecules.

Use the following data to sketch a heating curve for one mole of methanol. Start the curve at \(-100^{\circ} \mathrm{C}\) and end it at \(100^{\circ} \mathrm{C}\). $$\begin{array}{ll}\hline \text { Boiling point } & 65^{\circ} \mathrm{C} \\\\\hline \text { Melting point } & -94^{\circ} \mathrm{C} \\\\\hline \text { Heat of vaporization } & 35.3 \mathrm{kJ} / \mathrm{mol} \\\\\hline \text { Heat of fusion }\left(\Delta \mathrm{H}_{\text {fus }}\right) & 3.18 \mathrm{kJ} / \mathrm{mol} \\\\\hline \text { Molar heat capacity }(\ell) & 81.1 \mathrm{J} /\left(\mathrm{mol} \cdot^{\circ} \mathrm{C}\right) \\\\\hline \text { Molar heat capacity }(g) & 43.9 \mathrm{J} /\left(\mathrm{mol} \cdot^{\circ} \mathrm{C}\right) \\\\\hline \text { Molar heat capacity }(\mathrm{s}) & 48.7 \mathrm{J} /\left(\mathrm{mol} \cdot^{\circ} \mathrm{C}\right) \\\\\hline\end{array}$$

Is fuel value or fuel density a more useful measure of energy content of liquid fuels? Explain your answer.

When calculating the enthalpy change for a chemical reaction using bond energies, why is it important that the reactants and products all be gases?

The destruction of the ozone layer by chlorofluorocarbons (CFCs) can be described by the following reactions: $$\begin{aligned}\mathrm{ClO}(g)+\mathrm{O}_{3}(g) & \rightarrow \mathrm{Cl}(g)+2 \mathrm{O}_{2}(g) & \Delta H_{\mathrm{rxn}}^{\circ} &=-29.90 \mathrm{kJ} \\\2 \mathrm{O}_{3}(g) \rightarrow 3 \mathrm{O}_{2}(g) & & \Delta H_{\mathrm{rxn}}^{\circ} &=+24.18 \mathrm{kJ}\end{aligned}$$ Use the preceding \(\Delta H_{\mathrm{rxn}}^{\circ}\) values to determine the value of the standard heat of reaction for this reaction: $$\mathrm{Cl}(g)+\mathrm{O}_{3}(g) \rightarrow \mathrm{ClO}(g)+\mathrm{O}_{2}(g) \quad \Delta H_{\mathrm{rxn}}^{\circ}=?$$
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