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Chapter 32: Problem 4

The net attractive potential energy in Figure 2 is \(-6.93 \times 10^{-18} \mathrm{~J}\). Will energy be required to separate the nuclei or will energy be released upon separation? Explain.

Short Answer

Expert verified
Energy will be required to separate the nuclei.

Step by step solution

01

Identify Potential Energy

Firstly, identify the potential energy given in the problem. Here, the net attractive potential energy is stated as \(-6.93 \times 10^{-18} \mathrm{~J}\). The negative sign indicates that it's a bound state.
02

Understand the Meaning of Negative Potential Energy

Negative potential energy suggests that the system is already in a low energy state and it takes effort to disrupt this state. Thus, energy must be provided to break it apart.
03

Apply the Concept to the Problem

Applying the above understanding to the problem at hand, it can be concluded that energy is required to separate the nuclei. The energy needed would be used to overcome the attractive force between the nuclei. It will not be released but it must be supplied.

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Most popular questions from this chapter

For molecules, why are all of the values for enthalpies of atom combination negative?

Why is \(\Delta H_{\mathrm{ac}}^{\circ}\) of \(\mathrm{C}(\mathrm{g})=0 ?\) Why is \(\Delta H_{\mathrm{ac}}^{\circ}\) of \(\mathrm{H}(\mathrm{g})=0\) ?

What is the value of \(\Delta H^{\circ}\) for the overall process of separating one mole of \(\mathrm{CH}_{4}\) into its constituent atoms, and then reforming one mole of \(\mathrm{CH}_{4}\) ?

Is the enthalpy of atom combination for \(\mathrm{CH}_{4}(\mathrm{~g})\) exothermic or endothermic?

a) Draw the Lewis structures for \(\mathrm{N}_{2}\) and \(\mathrm{O}_{2}\). b) Explain how these Lewis structures are consistent with the relative enthalpies of atom combination for \(\mathrm{N}_{2}(\mathrm{~g})\) and \(\mathrm{O}_{2}(\mathrm{~g})\).
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