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Chapter 9: Problem 13

In which of the following states would \(\mathrm{NaCl}\) be electrically conducting: (a) solid, (b) molten (that is, melted), (c) dissolved in water? Explain your answers.

Short Answer

Expert verified
NaCl would be electrically conducting in both the molten state and when dissolved in water. It is not electrically conductive in the solid state as there are no free ions to carry the charge.

Step by step solution

01

Understanding Ionic Compounds

Ionic substances, like NaCl, consist of a lattice of positively and negatively charged ions. These ions, when in their solid state, are fixed in place, thus this form does not have mobile charges to carry the electrical current.
02

Examining Molten State

In the molten or liquid state, the ionic lattice of NaCl breaks down. The ions, both sodium (Na+) and chloride (Cl-), are free to move about within the liquid. Because these ions are now free to migrate, this allows a charge to be carried, and hence, NaCl in this state can conduct electricity.
03

Considering Dissolved State

When NaCl is dissolved in water, the ions again become mobile. The water molecules 'surround' each ion (a process known as hydration), thus allowing them to move freely and carry a charge. Therefore, in this state, NaCl can also conduct electricity.

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Most popular questions from this chapter

Compare the properties of ionic compounds and covalent compounds.

Nitroglycerin, one of the most commonly used explosives, has the structure The decomposition reaction is $$ \begin{array}{r} 4 \mathrm{C}_{3} \mathrm{H}_{5} \mathrm{~N}_{3} \mathrm{O}_{9}(l) \longrightarrow \\ 12 \mathrm{CO}_{2}(g)+10 \mathrm{H}_{2} \mathrm{O}(g)+6 \mathrm{~N}_{2}(g)+\mathrm{O}_{2}(g) \end{array} $$ The explosive action is the result of the heat released and the large increase in gaseous volume. (a) Calculate the \(\Delta H^{\circ}\) for the decomposition of one mole of nitroglycerin using both standard enthalpy of formation values and bond enthalpies. Assume that the two \(\mathrm{O}\) atoms in the \(\mathrm{NO}_{2}\) groups are attached to \(\mathrm{N}\) with one single bond and one double bond. (b) Calculate the combined volume of the gases at STP. (c) Assuming an initial explosion temperature of \(3000 \mathrm{~K}\), estimate the pressure exerted by the gases using the result from (b). (The standard enthalpy of formation of nitroglycerin is \(-371.1 \mathrm{~kJ} / \mathrm{mol} .\) )

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