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Chapter 51: Problem 1

Explain why \(\Delta H\) is positive for the melting of ice.

Short Answer

Expert verified
The \(\Delta H\) for the melting of ice is positive because it's an endothermic process. During the transition from solid (ice) to liquid (water), heat energy is absorbed from the surroundings to overcome the intermolecular forces of attraction, leading to a positive change in enthalpy.

Step by step solution

01

Understanding Phase Transition

Melting is a type of phase transition where a substance changes from a solid phase to a liquid phase. It is necessary to understand that during phase transitions, the arrangement and movement of particles change.
02

Ice to Water Transformation

In the specific case of ice melting, the ice in the solid state has its water molecules arranged in a highly ordered, rigid structure with hydrogen bonds holding them together. For it to melt into liquid water, enough heat energy must be provided to break these bonds.
03

Enthalpy Change Explanation

This heat absorption causes a positive change in the system's enthalpy (\(\Delta H\)). The energy taken in is used to overcome the forces of attraction between the molecules, enabling them to move more freely in the liquid state. Thus, the \(\Delta H\) for the melting of ice is positive because heat energy needs to be absorbed from the surroundings to transform the solid into a liquid.

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Most popular questions from this chapter

Consider the freezing of water: \(\mathrm{H}_{2} \mathrm{O}(\ell) \rightleftharpoons \mathrm{H}_{2} \mathrm{O}(\mathrm{s})\). a) Will \(\Delta H\) be positive or negative? b) Will \(\Delta S\) be positive or negative? c) Explain your reasoning for both of your answers.

Do you expect \(\Delta S\) to be positive or negative for the melting of ice? Explain your reasoning.

Under what conditions can an endothermic reaction occur naturally? Explain your reasoning.
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