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Chapter 6: Problem 4

Liquid water turns to ice. Is this process endothermic or exothermic? Explain what is occurring using the terms system, surroundings, heat, potential energy, and kinetic energy in the discussion.

Short Answer

Expert verified
The process of liquid water turning into ice is an exothermic process, as it releases heat to its surroundings. In this process, the system (liquid water) experiences an increase in potential energy due to more structured and stable hydrogen bonds forming in the ice lattice structure, while its kinetic energy decreases as water molecules slow down and lose energy.

Step by step solution

01

Identify the System and Surroundings

In this exercise, the system is the liquid water that is undergoing the phase change and turning into ice. The surroundings include everything outside the system, such as the container holding the water and the environment in which the process is occurring.
02

Determine Heat Transfer

When liquid water turns into ice, it releases heat to its surroundings. This is because the water molecules slow down and lose energy as they form the more ordered and structured solid ice. This heat transfer to the surroundings is known as an exothermic process.
03

Examine Potential Energy

During this phase change, the potential energy of the system increases. Potential energy refers to the stored energy in a substance based on its position or arrangement. In the case of liquid water turning to ice, the potential energy increases because the water molecules are moving closer together and forming more structured and stable hydrogen bonds in the ice lattice structure compared to the less structured arrangement of liquid water.
04

Examine Kinetic Energy

Kinetic energy refers to the energy of motion. In this process, the kinetic energy of the system decreases as the liquid water turns to ice. This is because the water molecules slow down and lose energy as they move closer together and form more stable bonds in the solid state. The decrease in kinetic energy within the system is partially responsible for the release of heat energy to the surroundings.
05

Endothermic or Exothermic Process

Based on the analysis of heat transfer, potential energy, and kinetic energy, we can conclude that the process of liquid water turning into ice is an exothermic process. This is because the system releases heat to the surroundings, the potential energy increases, and the kinetic energy decreases during the process.

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Most popular questions from this chapter

The enthalpy change for the reaction $$ \mathrm{CH}_{4}(g)+2 \mathrm{O}_{2}(g) \longrightarrow \mathrm{CO}_{2}(g)+2 \mathrm{H}_{2} \mathrm{O}(l) $$ is \(-891 \mathrm{~kJ}\) for the reaction as written. a. What quantity of heat is released for each mole of water formed? b. What quantity of heat is released for each mole of oxygen reacted?

Combustion reactions involve reacting a substance with oxygen. When compounds containing carbon and hydrogen are combusted, carbon dioxide and water are the products. Using the enthalpies of combustion for \(\mathrm{C}_{4} \mathrm{H}_{4}(-2341 \mathrm{~kJ} / \mathrm{mol}), \mathrm{C}_{4} \mathrm{H}_{8}(-2755 \mathrm{~kJ} / \mathrm{mol})\), and \(\mathrm{H}_{2}(-286 \mathrm{~kJ} / \mathrm{mol})\), calculate \(\Delta H\) for the reaction $$ \mathrm{C}_{4} \mathrm{H}_{4}(g)+2 \mathrm{H}_{2}(g) \longrightarrow \mathrm{C}_{4} \mathrm{H}_{8}(g) $$

Assume that \(4.19 \times 10^{6} \mathrm{~kJ}\) of energy is needed to heat a home. If this energy is derived from the combustion of methane \(\left(\mathrm{CH}_{4}\right)\), what volume of methane, measured at STP, must be burned? \(\left(\Delta H_{\text {combustion }}^{\circ}\right.\) for \(\mathrm{CH}_{4}=-891 \mathrm{~kJ} / \mathrm{mol}\) )

Consider the reaction $$ \begin{array}{r} 2 \mathrm{HCl}(a q)+\mathrm{Ba}(\mathrm{OH})_{2}(a q) \longrightarrow \mathrm{BaCl}_{2}(a q)+2 \mathrm{H}_{2} \mathrm{O}(l) \\ \Delta H=-118 \mathrm{~kJ} \end{array} $$ Calculate the heat when \(100.0 \mathrm{~mL}\) of \(0.500 \mathrm{M} \mathrm{HCl}\) is mixed with \(300.0 \mathrm{~mL}\) of \(0.100 \mathrm{M} \mathrm{Ba}(\mathrm{OH})_{2}\). Assuming that the temperature of both solutions was initially \(25.0^{\circ} \mathrm{C}\) and that the final mixture has a mass of \(400.0 \mathrm{~g}\) and a specific heat capacity of \(4.18 \mathrm{~J} /{ }^{\circ} \mathrm{C} \cdot \mathrm{g}\), calculate the final temperature of the mixture.

Consider the following reaction: $$ 2 \mathrm{H}_{2}(\mathrm{~g})+\mathrm{O}_{2}(\mathrm{~g}) \longrightarrow 2 \mathrm{H}_{2} \mathrm{O}(l) \quad \Delta H=-572 \mathrm{~kJ} $$ a. How much heat is evolved for the production of \(1.00 \mathrm{~mol}\) \(\mathrm{H}_{2} \mathrm{O}(l) ?\) b. How much heat is evolved when \(4.03 \mathrm{~g}\) hydrogen is reacted with excess oxygen? c. How much heat is evolved when \(186 \mathrm{~g}\) oxygen is reacted with excess hydrogen? d. The total volume of hydrogen gas needed to fill the Hindenburg was \(2.0 \times 10^{8} \mathrm{~L}\) at \(1.0 \mathrm{~atm}\) and \(25^{\circ} \mathrm{C}\). How much heat was evolved when the Hindenburg exploded, assuming all of the hydrogen reacted?
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