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Chapter 6: Problem 2

What is meant by the term lower in energy? Which is lower in energy, a mixture of hydrogen and oxygen gases or liquid water? How do you know? Which of the two is more stable? How do you know?

Short Answer

Expert verified
The term "lower in energy" refers to a substance or system with less potential energy compared to another substance or system. In this context, liquid water is lower in energy and more stable than a mixture of hydrogen and oxygen gases, as it is formed through the exothermic reaction 2 H鈧� (g) + O鈧� (g) -> 2 H鈧侽 (l) + energy, where energy is released. According to thermodynamics, substances with lower energy states are more stable, making liquid water more stable than the gas mixture.

Step by step solution

01

Define the term "lower in energy"

The term "lower in energy" refers to a substance or system having less potential energy in comparison to another substance or system. In the context of chemical reactions, lower energy often translates to more stable and less likely to undergo further reactions.
02

Compare liquid water's energy to a mixture of hydrogen and oxygen gases

In this step, we compare the energy states of liquid water and a mixture of hydrogen and oxygen gases. Liquid water results from the combination of hydrogen and oxygen gases in a chemical reaction called the formation of water: 2 H鈧� (g) + O鈧� (g) -> 2 H鈧侽 (l) + energy In this reaction, energy is released when the hydrogen and oxygen gases combine to form liquid water. This means that the energy state of the liquid water is lower than that of the mixture of hydrogen and oxygen gases.
03

Determine stability based on energy states

Now that we have established that liquid water is lower in energy than the mixture of hydrogen and oxygen gases, we can determine which of the two is more stable. According to thermodynamics, substances with lower energy states are more stable than substances with higher energy states. This means liquid water is more stable than the mixture of hydrogen and oxygen gases because it has a lower energy state. In conclusion, the term "lower in energy" means that a substance or system has less potential energy than another substance or system. Liquid water is lower in energy and more stable when compared to a mixture of hydrogen and oxygen gases, as observed in the formation of water reaction.

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Most popular questions from this chapter

Calculate \(\Delta H^{\circ}\) for each of the following reactions using the data in Appendix 4: $$ \begin{array}{c} 4 \mathrm{Na}(s)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{Na}_{2} \mathrm{O}(s) \\ 2 \mathrm{Na}(s)+2 \mathrm{H}_{2} \mathrm{O}(l) \longrightarrow 2 \mathrm{NaOH}(a q)+\mathrm{H}_{2}(g) \\ 2 \mathrm{Na}(s)+\mathrm{CO}_{2}(g) \longrightarrow \mathrm{Na}_{2} \mathrm{O}(s)+\mathrm{CO}(\mathrm{g}) \end{array} $$ Explain why a water or carbon dioxide fire extinguisher might not be effective in putting out a sodium fire.

A sample consisting of \(22.7 \mathrm{~g}\) of a nongaseous, unstable compound \(\mathrm{X}\) is placed inside a metal cylinder with a radius of \(8.00 \mathrm{~cm}\), and a piston is carefully placed on the surface of the compound so that, for all practical purposes, the distance between the bottom of the cylinder and the piston is zero. (A hole in the piston allows trapped air to escape as the piston is placed on the compound; then this hole is plugged so that nothing inside the cylinder can escape.) The piston-and-cylinder apparatus is carefully placed in \(10.00 \mathrm{~kg}\) water at \(25.00^{\circ} \mathrm{C}\). The barometric pressure is 778 torr. When the compound spontaneously decomposes, the piston moves up, the temperature of the water reaches a maximum of \(29.52^{\circ} \mathrm{C}\), and then it gradually decreases as the water loses heat to the surrounding air. The distance between the piston and the bottom of the cylinder, at the maximum temperature, is \(59.8 \mathrm{~cm}\). Chemical analysis shows that the cylinder contains \(0.300 \mathrm{~mol}\) carbon dioxide, \(0.250\) mol liquid water, \(0.025\) mol oxygen gas, and an undetermined amount of a gaseous element \(\mathrm{A}\). It is known that the enthalpy change for the decomposition of \(X\), according to the reaction described above, is \(-1893\) \(\mathrm{kJ} / \mathrm{mol} \mathrm{X}\). The standard enthalpies of formation for gaseous carbon dioxide and liquid water are \(-393.5 \mathrm{~kJ} / \mathrm{mol}\) and \(-286 \mathrm{~kJ} / \mathrm{mol}\), respectively. The heat capacity for water is \(4.184 \mathrm{~J} /{ }^{\circ} \mathrm{C} \cdot \mathrm{g}\). The conversion factor between \(\mathrm{L} \cdot \mathrm{atm}\) and \(\mathrm{J}\) can be determined from the two values for the gas constant \(R\), namely, \(0.08206 \mathrm{~L}\). \(\mathrm{atm} / \mathrm{K} \cdot \mathrm{mol}\) and \(8.3145 \mathrm{~J} / \mathrm{K} \cdot \mathrm{mol}\). The vapor pressure of water at \(29.5^{\circ} \mathrm{C}\) is 31 torr. Assume that the heat capacity of the pistonand-cylinder apparatus is negligible and that the piston has negligible mass. Given the preceding information, determine a. The formula for \(\mathrm{X}\). b. The pressure-volume work (in \(\mathrm{kJ}\) ) for the decomposition of the \(22.7-\mathrm{g}\) sample of \(\mathrm{X}\). c. The molar change in internal energy for the decomposition of \(X\) and the approximate standard enthalpy of formation for \(X\).

The enthalpy of combustion of solid carbon to form carbon dioxide is \(-393.7 \mathrm{~kJ} / \mathrm{mol}\) carbon, and the enthalpy of combustion of carbon monoxide to form carbon dioxide is \(-283.3 \mathrm{~kJ} / \mathrm{mol}\) CO. Use these data to calculate \(\Delta H\) for the reaction $$ 2 \mathrm{C}(s)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{CO}(g) $$

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?

If the internal energy of a thermodynamic system is increased by \(300 .\) J while \(75 \mathrm{~J}\) of expansion work is done, how much heat was transferred and in which direction, to or from the system?
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