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Chapter 5: Problem 39

Consider the following reaction, which occurs at room temperature and pressure: $$ 2 \mathrm{Cl}(g) \longrightarrow \mathrm{Cl}_{2}(g) \quad \Delta H=-243.4 \mathrm{~kJ} $$ Which has the higher enthalpy under these conditions, \(2 \mathrm{Cl}(g)\) or \(\mathrm{Cl}_{2}(g) ?\)

Short Answer

Expert verified
Under the given conditions, 2 Cl(g) has a higher enthalpy than Cl鈧�(g), as the reaction is exothermic with a 鈭咹 of -243.4 kJ.

Step by step solution

01

Understand the given reaction and enthalpy change

The reaction we are dealing with is: \( 2 \,\mathrm{Cl}(g) \longrightarrow \mathrm{Cl}_{2}(g)\), where 鈭咹 = -243.4 kJ. A negative value of 鈭咹 indicates that the reaction is exothermic, meaning that energy is released as the reaction occurs.
02

Relate the enthalpy change to the reactants and products

Let's use the given enthalpy change to relate the enthalpy of the reactants and products. For an exothermic reaction, the enthalpy of the products is lower than the enthalpy of the reactants. Mathematically, we can express this as: Enthalpy of reactants - Enthalpy of products = 鈭咹
03

Determine which species has the higher enthalpy

Since the reaction is exothermic, the enthalpy of the reactants (2 Cl(g)) is higher than the enthalpy of the products (Cl鈧�(g)). Therefore, under these conditions, 2 Cl(g) has higher enthalpy than Cl鈧�(g).

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Most popular questions from this chapter

For each of the following compounds, write a balanced thermochemical equation depicting the formation of one mole of the compound from its elements in their standard states and use Appendix \(C\) to obtain the value of \(\Delta H_{f}^{\circ}:\) (a) \(\mathrm{NH}_{3}(g)\), (b) \(\mathrm{SO}_{2}(g)\) (c) \(\mathrm{RbClO}_{3}(s)\) (d) \(\mathrm{NH}_{4} \mathrm{NO}_{3}(s)\).

A \(1.800-g\) sample of phenol \(\left(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{OH}\right)\) was burned in a bomb calorimeter whose total heat capacity is \(11.66 \mathrm{~kJ} /{ }^{\circ} \mathrm{C}\). The temperature of the calorimeter plus contents increased from \(21.36^{\circ} \mathrm{C}\) to \(26.37^{\circ} \mathrm{C}\). (a) Write a balanced chemical equation for the bomb calorimeter reaction. (b) What is the heat of combustion per gram of phenol? Per mole of phenol?

Suppose you toss a tennis ball upward. (a) Does the kinetic energy of the ball increase or decrease as it moves higher? (b) What happens to the potential energy of the ball as it moves higher? (c) If the same amount of energy were imparted to a ball the same size as a tennis ball, but of twice the mass, how high would it go in comparison to the tennis ball? Explain your answers.

From the following data for three prospective fuels, calculate which could provide the most energy per unit volume:$$ \begin{array}{lcc} & \begin{array}{c} \text { Density } \\ \text { at } 20^{\circ} \mathrm{C} \\ \left(\mathrm{g} / \mathrm{cm}^{3}\right) \end{array} & \begin{array}{c} \text { Molar Enthalpy } \\ \text { of Combustion } \\ \text { Fuel } \end{array} & \mathrm{kJ} / \mathrm{mol} \\ \hline \text { Nitroethane, } \mathrm{C}_{2} \mathrm{H}_{5} \mathrm{NO}_{2}(l) & 1.052 & -1368 \\ \text { Ethanol, } \mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}(l) & 0.789 & -1367 \\ \text { Methylhydrazine, } \mathrm{CH}_{6} \mathrm{~N}_{2}(l) & 0.874 & -1305 \end{array} $$

(a) Why are fats well suited for energy storage in the human body? (b) A particular chip snack food is composed of \(12 \%\) protein, \(14 \%\) fat, and the rest carbohydrate. What percentage of the calorie content of this food is fat? (c) How many grams of protein provide the same fuel value as \(25 \mathrm{~g}\) of fat?
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