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Chapter 17: Problem 4

What types of experiments can be carried out to determine whether a reaction is spontaneous? Does spontaneity have any relationship to the final equilibrium position of a reaction? Explain.

Short Answer

Expert verified
To determine whether a reaction is spontaneous, experiments can involve observation, measuring temperature changes, and calculating the change in Gibbs free energy (螖G) from experimental measurements. The spontaneity of a reaction is not directly related to its final equilibrium position. However, spontaneous reactions tend to move towards equilibrium, where 螖G becomes zero. The reaction may reach equilibrium before all reactants are converted to products.

Step by step solution

01

Understanding Spontaneity

Spontaneity in chemical reactions refers to whether a reaction will occur without the input of external energy. Spontaneous reactions are typically driven by the decrease in enthalpy (heat content) and/or an increase in entropy (disorder) of the system.
02

Gibbs Free Energy and Spontaneity

The spontaneity of a reaction can usually be determined by calculating the change in Gibbs free energy (螖G). The equation for 螖G is given by: 螖G = 螖H - T螖S where 螖H is the change in enthalpy, T is the temperature in kelvin, and 螖S is the change in entropy. If 螖G is negative, the reaction is spontaneous. If 螖G is positive, the reaction is non-spontaneous. If 螖G is zero, the reaction is in equilibrium.
03

Experimental Methods for Determining Spontaneity

There are several ways to experimentally determine if a reaction is spontaneous: 1. Observation: If a reaction happens without needing an external energy source, it's most likely spontaneous. 2. Measuring temperature changes: If the reaction is exothermic (releases heat), it is more likely to be spontaneous. Conversely, if the reaction is endothermic (absorbs heat), it may not be spontaneous. 3. Calculating 螖G from experimental measurements: Using experimental data to determine 螖H and 螖S, the value of 螖G can be calculated. If 螖G is negative, the reaction is spontaneous.
04

Relationship between Spontaneity and Equilibrium

The final equilibrium position of a reaction is not directly determined by the spontaneity of the reaction. However, there is a connection between the two, as spontaneous reactions tend to move towards equilibrium. At equilibrium, the forward and reverse reactions occur at the same rate, and 螖G becomes zero. Keep in mind that a spontaneous reaction doesn't necessarily imply that the reaction will go to completion, as it may reach equilibrium before all reactants are converted to products.

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Most popular questions from this chapter

The Ostwald process for the commercial production of nitric acid involves three steps: a. Calculate \(\Delta H^{\circ}, \Delta S^{\circ}, \Delta G^{\circ}\), and \(K\) (at \(298 \mathrm{~K}\) ) for each of the three steps in the Ostwald process (see Appendix 4 ). b. Calculate the equilibrium constant for the first step at \(825^{\circ} \mathrm{C}\), assuming \(\Delta H^{\circ}\) and \(\Delta S^{\circ}\) do not depend on temperature. c. Is there a thermodynamic reason for the high temperature in the first step, assuming standard conditions?

Using data from Appendix 4, calculate \(\Delta H^{\circ}, \Delta G^{\circ}\), and \(K\) (at 298 K) for the production of ozone from oxygen: $$3 \mathrm{O}_{2}(g) \rightleftharpoons 2 \mathrm{O}_{3}(g)$$ At \(30 \mathrm{~km}\) above the surface of the earth, the temperature is about 230\. \(\mathrm{K}\) and the partial pressure of oxygen is about \(1.0 \times 10^{-3}\) atm. Estimate the partial pressure of ozone in equilibrium with oxygen at \(30 \mathrm{~km}\) above the earth's surface. Is it reasonable to assume that the equilibrium between oxygen and ozone is maintained under these conditions? Explain.

For ammonia \(\left(\mathrm{NH}_{3}\right.\) ), the enthalpy of fusion is \(5.65 \mathrm{~kJ} / \mathrm{mol}\) and the entropy of fusion is \(28.9 \mathrm{~J} / \mathrm{K} \cdot \mathrm{mol}\). a. Will \(\mathrm{NH}_{3}(s)\) spontaneously melt at \(200 . \mathrm{K}\) ? b. What is the approximate melting point of ammonia?

Consider the reaction $$\mathrm{H}_{2}(g)+\mathrm{Br}_{2}(g) \rightleftharpoons 2 \mathrm{HBr}(g)$$ where \(\Delta H^{\circ}=-103.8 \mathrm{~kJ} / \mathrm{mol} .\) In a particular experiment, equal moles of \(\mathrm{H}_{2}(\mathrm{~g})\) at \(1.00 \mathrm{~atm}\) and \(\mathrm{Br}_{2}(\mathrm{~g})\) at \(1.00 \mathrm{~atm}\) were mixed in a \(1.00\) -L flask at \(25^{\circ} \mathrm{C}\) and allowed to reach equilibrium. Then the molecules of \(\mathrm{H}_{2}\) at equilibrium were counted using a very sensitive technique, and \(1.10 \times 10^{13}\) molecules were found. For this reaction, calculate the values of \(K, \Delta G^{\circ}\), and \(\Delta S^{\circ}\).

Consider the reactions $$\begin{aligned}\mathrm{Ni}^{2+}(a q)+6 \mathrm{NH}_{3}(a q) & \longrightarrow \mathrm{Ni}\left(\mathrm{NH}_{3}\right)_{6}^{2+}(a q) \\ \mathrm{Ni}^{2+}(a q)+3 \mathrm{en}(a q) & \longrightarrow \mathrm{Ni}(\mathrm{en})_{3}^{2+}(a q)\end{aligned}$$ where $$\text { en }=\mathrm{H}_{2} \mathrm{~N}-\mathrm{CH}_{2}-\mathrm{CH}_{2}-\mathrm{NH}_{2}$$ The \(\Delta H\) values for the two reactions are quite similar, yet \(K_{\text {reaction } 2}>K_{\text {reaction } 1 .}\) Explain.
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