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Chapter 2: Problem 5

\(\mathrm{SF}_{4}(g)+\mathrm{H}_{2} \mathrm{O}(l) \rightarrow \mathrm{SO}_{2}(g)+4 \mathrm{HF}(g) \Delta H=-828 \mathrm{kJ} / \mathrm{mol}\) Which of the following statements accurately describes the above reaction? (A) The entropy of the reactants exceeds that of the products. (B) \(\mathrm{H}_{2} \mathrm{O}(l)\) will always be the limiting reagent. (C) This reaction is never thermodynamically favored. (D) The temperature of the surroundings will increase as this reaction Progresses.

Short Answer

Expert verified
D. The temperature of the surroundings will increase as this reaction progresses.

Step by step solution

01

Identify the Enthalpy Change

The reaction is given to have an enthalpy change, \(\Delta H\), of -828 kJ/mol. This is negative, meaning that the reaction is exothermic and releases heat into the surroundings.
02

Assess Each Statement

Statement A: The entropy of reactants or products cannot be identified only based on the provided data. Statement B: The limiting reagent cannot be decided without knowing the amounts of the reactants involved. Statement C: Thermodynamic favorability of a reaction depends on a variety of factors including temperature, pressure, and entropy changes. Only knowing the enthalpy change is not sufficient to claim it's never thermodynamically favored. Statement D: As determined in Step 1, the reaction is an exothermic reaction, which means the reaction releases heat when it happens. This energy would likely result in an increase in the temperature of the surroundings, making this statement correct.

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Most popular questions from this chapter

\(\mathrm{NO}_{2}+\mathrm{O}_{3} \rightarrow \mathrm{NO}_{3}+\mathrm{O}_{2}\) \(\quad\) Slow \(\mathrm{NO}_{3}+\mathrm{NO}_{2} \rightarrow \mathrm{N}_{2} \mathrm{O}_{5}\) \(\quad\) Fast A proposed reaction mechanism for the reaction of nitrogen dioxide and ozone is detailed above. Which of the following is the rate law for the reaction? (A) Rate \(=k\left[\mathrm{NO}_{2}\right]\left[\mathrm{O}_{3}\right]\) (B) Rate \(=k\left[\mathrm{NO}_{3}\right]\left[\mathrm{NO}_{2}\right]\) (C) Rate \(=k\left[\mathrm{NO}_{2}\right]^{2}\left[\mathrm{O}_{3}\right]\) (D) Rate \(=k\left[\mathrm{NO}_{3}\right]\left[\mathrm{O}_{2}\right]\)

The enthalpy values for several reactions are as follows: (I) \(\mathrm{CH}_{4}(g)+\mathrm{H}_{2}(g) \rightarrow \mathrm{C}(s)+\mathrm{H}_{2} \mathrm{O}(g)\) \(\quad \Delta H=-131 \mathrm{kJ} / \mathrm{mol}_{\mathrm{rxn}}\) (II) \(\mathrm{CH}_{4}(g)+\mathrm{H}_{2} \mathrm{O}(g) \rightarrow 3 \mathrm{H}_{2}(g)+\mathrm{CO}(g)\) \(\quad \Delta H=206 \mathrm{kJ} / \mathrm{mol}_{\mathrm{rxn}}\) (III) \(\mathrm{CO}(g)+\mathrm{H}_{2} \mathrm{O}(g) \rightarrow \mathrm{CO}_{2}(g)+\mathrm{H}_{2}(g)\) \(\quad \Delta H=-41 \mathrm{kJ} / \mathrm{mol}_{\mathrm{rxn}}\) (IV) \(\mathrm{CH}_{4}(g)+2 \mathrm{O}_{2}(g) \rightarrow \mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(l)\) \(\quad \Delta H=-890 \mathrm{kJ} / \mathrm{mol}_{\mathrm{rxn}}\) In which of the reactions does the amount of energy released by the formation of bonds in the products exceed the amount of energy necessary to break the bonds of the reactants by the greatest amount? (A) Reaction I (B) Reaction II (C) Reaction III (D) Reaction IV

A sample of \(\mathrm{H}_{2} \mathrm{S}\) gas is placed in an evacuated, sealed container and heated until the following decomposition reaction occurs at \(1000 \mathrm{K} :\) $$2 \mathrm{H}_{2} \mathrm{S}(g) \rightarrow 2 \mathrm{H}_{2}(g)+\mathrm{S}_{2}(g) \qquad K_{\mathrm{c}}=1.0 \times 10^{-6}$$ If, at a given point in the reaction, the value for the reaction quotient \(Q\) is determined to be \(2.5 \times 10^{-8},\) which of the following is occurring? (A) The concentration of the reactant is decreasing while the concentration of the products is increasing. (B) The concentration of the reactant is increasing while the concentration of the products is decreasing. (C) The system has passed the equilibrium point, and the concentration of all species involved in the reaction will remain constant. (D) The concentrations of all species involved are changing at the same rate.

Which of the following best explains why the ionization of atoms can occur during photoelectron spectroscopy, even though ionization is not a thermodynamically favored process? (A) It is an exothermic process due to the release of energy as an electron is liberated from the Coulombic attraction holding it to the nucleus. (B) The entropy of the system increases due to the separation of the electron from its atom. (C) Energy contained in the light can be used to overcome the Coulombic attraction between electrons and the nucleus. (D) The products of the ionization are at a lower energy state than the reactants.

A sample of liquid butane \(\left(\mathrm{C}_{\mathrm{L}} \mathrm{H}_{10}\right)\) in a pressurized lighter is set up directly beneath an aluminum can, as show in the diagram above. The can contains 100.0 \(\mathrm{mL}\) of water, and when the butane is ignited the temperature of the water inside the can increases from \(25.0^{\circ} \mathrm{C}\) to \(82.3^{\circ} \mathrm{C}\) . The total mass of butane ignited is found to be 0.51 \(\mathrm{g}\) , the specific heat of water is \(4.18 \mathrm{J} / \mathrm{g} \cdot^{\circ} \mathrm{C},\) and the density of water is \(1.00 \mathrm{g} / \mathrm{mL} .\) (a) Write the balanced chemical equation for the combustion of one mole of butane in air. (i) How much heat did the water gain? (ii) What is the experimentally determined heat of combustion for (ii) Whane based on this experiment? Your answer should be in \(\mathrm{kJ} / \mathrm{mol}\) . (c) Given butane's density of 0.573 \(\mathrm{g} / \mathrm{mL}\) at \(25^{\circ} \mathrm{C},\) calculate how much heat would be emitted if 5.00 \(\mathrm{mL}\) of it were combusted at that temperature. (d) The overall combustion of butane is an exothermic reaction. Explain why this is, in terms of bond energies. (e) One of the major sources of error in this experiment comes from the heat that is aboorbed by the air. Why, then, might it not be a good ide to perform this experiment inside a sealed container to prevent the heat from leaving the system?
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