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Mobile App Problem 50
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 \(1000 \mathrm{K} :\) $$2 \mathrm{H}_{2} \mathrm{S}(g) \rightarrow 2 \mathrm{H}_{2}(g)+\mathrm{S}_{2}(g) \qquad K_{\mathrm{c}}=1.0 \times 10^{-6}$$ As the reaction progresses at a constant temperature of 1000 K, how does the value for the Gibbs free energy constant for the reaction change? (A) It stays constant. (B) It increases exponentially. (C) It increases linearly. (D) It decreases exponentially.
Problem 51
An unknown substance is found to have a high melting point. In addition, it is a poor conductor of electricity and does not dissolve in water. The substance most likely contains (A) ionic bonding (B) nonpolar covalent bonding (C) covalent network bonding (D) metallic bonding
Problem 52
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.
Problem 56
Atoms of four elements are examined: carbon, nitrogen, neon, and sulfur. Atoms of which element are most likely to form a structure with the formula \(\mathrm{XF}_{6}\) (where \(\mathrm{X}\) is one of the four atoms)? (A) Carbon (B) Nitrogen (C) Neon (D) Sulfur
Problem 59
\(\mathrm{NO}_{2}+\mathrm{O}_{3} \rightarrow \mathrm{NO}_{3}+\mathrm{O}_{2}\) \(\quad\) 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 \(=k\left[\mathrm{NO}_{3}\right]\left[\mathrm{O}_{2}\right]\)
