For the following acid-base reaction: H₂S(aq) + CN⁻(aq) ⇌ HS⁻(aq) + HCN(aq) ∆H° = -24.7 kJ/mol and ∆S° = -49.9 J/mol･K. If you mix 100 mL of 0.0450 M NaCN with 100 mL of 0.0450 M H₂S, after equilibrium is established at 25°C what will be the molar concentration of HCN?

Indicate which substance in the given pairs has the higher entropy value. Explain your choices.. (a) C2H5OH(l) or C3H7OH(l). (b) C2H5OH(l) or C2H5OH(g). (c) 2H(g) or H(g)

What determines Ssurr for a process? To calculate Ssurr at constant pressure and temperature, we use the following equation: Ssurr = H/T. Why does a minus sign appear in the equation, and why is Ssurr inversely proportional to temperature?

Elemental boron, in the form of thin fibers, can be made by reducing a boron halide with H2. BCl3(g) + 3/2 H2(g) B(s) + 3HCl(g) Calculate H, S, and G at 25 C for this reaction. Is the reaction predicted to be product favored at equilibrium at 25 C? If so, is it enthalpy driven or entropy driven?

The standard free energies of formation and the standard enthalpies of formation at 298 K for difluoroacetylene (C2F2) and hexafluorobenzene (C6F6) are Gfo(KJ/mol) Hfo(KJ/mol) C2F2(g) 191.2 241.3 Hexane 78.2 132.8 For the following reaction: C6F6(g)3C2F2(g) a. calculate S at 298 K. b. calculate K at 298 K. c. estimate K at 3000. K, assuming H and S do not depend on temperature.

Hydrogen gas and iodine vapor react to produce hydrogen iodide gas: H2(g)+I2(g)2HI(g) Calculate the free-energy change G for the following two conditions, at 25C. Which one is closer to equilibrium? Explain. a The partial pressures of H2(g), I2(g). and HI(g) are each 13 atm. b The partial pressures of H2(g) and I2(g) are each 13 atm; the partial pressure of HI(g) is 190 atm.

Given the following data at 25C 2NO(g)N2(g)+O2(g)K=1 10 30 2NO(g)+Br2(g)2NOBr(g)K=8 101 Calculate K for the formation of one mole of NOBr from its elements in the gaseous state.

In muscle cells under the condition of vigorous exercise, glucose is converted to lactic acid (lactate),CH3CHOHCOOH, by the chemical reaction C6H12O6 2 CH3CHOHCOOHrG = 197 kJ/mol (a) If all of the Gibbs free energy from this reaction wereused to convert ADP to ATP, calculate how many molesof ATP could be produced per mole of glucose. (b) The actual reaction involves the production of 3 molATP per mole of glucose. Calculate the rG for thisoverall reaction. (c) Is the overall reaction in part (b) reactant-favored orproduct-favored?

Explain how the entropy of the universe increases when an aluminum metal can is made from aluminum ore. Thefirst step is to extract the ore, which is primarily a formof A12O3, from the ground. After it is purified by freeingit from oxides of silicon and iron, aluminum oxide ischanged to the metal by an input of electrical energy. 2Al2O3(s)electricalenergy4Al(s)+3O2(g)

The decomposition of diamond to graphite [C(diamond) C(graphite)] is thermodynamically favored, but occurs slowly at room temperature. a. Use fG values from Appendix L to calculate rG and Keq for the reaction under standard conditions and 298.15 K. b. Use fH and S values from Appendix L to estimate rG and Keq for the reaction at 1000 K. Assume that enthalpy and entropy values are valid at these temperatures. Does heating shift the equilibrium toward the formation of diamond or graphite? c. Why is the formation of diamond favored at high pressures? d. The phase diagram shows that diamond is thermodynamically favored over graphite at 20,000 atmospheres pressure (about 2 GPa) at room temperature. Why is this conversion actually done at much higher temperatures and pressures?