Determine the sign of ΔS_sys for each process. b. water freezing

Nitrogen dioxide, a pollutant in the atmosphere, can combine with water to form nitric acid. One of the possible reactions is shown here. Calculate ΔG° and K_p for this reaction at 25 °C and comment on the spontaneity of the reaction. 3 NO₂(g) + H₂O(l)→ 2 HNO₃(aq) + NO(g)

Ethene (C₂H₄) can be halogenated by the reaction: C₂H₄(g) + X₂(g) → C₂H₄X₂(g) where X₂ can be Cl₂, Br₂, or I₂. Use the thermodynamic data given to calculate ΔH°, ΔS°, ΔG°, and Kp for the halogenation reaction by each of the three halogens at 25 °C. Which reaction is most spontaneous? Least spontaneous? What is the main factor responsible for the difference in the spontaneity of the three reactions? Does higher temperature make the reactions more spontaneous or less spontaneous?

Compound ΔH°_f (kJ/mol) S° (J/mol·K)

C₂H₄Cl₂(g) -129.7 308.0

C₂H₄Br₂(g) +38.3 330.6

C₂H₄I₂(g) +66.5 347.8

H₂ reacts with the halogens (X₂) according to the reaction: H₂(g) + X₂(g) → 2 HX(g) where X₂ can be Cl₂, Br₂, or I₂. Use the thermodynamic data in Appendix IIB to calculate ΔH°, ΔS°, ΔG°, and K_p for the reaction between hydrogen and each of the three halogens. Which reaction is most spontaneous? Least spontaneous? What is the main factor responsible for the difference in the spontaneity of the three reactions? Does higher temperature make the reactions more spontaneous or less spontaneous?

Consider this reaction occurring at 298 K: N₂O(g) + NO₂(g) ⇌ 3 NO(g) a. Show that the reaction is not spontaneous under standard conditions by calculating ΔG°_rxn.

Consider this reaction occurring at 298 K: N₂O(g) + NO₂(g) ⇌ 3 NO(g) b. If a reaction mixture contains only N₂O and NO₂ at partial pressures of 1.0 atm each, the reaction will be spontaneous until some NO forms in the mixture. What maximum partial pressure of NO builds up before the reaction ceases to be spontaneous?

Consider this reaction occurring at 298 K: N₂O(g) + NO₂(g) ⇌ 3 NO(g) c. Can the reaction be made more spontaneous by an increase or decrease in temperature? If so, what temperature is required to make the reaction spontaneous under standard conditions?

Consider this reaction occurring at 298 K: BaCO₃(s) ⇌ BaO(s) + CO₂(g) a. Show that the reaction is not spontaneous under standard conditions by calculating ΔG°_rxn.

Consider this reaction occurring at 298 K: BaCO₃(s) ⇌ BaO(s) + CO₂( g) b. If BaCO₃ is placed in an evacuated flask, what is the partial pressure of CO₂ when the reaction reaches equilibrium?

Living organisms use energy from the metabolism of food to create an energy-rich molecule called adenosine triphosphate (ATP). The ATP acts as an energy source for a variety of reactions that the living organism must carry out to survive. ATP provides energy through its hydrolysis, which can be symbolized as follows: ATP(aq) + H₂O(l) → ADP(aq) + P_i(aq) ΔGrxn ° = -30.5 kJ where ADP represents adenosine diphosphate and Pi represents an inorganic phosphate group (such as HPO₄^2-). a. Calculate the equilibrium constant, K, for the given reaction at 298 K.

Living organisms use energy from the metabolism of food to create an energy-rich molecule called adenosine triphosphate (ATP). The ATP acts as an energy source for a variety of reactions that the living organism must carry out to survive. ATP provides energy through its hydrolysis, which can be symbolized as follows: ATP(aq) + H₂O(l) → ADP(aq) + P_i(aq) ΔG°_rxn = -30.5 kJ where ADP represents adenosine diphosphate and P_i represents an inorganic phosphate group (such as HPO₄^2-). b. The free energy obtained from the oxidation (reaction with oxygen) of glucose (C₆H₁₂O₆) to form carbon dioxide and water can be used to re-form ATP by driving the given reaction in reverse. Calculate the standard free energy change for the oxidation of glucose and estimate the maximum number of moles of ATP that can be formed by the oxidation of one mole of glucose.

These reactions are important in catalytic converters in automobiles. Calculate ΔG° for each at 298 K. Predict the effect of increasing temperature on the magnitude of ΔG°.

a. 2 CO(g) + 2 NO(g) → N₂(g) + 2 CO₂(g)

b. 5 H₂(g) + 2 NO(g) → 2 NH₃(g) + 2 H₂O(g)

c. 2 H₂(g) + 2 NO(g) → N₂(g) + 2 H₂O(g)

d. 2 NH₃(g) + 2 O₂(g) → N₂O(g) + 3 H₂O(g)

All the oxides of nitrogen have positive values of ΔG°_f at 298 K, but only one common oxide of nitrogen has a positive ΔS°_f. Identify that oxide of nitrogen without reference to thermodynamic data and explain.

The values of ΔG°_f for the hydrogen halides become less negative with increasing atomic number. The ΔG°_f of HI is slightly positive. However, the trend in ΔS°_f is to become more positive with increasing atomic number. Explain.

Consider the reaction X₂(g) → 2X(g). When a vessel initially containing 755 torr of X2 comes to equilibrium at 298 K, the equilibrium partial pressure of X is 103 torr. The same reaction is repeated with an initial partial pressure of 748 torr of X₂ at 755 K; the equilibrium partial pressure of X is 532 torr. Find ΔH° for the reaction.

Indicate and explain the sign of ΔS_univ for each process. a. 2 H₂(g) + O₂(g) → 2 H₂O (l) at 298 K.

A metal salt with the formula MCl₂ crystallizes from water to form a solid with the composition MCl₂ • 6 H₂O. The equilibrium vapor pressure of water above this solid at 298 K is 18.3 mmHg. What is the value of ΔG for the reaction MCl₂ • 6 H₂O(s) ⇌ MCl₂(s) + 6 H₂O(g) when the pressure of water vapor is 18.3 mmHg? When the pressure of water vapor is 760 mmHg?

Determine the minimum concentration of the precipitating agent on the right to cause precipitation of the cation from the solution on the left. a. 0.035 M Ba(NO₃)₂; NaF