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?

Consider this reaction occurring at 298 K: BaCO₃(s) ⇌ BaO(s) + CO₂(g) c. Can the reaction be made more spontaneous by an increase or decrease in temperature? If so, at what temperature is the partial pressure of carbon dioxide 1.0 atm?

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)

Calculate ΔG° at 298 K for these reactions and predict the effect on ΔG° of lowering the temperature.

a. NH₃(g) + HBr(g) → NH₄Br(s)

b. CaCO₃(s) → CaO(s) + CO₂(g)

c. CH₄(g) + 3 Cl₂(g) → CHCl₃(g) + 3 HCl(g) (ΔG°_f for CHCl₃(g) is -70.4 kJ/mol.)

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.

Dinitrogen tetroxide decomposes to nitrogen dioxide: N₂O₄(g) → 2 NO₂(g) ΔH°_rxn = 55.3 kJ At 298 K, a reaction vessel initially contains 0.100 atm of N₂O₄. When equilibrium is reached, 58% of the N₂O₄ has decomposed to NO₂. What percentage of N₂O₄ decomposes at 388 K? Assume that the initial pressure of N₂O₄ is the same (0.100 atm).

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

The Haber process is very important for agriculture because it converts N₂(g) from the atmosphere into bound nitrogen, which can be taken up and used by plants. The Haber process reaction is N₂(g) + 3 H₂(g) → 2 NH₃(g). The reaction is exothermic but is carried out at relatively high temperatures. Why?

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?

The solubility of AgCl(s) in water at 25 °C is 1.33⨉10^-5 mol/L and its ΔH° of solution is 65.7 kJ/mol. What is its solubility at 50.0 °C?