Does entropy increase or decrease in the following processes?

a. Polymeric complex carbohydrates are metabolized by the body, converted into smaller simple sugars.

Does entropy increase or decrease in the following processes?

c. 2 SO₂(g) + O₂(g) → 2 SO₃(g)

Do the following reactions favor reactants or products at equilibrium? Give relative concentrations at equilibrium.

a. Sucrose(aq) + H₂O(l) ⇌ Glucose(aq) + Fructose(aq) K = 1.4 × 10⁵

Do the following reactions favor reactants or products at equilibrium? Give relative concentrations at equilibrium.

c. Fe₂O₃(s) + 3 CO(g) ⇌ 2 Fe(s) + 3 CO₂(g) K (at 727 °C) = 24.2

The following diagrams represent two similar reactions that have achieved equilibrium:

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a. Write the expression for the equilibrium constant for each reaction.

The following diagrams represent two similar reactions that have achieved equilibrium:

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b. Calculate the value for the equilibrium constant for each reaction.

Is the yield of SO₃ at equilibrium favored by a higher or lower pressure? By a higher or lower temperature?

2 SO₂(g) + O₂ ⇌ 2 SO₃(g) ∆H = -47 kcal/mol

What effect do the listed changes have on the position of the equilibrium in the reaction of carbon with hydrogen?

C(s) + 2 H₂(g) ⇌ CH₄(g) ∆H = -18 kcal/mol (-75kJ/mol)

a. Increasing temperature

What effect do the listed changes have on the position of the equilibrium in the reaction of carbon with hydrogen?

C(s) + 2 H₂(g) ⇌ CH₄(g) ∆H = -18 kcal/mol (-75kJ/mol)

b. Increasing pressure by decreasing volume

What effect do the listed changes have on the position of the equilibrium in the reaction of carbon with hydrogen?

C(s) + 2 H₂(g) ⇌ CH₄(g) ∆H = -18 kcal/mol (-75kJ/mol)

c. Allowing CH₄ to escape continuously from the reaction vessel

Two curves are shown in the following energy diagram:

b. Which curve represents the spontaneous reaction, and which the nonspontaneous?

The following diagram portrays a reaction of the type A(s) → B(g) + C(g), where the different-colored spheres represent different molecular structures. Assume that the reaction has ∆H = +9.1 kcal/mol (+38.1 kJ/mol).

a. What is the sign of ∆S for the reaction?

The following diagram portrays a reaction of the type A(s) → B(g) + C(g), where the different-colored spheres represent different molecular structures. Assume that the reaction has ∆H = +9.1 kcal/mol (+38.1 kJ/mol).

b. Is the reaction likely to be spontaneous at all temperatures, nonspontaneous at all temperatures, or spontaneous at some but nonspontaneous at others?

Is the total enthalpy (H) of the reactants for an endothermic reaction greater than or less than the total enthalpy of the products?

The vaporization of Br₂ from the liquid to the gas state requires 7.4 kcal/mol (31.0 kJ/mol).

a. What is the sign of ∆H for this process? Write a reaction showing heat as a product or reactant.

The vaporization of Br₂ from the liquid to the gas state requires 7.4 kcal/mol (31.0 kJ/mol).

c. How many kilojoules are needed to evaporate 82 g of Br₂?

Acetylene (H–C≡C–H) is the fuel used in welding torches.

b. Estimate ∆H for this reaction (in kJ/mol) using the bond energies listed in Table 7.1.

Nitrogen in air reacts at high temperatures to form NO₂ according to the following reaction: N₂ + 2 O₂ → 2 NO₂

b. Estimate ∆H for this reaction (in kcal and kJ) using the bond energies from Table 7.1.

Glucose, also known as "blood sugar" when measured in blood, has the formula C₆H₁₂O₆.

a. Write the equation for the combustion of glucose with O₂ to give CO₂ and H₂O.

Glucose, also known as "blood sugar" when measured in blood, has the formula C₆H₁₂O₆.

c. What is the minimum amount of energy (in kJ) a plant must absorb to produce 15.0 g of glucose?

Which of the following processes results in an increase in entropy of the system?

a. A drop of ink spreading out when it is placed in water

b. Steam condensing into drops on windows

c. Constructing a building from loose bricks

For each of the following processes, specify whether entropy increases or decreases. Explain each of your answers.

a. Assembling a jigsaw puzzle

What two factors affect the spontaneity of a reaction?

What is the difference between an exothermic reaction and an exergonic reaction?

Under what conditions might a reaction be endothermic but exergonic? Explain.

For the reaction

$NaCl\left(s\right)\stackrel{water}{\to }N{a}^{+}\left(aq\right)+C{l}^{\text{–}}\left(aq\right),\Delta H=\text{+1 kcal/mol (+4.184 kJ/mol)}$

b. Does entropy increase or decrease in this process?

For the reaction 2 Hg(l) + O₂(g) → 2 HgO(s), ∆H = –43 kcal/mol (–180 kJ/mol).

a. Does entropy increase or decrease in this process? Explain.

For the reaction 2 Hg(l) + O₂(g) → 2 HgO(s), ∆H = –43 kcal/mol (–180 kJ/mol).

b. Under what conditions would you expect this process to be spontaneous?

The following reaction is used in the industrial synthesis of polyvinyl chloride (PVC) polymer:

Cl₂(g) + H₂C=CH₂(g) → ClCH₂CH₂Cl(l) ∆H = –52 kcal/mol (–218 kJ/mol)

a. Is ∆S positive or negative for this process?