(a)
Interpretation: The starting material or product which is favored at equilibrium is to be identified.
Concept introduction: The change in Gibbs free energy is represented by
If the
Answer to Problem 6.35P
The formation of starting material is favored at the given value of
Explanation of Solution
Given
The value of
The given value of
(a) The formation of starting material is favored at the given value of
(b)
Interpretation: The starting material or product which is favored at equilibrium is to be identified.
Concept introduction: The change in Gibbs free energy, enthalpy and entropy is represented by
The change in Gibbs free energy describes the spontaneity of the reaction. The change in enthalpy describes the relative bond strength in the substance, whereas the change in entropy describes the randomness in the system.
Answer to Problem 6.35P
The formation of the productis favored at the given value of
Explanation of Solution
Given:
The value of
The given value of
The formation of the product is favored at the given value of
(c)
Interpretation: The starting material or product which is favored at equilibrium is to be identified.
Concept introduction: The change in Gibbs free energy, enthalpy and entropy is represented by
The change in Gibbs free energy describes the spontaneity of the reaction. The change in enthalpy describes the relative bond strength in the substance, whereas the change in entropy describes the randomness in the system.
Answer to Problem 6.35P
The formation of the starting material is favoredat the given values of
Explanation of Solution
Given
The values of
The given values of
The formation of the starting material is favouredat the given values of
(d)
Interpretation: The starting material or product which is favored at equilibrium is to be identified.
Concept introduction: The change in Gibbs free energy is represented by
If the
Answer to Problem 6.35P
The formation of the productis favored at the given value of
Explanation of Solution
Given
The value of
The given value of
The formation of the product is favored at the given value of
(e)
Interpretation: The starting material or product which is favored at equilibrium is to be identified.
Concept introduction: The change in Gibbs free energy, enthalpy and entropy is represented by
The change in Gibbs free energy describes the spontaneity of the reaction. The change in enthalpy describes the relative bond strength in the substance, whereas the change in entropy describes the randomness in the system.
Answer to Problem 6.35P
The formation of the starting materialis favored at the given value of
Explanation of Solution
Given
The value of
The given value of
The formation of the starting material is favored at the given value of
(f)
Interpretation: The starting material or product which is favored at equilibrium is to be identified.
Concept introduction: The change in Gibbs free energy, enthalpy and entropy is represented by
The change in Gibbs free energy describes the spontaneity of the reaction. The change in enthalpy describes the relative bond strength in the substance, whereas the change in entropy describes the randomness in the system.
Answer to Problem 6.35P
The formation of the productis favored at the given value of
Explanation of Solution
Given
The value of
For the spontaneous reaction, the value of
The formation of the product is favored at the given value of
(g)
Interpretation: The starting material or product which isfavored at equilibrium is to be identified.
Concept introduction: The change in Gibbs free energy, enthalpy and entropy is represented by
The change in Gibbs free energy describes the spontaneity of the reaction. The change in enthalpy describes the relative bond strength in the substance, whereas the change in entropy describes the randomness in the system.
Answer to Problem 6.35P
The formation of the starting material is favored at the given value of
Explanation of Solution
Given
The value of
The value of
The formation of the starting material is favored at the given value of
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Chapter 6 Solutions
Organic Chemistry
- Complete each of these reactions by filling in the blanks. Predict whether each reaction is product-favored or reactant-favored, and explain your reasoning. (a) (aq)+HSO4(aq)HCN(aq)+SO42(aq) (b) H2S (aq) + H2O() H3O+(aq) + _____ (aq) (c) H(aq) + H2O() OH(aq) +_____ (g)arrow_forwardPlease don't provide handwriting solutionarrow_forwardHydrogen iodide dissociates according to the equation 2HI(g) <=> H2(g) + I2 (g). A 0.2 moles of gaseous hydrogen iodide was placed in a 200 ml flask. At equilibrium it was found that 20% of the HI had dissociated. What is the Keq or Kc value for the equilibrium system? a. 1/4 b. 1/8 c. 1/16 d. 1/64arrow_forward
- Given the Ke value for the following reaction at a particular temperature: SO₂ (g) + O₂ (g) = SO3 (9) K₂ = 1.24 What is the value of Ke for the new equilibrium below at the same temperature? 2 SO3 (g) 2 SO₂ (g) + O₂ (g) T 0.367 O 1.61 0.650 O 0.115arrow_forwardConsider the following system at equilibrium: CH4(g) + H2O(g) D CO (g) + 3H2 (g) ΔH° = +206 kJ. Which of the following changes will shift the equilibrium to the left? decreasing the pressure adding a catalyst adding methane increasing the temperature decreasing the volumearrow_forwardSuppose you have the following chemical reaction at equilibrium: N2H4 (1) + N2O4 (1) = N2 (g) + H2O (g) If this reaction releases heat, what direction will the equilibrium shift when: 1. the amount of N2 is decreased? 2. the heat of the system is increased? 3. an inert gas with pressure 3.00 atm is placed in the system? 4. the volume of the system is reduced? 5. a catalyst in the reaction is placed?arrow_forward
- This reaction has K = 2.3 * 10-18. Are the reactants or the products favored?arrow_forwardIn Which of the following is always TRUE for a reaction whose value of Kc is 4.4 × 10-18? A. The reaction occurs quickly. B. At equilibrium, the reaction mixture is product-favored. C. The reaction occurs slowly. D. At equilibrium, there are equal moles of reactants and products E. At equilibrium, the reaction mixture is reactant-favored.arrow_forwardHh.201.arrow_forward
- answer #5arrow_forwardGiven the following equilibrium: 2 NO + O2 ↔ 2 NO2 ΔH= -27 kJ/mol Increasing the temperature of this system will cause:arrow_forwardA. HC CH+ CH3CH₂ B. H₂C-CH₂ + HCC C. CH3CH3 + H₂C-CH HC C + CH3 CH3 H₂C-CH+ HC CH CH3CH₂ + H₂C-CH₂ Which reaction has the smallest equilibrium constant? Oreaction A O reaction B Oreaction C O All equilibrium constants are equal.arrow_forward
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