Organic Chemistry
6th Edition
ISBN: 9781936221349
Author: Marc Loudon, Jim Parise
Publisher: W. H. Freeman
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Chapter 3, Problem 3.26P
Interpretation Introduction
(a)
Interpretation:
The correct number corresponding to the blank is to be stated.
Concept introduction:
The product of natural log of equilibrium constant, gas constant and specific temperature gives the value of free energy for the reaction. Free energy of a reaction is expressed in
Interpretation Introduction
(b)
Interpretation:
The correct number corresponding to the blank is to be stated.
Concept introduction:
The product of natural log of equilibrium constant, gas constant and specific temperature gives the value of free energy for the reaction. Free energy of a reaction is expressed in
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A reaction has a standard free‑energy change of −18.20 kJ (−4.350 kcal mol−1). Calculate the equilibrium constant for the reaction at 25 °C.
Keq =
Which of the following statements is true?
Select one:
At equilibrium, K = 0.
If K > 1, the reaction is spontaneous in the reverse direction under standard conditions.
For an endothermic reaction, increasing the temperature will increase the value of K.
If K = 1×109, equilibrium favours the reactant side.
At equilibrium, the concentrations of the reactants are always equal to the concentrations of the products.
Consider the following reaction at 25 °C: 3 NiO(s) + 2 NH₃(g) → 3 Ni(s) + N₂(g) + 3 H₂O(g) Given the information in the table
a. calculate ∆H° for the reaction.
b. calculate ∆S° for the reaction.
c. Determine the standard free energy for the reaction at 25 °C.
d. Determine the value of the equilibrium constant at 25 °C.
e. Estimate the temperature at which this reaction would be at equilibrium assuming that enthalpy and entropy are independent of temperature.
f. Determine the value of ∆G assuming that a mixture contains 57.6 g of NiO, 182.3 g of Ni, 0.24 atm of NH₃, 8.54 atm of N₂ and 10.07 atm of H₂O.
Chapter 3 Solutions
Organic Chemistry
Ch. 3 - Prob. 3.1PCh. 3 - Prob. 3.2PCh. 3 - Prob. 3.3PCh. 3 - Prob. 3.4PCh. 3 - Prob. 3.5PCh. 3 - Prob. 3.6PCh. 3 - Prob. 3.7PCh. 3 - Prob. 3.8PCh. 3 - Prob. 3.9PCh. 3 - Prob. 3.10P
Ch. 3 - Prob. 3.11PCh. 3 - Prob. 3.12PCh. 3 - Prob. 3.13PCh. 3 - Prob. 3.14PCh. 3 - Prob. 3.15PCh. 3 - Prob. 3.16PCh. 3 - Prob. 3.17PCh. 3 - Prob. 3.18PCh. 3 - Prob. 3.19PCh. 3 - Prob. 3.20PCh. 3 - Prob. 3.21PCh. 3 - Prob. 3.22PCh. 3 - Prob. 3.24PCh. 3 - Prob. 3.25PCh. 3 - Prob. 3.26PCh. 3 - Prob. 3.27PCh. 3 - Prob. 3.28PCh. 3 - Prob. 3.29PCh. 3 - Prob. 3.30PCh. 3 - Prob. 3.31PCh. 3 - Prob. 3.32APCh. 3 - Prob. 3.33APCh. 3 - Prob. 3.34APCh. 3 - Prob. 3.35APCh. 3 - Prob. 3.36APCh. 3 - Prob. 3.37APCh. 3 - Prob. 3.38APCh. 3 - Prob. 3.39APCh. 3 - Prob. 3.40APCh. 3 - Prob. 3.41APCh. 3 - Prob. 3.42APCh. 3 - Prob. 3.43APCh. 3 - Prob. 3.44APCh. 3 - Prob. 3.45APCh. 3 - Prob. 3.46APCh. 3 - Prob. 3.47APCh. 3 - Prob. 3.48APCh. 3 - Prob. 3.49APCh. 3 - Prob. 3.50APCh. 3 - Prob. 3.51APCh. 3 - Prob. 3.52APCh. 3 - Prob. 3.53APCh. 3 - Prob. 3.54APCh. 3 - Prob. 3.55APCh. 3 - Prob. 3.56APCh. 3 - Prob. 3.57APCh. 3 - Prob. 3.58APCh. 3 - Prob. 3.59APCh. 3 - Prob. 3.60AP
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- What information can be determined from G for a reaction? Does one get the same information from G, the standard free energy change? G allows determination of the equilibrium constant K for a reaction. How? How can one estimate the value of K at temperatures other than 25C for a reaction? How can one estimate the temperature where K = 1 for a reaction? Do all reactions have a specific temperature where K = 1?arrow_forwardActually, the carbon in CO2(g) is thermodynamically unstable with respect to the carbon in calcium carbonate(limestone). Verify this by determining the standardGibbs free energy change for the reaction of lime,CaO(s), with CO2(g) to make CaCO3(s).arrow_forwardWhat is the relationship between the standard free energy change and the equilibrium constant of the reaction?arrow_forward
- Using the thermodynamic informationn, claculate the standard reaction free energy of the following chemical reaction: Fe2O3(s)+3H2(g)---> 2Fe(s)+3H2O(l)arrow_forwardthe equilibrium constant at a temperature of 25 °C is determined to be K=603500. What can be concluded from this? Pick one: a) Since the value of the equilibrium constant is large, the reaction is fast b) The equilibrium of the reaction favors the reaction. However, it is not possible to be sure whether it is worth making ammonia using this method, because the reaction can be slow c) The reaction is spontaneous, but a large part of the starting material remains unreacted d) both enthalpy and entropy terms are favorable for the reactionarrow_forwardThe acid dissociation constant for a weak acid HX at 25°C is 1.9 10–6. Calculate the free energy of formation for X–(aq) at 25°C. The standard free energies of HX(aq) and H+(aq) at 25°C are –245.4 kJ/mol and 0, respectively.arrow_forward
- 2b which determines whether a reaction is spontaneous. the net free energy change of the reaction or the activation energy of the reactionarrow_forwardThe standard free energy of formation, DGf°, of atomic oxygen is 230.1 kJ/mol. Determine the equilibrium constant for the following reaction at standard thermodynamic conditions. O2(g) ↔ 2O(g)arrow_forward1. Calculate the standard reaction free energy of the following chemical reaction:arrow_forward
- At 575 K, ∆G = -3.2 kJ/mol for the reaction A (g) → 2 B (g). If the partial pressures of A and B are 5.68 atm and 0.25 atm respectively, what is the standard free energy for this reaction at this temperature?arrow_forwardConsider the following reaction at 25 °C: 3 NiO(s) + 2 NH₃(g) → 3 Ni(s) + N₂(g) + 3 H₂O(g) a.Given the information in the table, calculate the delta So for the reaction. b.Given the information in the table, calculate the delta Ho for the reaction. c. Determine the standard free energy for the reaction at 25oC. d. Determine the value of the equilibrium constant at 25oC.arrow_forwardCalculate the standard Gibbs free energy of the reaction, ΔG∘rxn. The standard enthalpy of the reaction, ΔH∘rxn, is −44.2 kJ⋅mol−1. C2H4(g)= 68.4 H2O(l)= -237.1 C2H5OH(l)= -166.6arrow_forward
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