Concept explainers
Interpretation:
The Gibbs free energy and required change in enthalpy for a reaction system are to be calculated with given
Concept introduction:
Gibbs Free Energy can be defined as
Here,
When the change in entropy is negligible or zero, the equation changes to the expression:
Second law of thermodynamics tells about the spontaneity of a reaction and Gibbs free energy will tell in which direction the reaction is spontaneous.
It can be expressed mathematically as
Here,
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Check out a sample textbook solutionChapter 3 Solutions
Organic Chemistry, 12e Study Guide/Student Solutions Manual
- (28) The standard Gibbs free energy associated with the following reaction is -91.2 kJ: HCI (g) + NH3 (g) → NH,CI (s) What will be the value of AG,nn if the reaction takes place at 42.2°C, the partial pressure of HCI (g) is 0.788 atm and the partial pressure of NH3 (g) is 0.284 atm? (A) (B) -95.1 kl -90.7 kl (C) (D) (E) 3.93 kJ noltemol or ni lu bluos noinsou -79.5 kJ -87.3 kJarrow_forwardGiven : (a) BCl3(g) + 3H2O(l) →H3BO3(s) + 3HCl(g) ΔH = -112.5 kJ (b) B2H6(g) + 6H2O(l) →2H3BO3(s) + 6H2(g) ΔH = -493.4 kJ (c) 1/2H2(g) + 1/2Cl2(g) →HCl(g) ΔH = -92.3 kJ Calculate the value of ΔH for the reaction: B2H6(g) + 6Cl2(g) →2BCl3(g) + 6HCl(g) ΔH = ? Select one: a.-1476KJ b.-1376KJ c. -1576KJ d.-1576KJarrow_forwardState if each of the following processes is spontaneous, not spontaneous, or if additional information is needed to give an answer. Make sure that you detail whatadditional information you need in order to decide.(A) A process at constant temperature and pressure for which ∆S of the system ispositive.(B) A process for which ∆S is negative and ∆Ssurr is positive.(C) A process for which ∆S is negative and ∆Ssurr is zero.arrow_forward
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- Determine Δngasfor each of the following reactions:arrow_forwardWith a ΔΔGo of -550.23 kJ, calculate the equilibrium constant for the reaction at 25.0 oC.arrow_forward6. (a) How much does the free energy (kJ/mole) of 15 g of pure Cu change by adding 5 g of pure Zn at a temperature of 1100 degrees C? Assume an ideal solution, and that Go(Cu) = -1200 kJ/mole, and Go(Zn) = -2000 kJ/mole at this temperature. A(Cu) = 63.55, and A(Zn) = 65.39. b) By how much more does the system free energy change by adding 5 g of Ga to the mixture in part a)? A(Ga) = 69.7, and Go(Ga) = - 3000 kJ/mole. %3Darrow_forward
- Which statement is FALSE? (A) If a reaction is thermodynamically spontaneous it may occur slowly. (B) Activation energy is a kinetic quantity rather than a thermodynamic quantity. (C) If a reaction is thermodynamically spontaneous it may occur rapidly. (D) If a reaction is thermodynamically spontaneous, it must have a low activation energy. (E) If a reaction is thermodynamically nonspontaneous, it will not occur spontaneously.arrow_forward1. The depletion of ozone in the stratosphere can be summarized by this equation: 203(g) 302(g) O3(g) O2(g) AH°f 142.7 kJ/mol 0 So 239 J/K.mol 205 J/K-mol (i) Calculate AS° and AG° for this reaction. (ii) Calculate the equilibrium constant. (iii) Explain, in molecular terms, the sign of AS° for this equilibrium. (iv) What is the significance of your answers with respect to ozone depletion? (v) How would you expect the value of AG to change with increasing temperature? Explain.arrow_forwardThe equilibrium constant for a reaction carried out at 25 degrees celsius is 100. (a) if the reaction favorable or unfavorable? (b) what is the delta G prime (gibbs free energy ^prime) for the reaction?arrow_forward
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